02. solution and colligative properties

28Solution And Colligative Properties

MH- CET- (CHEMISTRY)

02. Solution And Colligative Properties

Solution: A solution is a homogeneous mixture of two or more non reacting substances on molecular level.

Solute and Solvent: The contituent of the mixture present in a smaller amount is called Solute and the onepresent in a larger amount is called the solvent.

S.N. Types of solution State of State of Example

solute solvent

(A) Gaseous Solution

01 Gas in gas Gas Gas Air, mixture of N2 and O

2

02 Liquid in gas Gas Gas Evaporation ofliquids, water vapors in air

03 Solid in gas Solid Gas Smoke, evaporation of camphor.

(B) Liquid Solution

04 Gas in liquid Gas Liquid Oxyen in water, CO2 in water (carbonated drinks)

05 Liquid in liquid Liquid Liquid Ethyl alcohol in water, mixture of two miscible liquids

06 Solid in liquid Solid Liquid Sugar, salt solution.

(C) Solid solution

07 Gas in solid Gas Solid Adsorption of H2 by Nickel.

08 Liquid in solid Liquid Solid Mercury in silver (Hg-Ag)(Amalgum).

09 Solid in solid Solid Solid Metal alloys, Carbon in iron (steel).

Notes: The solution: (1) liquid in gas (2) Solid ingas not possible because they do not formhomogenous mixture.

(B) On basis of on of components:

1. Binary solution: Asolution containing twocomponents i.e. solute and solvent.

2. Ternery solution: Asolution containing fourcomponents i.e. 'solute and solvent.

3. Quaternary solution: Asolution containingfour components i.e. solute and solvent.

(C) On the basis of strength :

1. Dilute solution: A solution containing arelatively low concentration solute is calleddilute solution.

2. Concentrated solution: A solution containingrelatively high concentration is calledconcentrated solution.

3. Unsaturated solution: Solution which candissolved some more solute at giventemperature is called unsaturated solution.

4. Saturated solution: Solutionwhich containsmaximumamount ofsolutethat canbedissolvedin given amount of solvent at

particulartemperature calledsaturated solution.Thus in saturated solution dynamic equilibriumexists between solid solute and dissolvedsolute.

5. Super saturated solution: A solutioncontaining large amount of solute than thatrequired for saturation of a given amount ofsolvent at a particular temperature is calledsuper saturated solution.

(D) On the basis of solvent:

1. Aqueous solution: A solution in which watersolvents is called aqueous solution.

2. Non aqueous solution: Asolution in whichsolvent is other than water is called nonaqueous solution.

Concentration of a solution:

The amount of solute present in a given amountof solution is called concentration of a solution.

Ways of expressing concentration:

There are several ways of expressingconcentration of a solution

(a) Percentage by mass

(b) Mole fraction

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(c) Molarity

(d) Molality

Soluyion and Colligative Properties

2

1 2

V%(V / V) 100

V V

Changes –

Name Symbol Definition Formula Effect of Unit

temperature

Mass percent %(W/W) Parts of solute (W2) present

in 100 parts of solution (1).

Both parts in terms of mass

or weight

Volume percent %(VN) Parts (Volume) of solute

present in 100 parts

(volume) of solution.

Both parts in terms of

volume in same units.

Normality N Number of gram Changes eq. dm–3

equivalents of solute in

one dm3 of solution

Molarity M Number of moles of solute Changes mol dm–3

in one dm3 of solution

Molality m Number of moles of solute No mol kg-1

in one kg solvent (1000g).

Mole X Ratio of the number of No –

moles of one component

(solvent or solute) to the

total number of moles total

of all components in

solution.

Formality F Number of gram formula of Changes mol dm-3

solute in one dm3 of solution

Parts per ppm Parts of solute in one – ppm

million million parts

of solution (in same unit)

Massor volumeofcomponent Ain kg

FTotalmass(or volume)of solution in kg

3

Massof solutein gmF

gmformulaVin dmmassofof solutionsolute

1 21 2

1 2 1

n nX ,X

n n n n

Massof soluteingm

mMassof

Molar mass solventinof solute kg

3

Massof soluteingmN

V ofGrammolar solutionmassof soluteindm

W2%(W / W) 100W W1 2

Note: Wl ,W

2 and n

1 ,n

2 be the mass the number

of moles of solvent and solute respectively.

Colligative properties: (Greek, colligtuscollectedtogether): A property which depends on thenumber of particles in solution and not in way onthe size or chemical nature of particles is calledcolligative property.

Types of colligative properties:

1. Relative lowering of the vapour pressure.

2. Elevation in the boiling point

3. Depression in the freezing point

4. Osmotic pressure

Vapour pressure of solution:

The pressure exerted by the vapours, whenvapours are in equilibrium with solution, at aparticular temperature is called vapour pressureof solution.

Colligative properties:

(I) Lowering of vapour pressure of solvent:

The difference between vapour pressure of puresolvent (P

0) and solution (p) is called lowering of





vapour pressure of solvent. It is not colligativeproperty.

Expression: Lowering of vapour pressure

= 01p p

Raoult's law for partial vapour pressure:

At a given temperature, for a solution of volatileliquids, the partial vapour pressure of eachcomponent is equal to the product of vapourpressure of the pure component and its mole

fraction in the solution. 0 01 1 2 2p p X p X

Raoult's law for solution containing

nonvolatile solute:The vapour pressure ofsolution containing non-volatile solute is directlyproportional to the mole fraction of the solvent.Relative lowering in vapour pressure: Theratio of lowering of vapour pressure of solutioncontaining non-volatile solute to the vapourpressure ofpure solvent is called relative loweringof vapour pressure.

Expression:

01

01

p pX

p

where 0

1(p p) is

called lowering of vapour pressure and

01

01

P P

P

is called relative lowering of vapour pressure. ismole fraction of non volatile soluter.

Limitations of Raoult's law: It is not applicable

1. Concentrated solution

2. Volatile solute

3. Dissociation

4. Association

Determination of molar mass:

Relative lowering of a vapour pressure isdetermined by Ostwald and Walker's dynamicmethod.

(Gas saturation method).

Calculation: Molar mass of non-volatile solute

M2is calculated as

01 2 1

01 2 2

P P W M

P M M

(II) Boiling point elevation:(Ebullioscopy):

Boiling point: The temperature at which thevapour pressure of liquid is equal to theatmospheric pressure (1 atm pressure = 760 mm)is called boiling point ofliquid, It is not colligativeproperty.

Boiling point elevationfc ( Tb):

The increase in the boiling point of pure solventwhen a non volatile solute dissolved in it, is calledelevation of boiling point. It is colligative property.

Expression: If T0 be the boiling point ofthe pureliquid (solvent) and 'T' be boiling point of the

solution then, 0b 1T p p

Mole elevation constant or boiling point

elevation constant or Ebulliscopic constant

of the solvent (Kb) : The elevation in boiling

point when the molality of the solution is unity(i.e. 1mole of solute is dissolved in 1kg (lOOg)ofthe solvent.

Expression:

(i) Tb molality T

b = K

b × molality

(ii) If the molality is one, then Kb = T

b.

Unit of Kb: The Unit of K

b are either, Degree/

molality i.e. Km-1 or cm -1or K kg mol-1.

Determination of Molar mass: Molar mass ofsolute from the elevation in boiling point isdetermined by Landsberger and Walker's method[Ebullioscipic method]

Calculation: Molar mass of non-volatile solute

b 22

b 1

K WM

T W

kg mol-1

ORb 2

2

b 1

K W 1000M

T W

gram mol-1

Where W2be the mass of non-volatile solute in

kg, W1mass of solvent in kg and M

2 and M

1is the

solute and solvent in kg mol-1

(III) Depression in Freezing Point (Cryoscopy)

Freezing point:

The temperature at which vapour pressure ofitsliquid is equal to the vapour pressure of tiiecorresponding solid is called freezing point. It isnot colligative property. Depression in freezingpoint: The decrease in temperature ofthe solventwhen solute is dissolved in it, is called depressionin freezing point.

Expression: If To be the freezing point of thepure liquid (solvent) and 'T' be the freezing pointof the solution then

Tf= TTo- T

Molal depression constant (Cryosco s:ric

constant, Kf): Tfie depression in freezing point

for 1 molal solution i.e. a solution in which 1 gmmole of solute is dissolved irl 1 kg (1000g) ofsolvent is called molal depression constant or





cryoscopic constant.

Expression:

(i) fT molality f fT K molality

(ii) If the molality is one, then Kf= T

f

Units of Kf : The units of Kfare either, Degree/

molality i.e. Km-1 or °Cm–1 or Kkg mol–1

Determination of molar mass :

Molar mass ofnon-volatile solute from depressionin freezing point is determined by Beckmann'smethod.

Calculation: Molar mass of non-volatile soluteM

2 is calculated as

f 22

f 1

K WM

T W

kg mol –1

OR f 22

f 1

K W 1000M

T W

gram mol–1

Keep in mind:

Use of ethylene glycol as antifreeze: To avoidthe freezing ofwater, a solution of ethylene glycolin water is used in radiator. This solution hasfreezing point below 0°C.Thus freezing point ofwater can be lowered.

(IV) Osmosis and Osmotic pressure: Osmosis

(Greek - Topush): (Abbe Nollet in 1748)The spontaneous flow of solvent molecules formthe solution of region of lower concentration tothe region of higher concentration through asemipermeable membrane is called osmosis.

Exo-Osmosis: When the membrane permits thesolvent molecules to come out through themembrane is called exo osmosis, Ex. : If we putgrapes in concentrated NaCl solution, the grapesshrink.

Endo-Osmosis: When the membrane permi thesolvent molecules to enter inside through themembrane is called endo-osrnosis. Ex. : If wekept grapes in pure water, the grapes swells.Semipermeable membrane (SPM) Amembranewhich allows only solvent molecules and not thesolute molecules to pass through it, is calledsemipermeable membrane.

(a) Natural semipermedable membrane : Thenaturally occuring semipermeable membranes areparchemnt and cellophane bladder of goat or pig.

(b) Artificial sempermeable membrane: It isprepared in laboratory by mixing of aqueoussolution of potassium ferrocyanide and coppersulphate in a porous pot. The gelationous

percipitate of copper ferrocyanide fills in the2 CuSO

4 + K

4[Fe (CN)

6]

Copper Sulphate

Potassium Ferrocyanide

Cu2[Fe (CN)

6 + 2 K

2SO

4

SPM Potassium

Sulphate

Osmotic Pressure ︵︶ :

The excess of hydrostatic pressure which isdeveloped as a result of osmosis is called osmoticpressure. OR

The excess pressure which must be applied toprevent the passing of solvent through asemipermeable membrane is called osmoticpressure. OR

Osmotic pressure is.the excess of pressure whichmust be applied to a solution in order to increasethe vapour pressure of the solution untill itbecomes equal to the vapour pressure of solvent.Measurement of osmotic pressure: Thevarious methods employed for determination are:

(i) Pfeffer's method.

(ii) Morse and Frazer's method.

(iii) Berkeley and Hartley's method (commonmethod).

Calculation:

Osmotic pressure = h d g

Where, h = height of column, d = density ofsolution in the column and g = acceleration dueto gravity.

Application: From the measurement of osmoticpressure, the molecular mass of proteins, polymersand macromolecules can be determined.

Laws of Osmotic pressure:

1. van't Hoff's theory of dilute solutions:

(i) Bolye's van't Hoff law:

(a) C ....(i)

(b) n 1

CV V

(n = 1 mole) ...(ii)

Thus from equation (1) and (2) 1

V

V = constant

(ii) Charle's-van't Hofflaw:

(i) T T

= Constant

(iii) van't Hoff solution equation:





V = nRT (For n mole of solute)

Where R = Gas constant.

Determination of molecular mass of solute

from osmotic pressure:

By van't Hoff solution equation.

2 2

2

n W RTRT,

V M V

or 2

W RTM

V

Where, n

2 = Number of moles of solute

Van't Haff-Avogadro's law:

The volume (V) of a solution containing 1 mole

of solute at 273 K (oC)is 22.6 dm3 when theosmotic pressure is 1 atm (1.01325 ×105 pa)

Expression: If 1 2 and V1=V

2.The

according to Avagadro's law, n1= n

2

Abnormal molecular masses and solutions

of electrolytes:

1. Association of solute molecules: Due toassociation, there is decrease in the numberof solute particles on dissolving in a solventand thus decreases the values of colligativeproperties. Hence higher values are obtainedfor the molecular mass of solutes ascompared to the normal values.

2. Dissociation of solute molecules: Due todissociation the number of solute particlesin solution is more than the expected valuei.e. these solutions give higher values ofcolligative properties. The values ofcolligative properties are inverselypropertional to molecular masess, hence thecalculated values of molar masses for suchsubstances will be less than the normalvalues.

Explanation:

1. When i < 1 association occurs andtheoretical molar mass is less thancalculated mass from colligative property.

2. When i > 1 dissociation occurs andtheoretical molecular mass is more thancalculated mass from colligative property.

3. When i = 1, than solute does not undergoassociation or dissociation in the solvent.Solubilities of different solutions :

1. Solutions of gases in liquids:

Solubility of gases in liquids depends upon:

(i) Nature of gas (ii) Nature of the solvent

(iii) Temperature (iv) Pressure

(i) Nature of gas

(a) Gases which interact with the solvent or ionisein solutions have high solubility

(NH3 and HCl)

(b) Gases which do not interact with the water(H

2, O

2, N

2) are less soluble.

ii) Nature of solvent: Polar gases dissolvemore in polar solvent than non-polar solvent(like dissolves like)

iii) Temperature: Solubility of a gas in liquiddecreases with rise in temperature.

iv) Pressure: Solubility of a gas in liquidincreases with increase in pressure.

Henry's law (Relation between Sand P):

At constant temperature the quantity of gas inliquid solvent is proportional to the pressure ofthe gas over the solution

Expression: S P S = KP

Where 'S' solubility gas dissolved in a givenvolume of a solvent at constan, temperature'K' = Henry's constant

Henry constant (K):

Solubility of gas in mol dm–3 at 1 atmospherepressure at reference temperature is called HenryConstant.

When P = latm S = K

Application of Henry's law:

(i) In the production of carbonated drink

(ii) In deep sea driving

(iii) In the function of lungs.

(iv) In climbers or people living high altitutes.

2. Solution of solids in liquids:

Solubility of solids in liquid depends upon:

(a) Nature of Solute and solvent (Like

dissolves like):

(i) Polar solutes dissolve easily in polar solvent.Ex [NaCl (Polar) dissolves in water (Polar).

(ii) Polar solute does not dissolve in non-polarsolvent. [NaCl (Polar)] does not dissolve inbenzene (non-solvent).

Note: Sugar (non polar) dissolves in water. Herethe disolution is due to hydrogen bonding thatoccurs between water and sugar molecules.

(b) Effect of temperature on solubility:

(i) If the enthalpy of the solution is positive(Endothermic compound) the increase intemperature favours the solubility Ex.

KNO3,NaNO

3,AgNO

3, KI





(ii) If the enthalpy of the solution is negative(Endothermic compound) the increase intemperature decrease the solubility Ex.

CaCrO4, CaSO

4, (CH

3COO)

2 Ca

Solid solution (solid in solid) :

A solution of two or more elements containing only metals and nonmetals is called Alloy or soil solution.

Sr. No. Name of Alloy Constituents (metals) Property Uses

1. Duralium Al + Cu + Mg + Mn Light and strong In construction of air crafts

2. Aluminium AI + Cu + Light and strong In construction of air crafts

Bronze small amount of Mn

3. Babbit metal Sb + Sn + Cu Autofriction In machine bearing

4. Bronze Cu + Ni Hard Hardening agent

5. Stainless steel Fe + Cr + Ni Resistant to In cutlery

corrosion

6. Spiegeleisen 5 to 20% Mn in Fe Hard In manufacturing rails safes and

heavy machinery

7. Ferromaganeous Mn(70 to 80%) In making electrical and

+ Fe (20 to 30%) heavy machinery

8. Manganin Mn + Fe + Cu + Ni Zero temperature In making electrical measurements

Cu(84%) + Mn coefficient

(12%) + Ni (4%)

Van't Hoff factor (i) (1886): In order to accountfor the extent of association or dissociation ofsubstances, van't Hoffintroduced a factor 'i''called van't Hofffactor.

Expression: 'i'can be defined as the ratio ofobserved and theoretical value of colligativeproperty. Observed colligative property

(i) Observedcolligative property

Theoreticalcolligativepropertyi

= Experimetnalcolligativeproperty

Normalvalueof thesameproperty

ii) obs obs f obs b obs

theor theor f theor b theor

( P) ( T ) ( T )

( P) ( T ) ( T )

i

iii) But C.P n

Observed number of particles

Theoretica number of particlesi

iv)1

C.P.Molarmass

Theoreticalmolar massof solute

Observed molar massof solutei

Degree of dissociation : Fraction of the

total number ofmoles ofsubstance that undergodissociation at equlibrium is called degree ofdissociation.

Expression:

Degree of dissociation ( )

Νumber of molesdissociated=

Totalnumber of moles takes

Percentage dissociation (% ): % = × 100

6. van't Hoff factor (i) and degree of

dissociation ( )

1

n 1

i





3 2 2

3 4

2 4 3

4 6

n no.of particlesElectrolytes Formulaafter dissociation

Nacl 2 i 1

i 1Ba(NO ) or CaCl 3

2i 1

Na PO 43

i 1Al (SO ) 5

4i 1

K [Fe(CN) ] 54

7. van't Hoff factor (i) and degree of association

:

n(l i)'

(n l)

Examples;

(i) If n = 2 i.e. for dimerisation (2A A2)

' = 2 (1– i) or = i = /2

(ii) If n = 3 i.e. for trimerisation (3A AA3)

3

' (1 i)2

or 2 '

i 13

8. Modified relations for substances :

(a) bT and 01

P

P

b 2b

2 1

1000 K WT

M W

and

01

01

P P

P

or = 2 1

01 1 2

W MP

P W M

bb 0

2 1

1000 K PT

M P

(b) bT and

b 2b

2 1

1000 K WT

M W

and V n RT

b 2b

1 2

1000 K WT n n

W M

Or bb

1

1000 K V VT n

W RT RT

Orb

b

1000 K V WT d

d RT V

(Where d = density of the solvent)

Note: As the solution is dilute volume of thesolution == volume of the solvent.

(c) fT and 01

P

P

0f 1

f 02 1

1000 K P PT

M P

(d) fT and

ff

1000 KT

d RT

ModifiedExpressions for substances

undergoing dissociation or association (Van't

Hoff's factor):

i) CRT i ii) b bT K m i

iii) f fT K m i iv) 01

P n

P N

i

Where nand N are the number of molecules ofsolute and solvent respectively.

IMPORTANT TIPS

1. Isotonic solution: The solutions having sameosmotic pressure are called isotonic solutions orisomotic solutions.

2. Hypertonic solution: A solution which haslower osmotic pressure relative to other solutionis called hypotonic with respect to other.

3. Hypotonic solution: A solution which has lowerosmotic pressure relative to other solution is calledhypotonic with respect to other.

4. Haemolysis: The osmotic pressure blood is 8atm. If blood cells are put in water, it enters inthem and the cells swell up. If water enters inlarge excess the cells burst out. It is calledhaemolysis.

5. Turgor: The pressure developed inside the celldue to the inflow of water into it, is called turgor.

6. Plasmlysis or Crenation: On the contrary, ifblood cells are put in concentrated solution ofcommon salt (NaCl,) water flows out and the cellsshrink down.

7. Reverse Osmosis and Desalination of Sea

water: When the pressure applied on the solutionside is more than the osmotic pressure then





solvent molecules start moving from solution sidetowards pure solvent side through semipermeablemembrane. This is called as reverse osmosis.

8. 0.1% solution of urea, glucose and sucrose,(mol/100 ml) follows the order: urea > glucose> sucrose. Thus urea will have the lowest freezingpoint and vapour pressure. The b.p. will be thehighest.

9. Order of decreasing freezing point (100%

ionization) ( fT Number of particles) (smaller

fT greater will be freezing point)

0.05M NaNO3>0.04 M Ba Cl

2 > 0.075 M

CuSO4

10. For different solutes ofsame molar concentration,the colligative properties have the greater valuefor the solution which gives number of particleson ionization.

Decreasing order of bT for 0.01 M solution.

( bT number of particles)

K3Fe(CN)

6 > K

2HgI

4 > Na[Ag(CN)

2]

n = 4 3 2

11. If (a) 1m Urea (b) 1 m NaCl (c) 1 m Na2SO

4

(d) 1m Na3PO

4 then order of colligative

properties

(i) 0

1b f0

1

P P, T , T ,

P

is d > c > b > a

(ii) F.Pt. and V.P. is a > b > c > d

12. When 1 mole of non-volatile solute is dissolved in1 kg of water then :

(i) B.Pt. = 100 + 0.51 = 100.51°C

(ii) F.Pt. = 0 – 1.86 = –1.86°C

13. Deliquescene:

a) Crystalline substance that absorbs moisturefrom the atmosphere and get dissolve in it.The phenomenon is called deliquescence.Ex. NaOH, MgSO

4 etc.

b) For such substances vapour pressure of theirsaturated solution is lower than the vapourpressure of water in the atmosphere at thattemperature.

14. Efflorescence:

a) Crystalline substance that gives up its waterof crystallization to atmosphere and getdisintegrated into dehydrated product. Thephenomenon is called efflorescence. Ex.:Na

2CO

3.10H

2O, Na

2S

2O

3· 5H

2O

b) Vapour pressure of hydrated crystal is

greater than that of water vapours in theatmosphere at that temperature.

IMPORTANT FORMULAE

(A) Ways of expressing concentration

1. Percent by mass:

% by mass of solute = Massof solute

Massof solution × 100

% x = 'x' g of solute in 100g of solvent. Hencemass of solvent = (100 – x)g.

2. Mole Fraction

If 'n' moles of solute and 'N' number of moles ofsolvent, then mole fraction of solute would be :

a) Xsolute

= n

n N or W

2 = X

2 × Molar mass,

b) Xsolvent

= N

n N or W

1 = X

1 × Molar mass,

Xsolute

= Molesof solute

Molesof solute molesof solvent ,

Xsolvent

= 2

2

Molality M,

1 molality M

XSolvent =

2

2 1

Molarity M

molarity (M M ) d

3. Molarity (Molar concentration):

Molarity = 3

Molesof solute

Volumein dm

3

Massof solute

Molar massof solute V(dm ) =

%Mass 10 d

Molar mass

(Where'd' expressed in g/cm3)Explanation :

Molar 1

2Molar 2

Semimolar 0.5

Pentimolar 0.2

Decimolar 0.1

Centimolar 0.01

Millimolar 0.001

3

No.of molesMolarity ofsolutions(m) in1dm





4. Molality :

Molality (m) Molesof solute

Massof solvent in kilogram = Molesof solute

Molar massof solute Massof solvent in kg

Molality (m) = Molarity ×

3Vol.of solution in dm

Massof solvent in kg = 3 3

Massof solute(g)

Molar massof solute(g)[vol.ofsolution (cm ) d(g / cm ) Massof solute(g)]

Explanation :

Motal 1

2Motal 2

Semimotal 0.5

Pentiomolal 0.2

decimolal 0.1

Centimolal 0.01

Millimolal 0.001

Molarity of Molein 1kgsolution(m) of solvent

5. Relation between molarity and molality:

(a) Molarity

3

Molality Massof solvent in kg

Volumeof solution in dm

(b) (i) If 'd' of solvent is given then M = m x d (for dilute solution)

(ii) If 'd' of solution is given then Molality = Molarity 1000

(d 1000) (Molarity Molar Mass)

Relation between Molarity (m) and Mole fraction:

X d 1000soluteMolarityX Molar massof solvent (X Molar massof solute)solvent solvent

Relation between Molality (m) and mole fraction of solute (X2) in water is

2

mX

55.56 m

(Where moles of water in 1 dm3 is 55.56)

Henry's law:

(i) S = K × P (K Henry's constant in atm-1)

(ii) P = K × Xgas

(K Henry's constant in atm)

Where S solubility in mol dm–3

X mole fraction of gas (solute)

Raoult's law:

1. For volatile solute (for ideal solution)

0 01 2 1 1 2 2p p p p X p X

01p and 0

2p be vapour pressure of pure components 'A1' AA

2. respectively





2. For non volatile solute :

01

01

p p

p

= X

2=

2 2 2

1 21 2

1 2

n W / MW Wn nM M

where 01

01

p p

p

is relative lowering of vapour

pressure.

01p P is lowering of vapour pressure and X

2 is

the mole-fraction of nonvolatile solute.

3. Tocalculate molar mass of solute (M2) from

Raoult's Law:

012 1 1

2 01 1

W M pM kg mol

W p p

Or 0

12 1 12 0

1 1

W M pM 1000g mol

W p p

Where, W1 Mass of solvent in kg W

2 Massof solute in kg

M1 Molar mass of solvent in kg M

2 Molar

mass of solute in kg

P Vapour pressure of solution 01p Vapour

pressure of pure solvent

Boiling point :

(i) Elevation in boiling point b( T )

bT = Boiling point of solution - Boiling point

of pure solvent

(ii) Molal elevation constant or boiling elevationconstant or Ebulliscopic constant of solvent

(Kb): b bT K Molality (if association or

dissociation then b bT i K Molality )

(iii) Determination of molar mass of nonvolatilesolute.

b 2b

2 1

K WT

M W

OR b 22

b 1

K WM

T W

kg mol–1

OR1b 2

2

b 1

K W 1000M gmol

T W

[E] Freezing point:

(i) Depression in Freezing point (Cryoscopy)

f( T ) :

Depression of freezing point f( T ) =

Freezing point of the solvent - Freezing pointof the solution.

(ii) Molal depression constant (Cryoscopicconstant, K

f ) :

fT = Kf × molality × molality (if association

or dissociation then fT = i × Kf × molality)

(iii) Determination of molar mass of nonvolatilesolute from depression in freezing point :

f 2f

2 1

K WT

M W

OR M2

= 1f 2

f 1

K Wkg mol

T W

OR 22

f 1

Kf W 1000M

T W

g mol–1

[F] Osmotic pressure ( ) :

Expression for osmotic pressure: Osmoticpressure = h d g

Where h = height of column d = density of solutionin the column and g = acceleration due togravity = 9.8 ms2

[G] Van't Hoff solution equation:

Determination of molar mass of solute fromosmotic pressure:

V nRT OR 2

2

W RT

M V

OR 22

W RTM

V

Units of R, and V::

1 1 1

1 1 1

2 3

2 3

0.082litre 8.314 8.314Unitsof R atm K JK JK

mol mol mol

Unitsof ( ) atm kPa (k Nm ) dm

Unitsof (V) lit Pa (Nm ) m

4. Relation between osmotic pressure ( ) , lowering

of vapour pressure elevation of boiling point anddepression in freezing point.

01

01 2

P p dRT

P M

= b

b

dRTT

1000K





Where'd' is the density of solution at temperature'T' and M

2 is the molar mass of solute in grams.

5. Relation between degree of dissociation ( ) and

van't-Hoff factor (i)

1

n ' 1

i

n ' Number of cations and anions

6. Relation between degree of association ( ) and

van't-Hoff factor (i)

1 1' n

1 1 n1n

i i

n Number of molecules associated.

7. solution hydration LatticH H H





OBJECTIVE TYPE QUESTIONS

I. Types of Solution and way of expressing

concentration and Henry's Law

1. A solution is

a) a mixture of two compounds

b) a compound of two compounds

c) a homogeneous mixture of two compounds

d) all the above

2. Which of the following statements is incorrectabout a solution?

a) A solution is always a homogeneous mixture.

b) The solute particles in a solution have size lessthan 10 Å.

c) Brass cannot be called a solution.

d) An ionic compound dissolved in water if thehydration energy is greater than lattice energy.

3. An alloy is a homogeneous mixture of

a) a metal and a non-metal

b) two-non-metals

c) two metals

d) two or more metals

4. Out of Molarity (M), molarity (m), formality (F)and mole fraction (x), those dependent ontemperature are

a) M, m b) F, x

c) m, x d) M, F

5. Ionic compounds are readily soluble in polarsolvents because

a) they have high solubility in water.

b) water molecules is polar in nature

c) ionic crystals are easily broken down in thepolar solvents

d) of strong electrostatic forces of attractionbetween ions of crystals and the polar solventmolecules.

6. Solubility curve of Na2SO

4 lOH

2O in water with

temperature is given as

a) Solution process is exothermic

b) Solution process is exothermic till 34°C andendothermic after 34°C

c) Solution process is endothermic till 34°C andexothermic thereafter

d) Solution process is endothermic

7. Two solutions A and B have same mole fractionsof the solute. If 1 dm3 of A is mixed with 2 dm3 ofB, the mole fraction of the solute in the mixturewould

a) decrease

b) increase

c) remain unchanged

d) change

8. CuSO4. 5H

2O is a

a) solution of a solid in a liquid

b) solution ofliquid in a solid

c) salt only and cannot be called a solution

d) coordination compound of copper with watermolecules as the ligands.

9. Which one of the following statements is true fora solution?

a) Molarity is always equal to molality

b) Molarity is always less than molality

c) Molarity is always greater than molality

d) none of these

10. The plot of partial vapour pressure of solventverses its mole fraction in the solution of aconstant temp. is

a) a straight line

b) a straight line parallel to one axis

c) a straight line passing through origin

d) none of the above

11. The sum of mole fractions of A, Band e in as6lution containing O.lmole each ofA, Band e is

a) 0.1 b) 0.3

c) 1.0 d) 1/3

12. Which ofthe following statement is correct aboutsteel (S) and tungsten carbide (We) ?

a) S is a substitutional solid while we is aninterstitial solid solution

b) S is an interstitial solid while we is asubstitutional solid solution

c) Both are interstitial solid solutions

d) Both are substitutional solid solutions

13. The vapour pressures of pure solvent and solutionare 120 mm and 108 mm respectively. The molefraction of the solvent in the solution is

a) 0.1 b) 0.9

c) 120/108 d) 1.08

14. The vapour pressure of solution and pure solventP and P

oresp. If P/P ois 0.15. Then the mole





fraction of the solute in the solution is

a) 0.85 b) 0.15

c) 1/0.15 d) 1/0.85

15. Increasing the temperature of an aqueous solutionwill cause

a) decrease in molality

b) decrease in molarity

c) decrease in mole fraction

d) decrease in % w/w

16. Which of the following represents a metastablesystem?

a) A dilute solution

b) An unsaturated solution

c) A saturated solution

d) A supersaturated solution

17. The example of solution of liquid in gas is

a) dry air b) aerated waterc) amalgam d) moist air

18. Out of molarity (M), molarity (rn), normality (N)and mole fraction (z), those independent of temp.are

a) M. m b) M,N

c) m, x d) N, x

19. Which ofthe following statement is not correct?

a) 1 ppm of fluoride ions in water prevents toothdecay

b) 1.5ppm of fluoride ions in water causes teethto become mottled

c) Higher concentration of fluoride ions acts as apoison for rats

d) Intravenous injections should have lower ionicconcentration than that of out blood plasma

20. A solid dissolves in water if

a) lattice energy is greater than hydration energy

b) lattice energy is less than hydration energy

c) lattice energy is equal to hydration energyd) dissolution is exothermic.

21. Which one of the following statement is incorrect?

a) Normality of a solution depends ontemperature

b) Molality of a solution depends on temperature

c) Molarity ofa solution depends on temperature

d) Molality of a solution relates to mass of solventand moles of solute

22. The factor f

f

T

K

represent:

a) Molarity b) Formality

c) Normality d) Molality

23. Iodine is more soluble in alcohol than in carbontetrachloride because

a) iodine and alcohol both are non-polar

b) randomness factor is greater in alcohol their inCCl

4

c) dissolution of iodine in alcohol is exothermicwhereas it is endothermic in CCl

4

d) dissolution of bothe is endothermic but heat ofdissolution in alcohol is less than in CCl

4

24. An example of a solution having liquid in solid is

a) Moist air b) Dry air

c) Au-Hg d) C2H

5OH + H

2O

25. Two solutions of KNO3 and CH

3COOH are

prepared separately. Molarity of both is 0.1 Mand osmotic pressures are P

1, and P

2 respectively.

The correct relationship between the osmoticpressures is:

a) P2> P

1b) P

1= P

2

c) P1> P

2d) P

1, and P

2

FRAC...

26. For an aqueous solution of the same solute, termsof concentration,

a) 1M = 1 m

b) 1M > 1m

c) 1 m > 1M

d) Any of these is possible

27. If P0 and P are the vapour pressures ofthe solvent

and solution respectively, n1 and n

2 are the mole

fractions of the solvent and solute respectively,then

a) P = P0n

1b) P = P

0n

2

c) P0 = Pn

2d) 1

0

2

nP P

n

28. Solubility of a gas in a liquid increases with

a) increase of pressure and increase oftemperature

b) decrease of pressure and increase oftemperature

c) increase of pressure and decrease oftemperature

d) decrease of pressure and decrease oftemperature

29. Sugar is soluble in water due to

a) High solvation energy

b) Lonie character of sugar

c) High dipole moment of wate, r

d) Hydrogen bond formation With water.





30. An example of solid solution is:

a) Amalgam

b) Brass

c) Na in NH3

d) Dust in air

31. If mole fraction of the solvent in a solutiondecreases then

a) vapour pressure of solution increases

b) boiling point decreases

c) osmotic pressure increases

d) all are correct

32. Which of the following is incorrect?

a) Mass of the gas dissolved is inverselyproportional to its pressure

b) Mass of the gas dissolved is inverselyproportional to temperature

c) A soda-water bottle contains oxygen gasdissolved under pressure

d) Permanent gases are less soluble thantemperature gases.

33. Which is not the colligative property?

a) Refractive index

b) Osmotic pressure

c) Lowering of vapour pressure

d) Elevation in boiling point

34. Which of the following correctly representsHenry's law?

a) m = KHP

A

b) xA = K

HP

A

c) PA = K

Hx

A

d) All of these

II. Lowering of Vapour pressure and Raoult's

Law

35. The use of common salts, NaCI or CaCl2

anhydrous is made to clear snow on the roads.This causes

a) a lowering in f. pt. of water

b) a lowering in m. pt. of ice

c) ice melts at the temperature of atmospherepresents at that time

d) all

36. Which of the following of correct for a solutioncontaining non volatile solute from Raoult's law?

a) V= +ve, H = +ve

b) V= -ve, H = -ve

c) V= +ve, H = -ve

d) V= -ve, H = +ve

37. A liquid is kept in a closed vessel. If a glass plate

(negligible mass) with a small hole is kept on topof the liquid surface, then the vapour pressure ofthe liquid in the vessel is

a) more than what would be if the glass platewere removed

b) same as what would be ifthe glass plate wereremoved

c) less than what would be ifthe glass plate wereremoved

d) cannot be predicted

38. 5 mL of acetone is mixed with 100mL of H2O. The

vapour pressure of water above the solution is

a) equal to the vapour pressure of pure water

b) equal to the vapour pressure ofthe solution

c) less than the vapour pressure of pure water

d) more than the vapour pressure of pure water.

39. In which of the following molecular massdetermination method, sensitivity of themeasurements decreases as the molecular massof the solute increases

a) elevation of boiling point/depression in f.pt.

b) viscosity

c) osmotic pressure

d) none

40. When a crystal of the solute is introduced into asuper saturated solution of the solute

a) the solute dissolves

b) the excess solute crystallises out

c) the solution becomes unsaturated

d) the solution remains super saturated

41. For an ideal binary liquid solution with 0 0A BP P

which of the following relations between xA(mole

fraction ofAin liquid phase) and yA(mole fraction

ofA in vapour phase) is correctly represented?

a) xA

= yA

b) xA> y

A

c) xA < y

A

d) xA< y

A cannot be correlated with each other

42. V.P.of a solution containing non-volatile solute is

a) more than the vapour pressure of solvent

b) less that the vapour pressure of a solvent

c) equal to the vapour pressure of solvent

d) none

43. The relative lowering ofvapour pressure is equalto the more fraction of the non-volatile solute.This statement was given by .

a) Raoult b) Henry

c) Joule d) Dalton





44. An aqueous solution of methanol has vapourpressure

a) equal to that of water

b) equal to that of methanol

c) more than that of water

d) less than that of water

45. When a substance is dissolved in a solvent, thevapour pressure of solvent decreases. This brings

a) an increase in b.pt. ofthe solution

b) a decrease in b.pt. of a solution

c) an increase in f.pt. of the solvent

d) none

46. By adding water to the solution, its

a) concentration remains same

b) concentration increases

c) ionisation decreases

d) concentration decreases

47. The lowering of vapour pressure of the solventtakes place

a) only when the solute is non-volatile

b) only when the solute is volatile

c) only when the solute is a non-electrolyte

d) in all the above three cases.

48. Two solutions have different osmotic pressures.The solution of lower osmotic pressure is called

a) Isotonic solution

b) Hypertonic solution

c) Hypotonic solution

d) None

49. Which one of the following is an expression ofRaoult's law if P

A is the partial pressure of the

solvent is a solution, ~ is the partial pressure ofthe pure solvent and if X

Aand X

B are the mole

fraction ofthe solute and the solvent repectively?

a) 0A A AP P X b) 0

A A A BP P X (1/ X )

c) 0A A BP P X d) 0

A A BP P(X / X )

50. The pressure under which liquid and its vapourcan coexist in equilibrium is known as

a) normal vapour pressure

b) saturated vapour pressure

c) real vapour pressure

d) limiting vapour pressure

51. The lowering of vapour pressure in case of dilutesolutions is directly proportional to

a) molality b) molarity

c) mole fraction d) all

52. Existance of aquatic life is an application of

a) Henry's law b) Raoult's law

c) Dalton's law d) Boyle's law

53. In two solutions having different osmoticpressures, the solution ofhigher osmotic pressureis called

a) Isotonic solution

b) Hypertonic solution

c) Hypotonic solution

d) None

54. When an ideal binary solution is in equilibriumwith its vapour, molar ratio ofthe two componentsin the solution and in the vapour phase is

a) same

b) different

c) mayor may not be same depending uponvolatile nature of the two components

d) all

55. If Raoult's law is obeyed, the vapour pressure ofthe solvent in a solution is directly proportional to

a) (l-mole fraction of solute)

b) mole fraction of the solute

c) mole fraction of the solvent and solute

d) the volume of the solution

56. The relative lowering to the vapour pressure isequal to the ratio between the number of

a) solute molecules to the solvent molecules

b) solute molecules to the total molecules in thesolution

c) solvent molecules to the total molecules in thesolution

d) solvent molecules to the total number ofionsof the solute.

57. For determination ofmolecular masses, Raoult'slaw is applicable only to

a) dilute solutions of electrolytes

b) concentrated solutions of electrolytes

c) dilute solutions of non-electrolytes

d) concentrated solutions of non-electrolytes.

58. 12 g of urea is dissolved in 1 litre of water and68.4 g of sucrose is dissolved in 1 litre of water.The lowering of vapour pressure of first case is

a) equal to second

b) greater than second

c) less than second

d) double that of second

59. The solubility of a gas in liquid at a temperatureis directly proportional to its

a) Density b) Melting point





c) Boiling point d) Pressure

60. The vapour pressure of water depends upon:

a) surface area of container

b) volume of container

c) temperature

d) all

61. Dust is an example of-

a) solid solution

b) liquid solution

c) gas solution

d) none

62. The molal elevation/depression constant dependson

a) nature of solvent

b) nature of solute

c) temperature

d) H solution

63. Which of the following statement is correct?

a) Lowering of vapour pressure takes place onlyin ideal solutions.

b) Lowering of vapour pressure does not dependupon the solvent at a given concentration ofthe solute.

c) Lowering of vapour pressure depends uponthe nature of the solute.

d) Relative lowering of vapour pressure does notdepend upon the solvent at a givenconcentration of solute.

64. For a dilute solution, Raoult's law states that

a) the lowering of vapour pressure is equal tothe mole fraction of solute

b) the relative lowering of vapour pressure isequal to the mole fraction of solute 2.15

c) the relative lowering of vapour pressure isproportional to the amount of solute in solution

d) the vapour pressure of the solution is equal tothe mole fraction of solvent

65. Which is not a colligative property?

a) Atmospheric pressure

b) Lowering of vapour pressure

c) Osmotic pressure

d) Elevation of boiling point.

66. An example of colligative property is

a) Freezing point

b) Boiling point

c) Vapour pressure

d) Osmotic pressure

67. The colligative properties of a solution depend on

a) number of solute particles present in it

b) chemical nature of the solute particles presentin it.

c) nature of the solvent used

d) none

68. Which method cannot be used to find out themolecular mass of non-volatile solute

a) Victor Mayer's method

b) Osmotic pressure method

c) Cryoscopic method

d) Ebullioscopic method

69. The vapour pressure of a dilute solution of a soluteis NOT influenced by

a) temperature of solution

b) melting point of solute

c) mole fraction of solute

d) degree of dissociation of solute

70. The vapour pressure (VP) of a dilute solution ofnon-volatile solute is P and the VP ofpure solventis P

0' the lowering of the VP is:

a) + ve b) - ve

c) 0

P

P d) 0P

P71. Alcohol has ... vapour pressure than water at the

same temperature

a) more b) less

c) same d) none

72. Binary liquid solutions which exhibit negativedeviations from Raoult's law boil attemperature...... than the expected value

c) lower b) higher

c) same d) can not be said

73. Which solution will show the maximum vapourpressure at 300 K

a) 1MNaCI b) 1MCaCl2

c) 1MCH3COOH d) 1MC

12HO

ll

74. If Po and P

s are the vapour pressure of solvent

and solution respectively and N1 and N

2are the

mole of solute and solvent then

a) 0 S 1

0 1 2

(P P ) N

P (N N )

b) 0 S 1

S 2

(P P ) N

P N

c)1

s 0

1 2

NP P

(N N )

d) All





75. Which ofthe following will have the highest F.P.at one atm pressure?

a) 0.1 MNaCI solution

b) 0.1 Msugar solution

c) 0.1 M BaCl2 solution

d) 0.1 M FeCl3 solution.

76. A liquid is in equilibrium with its vapours at itsboiling point. On the average the molecules inthe two phases have equal

a) potential energy

b) total energy

c) kinetic energy

d) intermolecular forces

77. If the temperature increases from O°C to 50°Cat atmospheric pressure, which of the followingprocessess is excepted to take place more in caseofliquids

a) fusion b) vaporisation

c) solubilization d) none

78. The lubricating action ofan oil is more if it possess

a) high vapour pressure

b) low vapour pressure

c) high surface tension

d) high density

79. In a solution if the amount of solvent is doubled,keeping the amount of solutes same, the share ofsolute in the solution

a) become half

b) would decrease but not a half

c) remain unchanged

d) changed unpredictably

80. Which of the following plots does not representthe behaviour of an ideal binary liquid solution?

a) Plot PA

versus xA

(mole fraction ofAin liquidphase) is linear

b) Plot of PB versus x

B is linear

c) Plot of Ptotal

versus xA (or x

B) is linear

d) Plot of Ptotal

versus xA is non-linear

81. In a very dilute solution the no. of moles of solventare 10 times more than that ofthe solute. Thev.P. of the solution would be

(VP. of pure solvent = 80 mm)

a) 80 mm b) 88 mm

c) 72 mm d) 92 mm

82. When a liquid is heated its vapour pressure

a) continuously increases

b) continuously decreases

c) increases and becomes constant at b.pt of liquid

d) records no predictable change

83. 0.1 M NaCI and 0.1 M CH3COOH are found to

have osmotic pressure of p1 and P

2 respectively

then what is the correct statement?

a) P1 > P

2b) P

1 = P

2

c) P1 < P

2d) P

1 = P

2= 0 atm.

84. Among (P) water (Q) ethanol and (R) mercurythe correct order of vapour pressure at roomtemp. is

a) P > Q > R b) Q > P > R

c) R > Q > P d) Q > R > P

85. In a solution of two miscible volatile liquids A andB, the plots of their partical VP. Vs their molefractions is given by (Assume, VP. of pure A>v.P. of pure B)

III. Boiling Point Elevation

86. Which solution will have highest boiling point?

a) 1% glucose b) 1% NaCl

c) 1% sucrose d) 1% CaCl2

87. You are given 100 cc of CC14 to extract iodine

from 200 ccof its aqueous solution. For extractingmaximum amount of iodine, which one of thefollowing

a) use of 100 cc of CC14 once

b) use of 50 cc of CCl4 twice

c) use of 10 cc of CC14 tep times

d) use of 25 cc of CC14 four times

88. The molal elevation constant is the ratio of theelevation in boiling point to

a) molarity

b) molality

c) mole fraction of solute

d) mole fraction of solvent.

89. The elevation in boiling point for one molal solutionof a solute in a solvent is called

a) Cryoscopic constant

b) Boiling point constant

c) Molal Ebullioscopic constant

d) None





90. Boiling point of a solution is independent of

a) amount of solution

b) pressure

c) nature of solvent

d) concentration of solution

91. Which solution will show maximum elevation inb.pt.

a) 0.1 M KCl

b) 0.lMBaCI2

c) 0.1 MFeCl3

d) 0.1M Fe2 (8O

4)

3

92. Which one of the is not the correct unit of molalelevation constant?

a) °C/m b) K/m

c) K kg mol-1 d) K mol kg–1

93. At high altitudes the boiling point of waterdecreases because

a) atmospheric pressure is low

b) temperature is low

c) atmospheric pressure is high

d) none

94. A teacher one day pointed out to his studentspeculiar fact that water is unique liquid whichfreezes exactly at O°Cand boils exactly at l00°C.He asked the students to find the correctstatement based on this fact

a) water dissolves anything however sparinglythe dissolution may be

b) water is a polar molecule

c) boiling and freezing temperatures of waterwere used to define a temperature scale

d) liquid water is denser than ice

95. Boiling point of water is defined as thetemperature at which

a) vapour pressure of water is equal to that ofone atmospheric pressure

b) bubbles are formed

c) steam comes out

d) none

96. If the amount of a non-electrolyte dissolved isdouble but that of solvent is quadrupled, theelevation in boiling point of the solution will be

a) doubled

b) halved

c) four times

d) unchanged

97. The melting points ofmost ofthe solid substancesincrease with an increase of pressure acting onthem. However, ice melts at a temperature lower

than its usual melting point, when the pressureincrease. This is because

a) ice is less denser than water

b) pressure generates heat

c) the bonds break under pressure

d) ice is not a true solid.

98. The correct relationship between the boiling pointsof very dilute solutions of AICl

3 (t

l) and CaCl

2

(t2) having the same molar concentration is

a) tl = t

2b) t

l > t

2

c) t2 > t

ld) t

2 > t

l

99. The highest temperature at which vapour pressureof a liquid can be measured is

a) boiling point ofliquid

b) critical temperature (T)

c) critical solution temperature

d) inversion temperature

100. The elevation of boiling point method is used forthe determination of molecular mass of

a) non-volatile and soluble solute

b) non-volatile and insoluble solute

c) volatile and soluble solute

d) volatile and insoluble solute

101. Molal elevation constant of a liquid is:

a) the elevation ofb.pt. which would be producedby dissolving one mole of solute in 100 g ofsolvent

b) the elevation ofb.pt. which would be producedby dissolving 1 mole solute in 10 g of solvent

c) elevation in b.pt. which would be producedby dissolving 1 mole of solute in 1000 g ofsolvent

d) none

102. The boiling point of C6H

6, CH

3H, C

6H

5NH

2 and

C6H

6NO

2 are 80°C, 65°C, 184°C and 212°C

respectively. Which will show highest vapourpressure at room temperature

a) C6H

6b) CH

3OH

c) C6H

5NH

2d) C

6H

5NO

2

103. A pressure cooker reduces cooking time because:

a) heat is more evenly distributed

b) b.pt. of water inside the cooker is increased

c) the high pressure tenderises the food

d) all

104. Water will boil at 101.5°Cat which ofthe followingpressure :

a) 76 cm of Hg

b) 76 mm of Hg





c) > 76 cm of Hg

d) < 76 cm of Hg

105. Which characterises the weak intermolecularforces of attraction in a liquid

a) high boiling point

b) high vapour pressure

c) high critical temperature

d) high heat of vapour isat ion

106. Addition of common salt to a sample of waterwill

a) increase its freezing point and increase theboiling point

b) decrease its freezing point and increase theboiling point

c) increase both the boiling and the freezing point

d) decrease both the boiling and the freezingpoint.

107. Equimolal solutions will have the same boilingpoint, provided they do not show

a) electrolysis

b) association

c) dissociation

d) association or dissociation

108. An aqueous solution is heated until it begins toboil. The atmospheric pressure is 760 mm ofHg.The boiling temperature will be

a) 100°C b) > 100°C

c) < 100°C d) None

109. When a substance is dissolved in a solvent, thevapour pressure of the solvent is decreased. Thisresults in

a) an increase in the b.p. of the solution

b) a decrease in the b.p. of the solvent

c) The solution having a higher freezing point thanthe solvent

d) the solution having a lower osmotic pressurethan the solvent.

110. On the basis of intermolecular forces predict thecorrect order of decreasing boiling points of thecompounds

a) CH3OH > H

2> CH

4

b) CH3OH> CH

4 > H

2

c) CH4 > CH

3pH > H

2

d) H2> CH

4 > CH

3OH

111. Elevation of boiling point is directly proportionalto

a) molality of the solution

b) depression of freezing point in the same solution

c) both of these

d) none of these

112. Todetermine the elevation of boiling point moreaccurately. The solvent area should take

a) higher value of Kb

b) lower value of Kb

c) high molar mass

d) low molar mass

113. The molecular mass of a solute cannot becalculated by one of the following relations

a) 22

1

Kb 1000 wM

Tb w

b) 22

w RTM

V

c)

10 2 1

2 10 1

P w MM

(P P) w

d)b 2

2

b 1

T wM 1000

K w

114. Assuming complete ionization, which one of thefollowing aqueous solution will have maximumboiling point?

a) 0.2 MNaCl b) 0.2MCaCl2

c) 0.1 M BaC12

d) 0.1 M FeCl3

115. Some statements are given below

a) for the same solution Tb = T

f

b) 5%of solution of urea will have more osmoticpressure than that 10% solution of glucose

c) elevation of B.pt. is due to increase in vapourpressure of solution on adding solute

d) depression of F.pt. is due to decrease in vapourpressure of solution on adding solute. Amongthe above

a) B and D are true

b) A, Band D are false

c) B and C are false

d) only D is true

116. Ebullioscopy is concerned with

a) osmotic pressure

b) lowering of vapour pressure

c) elevation of B.pt

d) depression of F.pt

IV. Freezing Point Depression

117. The temperature at which vapour pressure of asofvent in its liquid and solid phase becomes sameis called





a) b.pt b) f.pt

c) sublimation point d) none

118. To form a super saturated solution of salt onemust

a) cool slowly

b) coolrapidly

c) add some salt to cold solution

d) use a clear vessel

119. The freezing point of 1% aqueous solution ofcalcium nitrate will be

a) 0°C b) Above 0°C

c) 1°C d) Below 0°C

120. The molal depression constant depends upon

a) nature of the solute

b) nature of the solvent

c) heat of solution of the solute in the solvent

d) vapour pressure of the solution.

121. The moles of a solute are dissolved in Wg ofwater. If K

f, is the molal depression constant of

water, the freezing point of the solution will be

a)f 1

1

1000K W

W b)f

1

1000K n

W

c) f 11000K W

nd) f 11000K W

n

122. The depression in freezing point is maximum if,... is used as solvent

a) camphor b) naphthalene

c) benzene d) water

123. During freezing point depression in the solutionthe following are in equilibrium-

a) liquid solvent-solid solvent

b) liquid solvent-solid solute

c) liquid solute-solid solute

d) liquid solid-solid solvent

124. What will be the molecular weight of NaCldetermined experimentally following elevation inthe boiling point or depression in freezing pointmethod

a) < 58.5 b) > 58.5

c) = 58.5 d) None

125. On freezing an equeous solution of sugar, the solidthat starts separating out is

a) sugar

b) ice

c) solution with the same composition

d) solution with a different composition.

126. The value of Kf for water is 1.86°,calculated from

glucose solution. The value of Kf, for water

calculated for NaCI solution will be

a) = 1.86 b) < 1.86

c) > 1.86 d) Zero

127. The depression in f.pt. is directly proportional to

a) Normality b) Molality

c) Molarity d) None

128. Which one of the following statement is incorrect?

a) Greater the lowering of va pouring pressure,greater is the boiling point of the solution

b) Greater the lowering of vapour pressure,greater is the freezing point of the solution.

c) At the freezing point, the solute and the solventhave same vapour pressure

d) The units of molal depression constant are

Km-1.

129. Which ofthe following 0.1 M aqueous solutions

will have the lowest freezing point

a) Potassium sulphate

b) Sodium chloride

c) Urea

d) Glucose

130. The molal cryoscopic constant for water is

a) 1.86 K molality-1

b) 5.26 K molality-1

c) 55.5 Kmolality-1

d) 0.52 K molality-1

131. When mercuric iodide is added to the aqueoussolution of potassium iodide, the

a) f.pt. is raised

b) f.pt. is lowered

c) f.pt. does not change

d) b.pt. does not change

132. Molal elevation constant and molal depressi: .,constant for water respectively (in °C/m) are

a) 0.52, 1.86 b) 1.86, 0.52

c) 1.52, 0.86 d) 0.86, 1.52

133. At a suitable pressure near the freezing point ofice, there exists

a) only ice

b) ice and water

c) ice and steam

d) ice, water and steam, all existing side by side

134. The-reverse of fusion is freezing and it is

a) endothermic

b) exothermic

c) neither exothermic nor endothermic





d) may be exothermic or endothermic

135. In cold countries, ethylene glycol is added towater in the radiators of cars during winters. Itresults in

a) lowering in boiling point

b) reducing viscosity

c) reducing specific heat

d) lowering in freezing point

136. Equimolal solutions of A and B show depressionin freezing point in the ratio 2 : 1. A remains in itsnormal state in solution. B will be in solution

a) normal b) dissociated

c) associated d) hydrolysed.

137. The molar mass of benzoic acid in benzene asdetermined by depression in f. pt. methodcorrespond to

a) ionization of benzoic acid

b) dimerization of benzoic acid

c) trimerization of benzoic acid

d) solvation of benzoic acid

V. Osmosis and Osmatic Pressure

138. At constant temp. the osmotic pressure (n) andthe molarity (M) of the solution are related as

a) M b)1

M

c) M d)1

M

139. The molecular mass (rn) of a solute and osmoticpressure (rr) of its solution are related as

a) wRT / m b) m RT / w

c) wm RT / w d) m WR / T

140. Which one of the following statement is falseabout osmotic pressure?

a) It is the pressure of the hydrostatic columnset up due to osmosis.

b) It is the pressure applied on the solution toprevent the entry of the solvent into it throughthe semi-permeable membrane.

c) During osmosis, the flow of solvent is onlyfrom dilute solution to concentrated solution.

d) Osmotic pressure is directly proportional tothe temperature of the solution.

141. Assuming the degree of ionization to be equal,the ratio of osmatic pressures of equimolar solutionof Al

2(SO

4)

3 ,Na

3PO

4 and K

4[Fe(CN)

6]is

a) 5 : 4 : 5 b) 4 : 5 : 6

c) 1: 0.8 : 1 d) 0.8 : 1 : 1

142. The relationship between osmotic pressure at 273K when 10 g glucose (P

1), 10 g MgC1

2(P

2), and

10 g NaCl (P3)are dissolved in 250 mL of water

is

a) P1> P

2 > P

3

b) P3 > P

1 > P

2

c) P2> P

1 > P

3

d) P2> P

3> P

1

143. If 0.1 M solution of glucose and 0.1M solution ofurea are placed on two sides ofthe semipermeablemembrane to equal heights, then it will be correctto say that

a) there will be no net movement across themembrane

b) glucose will flow towards urea solution

c) urea will flow towards glucose solution

d) water will flow from urea solution to glucosesolution.

144. A solution which has lower osmotic pressurecompared to that of the other solution is know as

a) Hypotonic

c) Isotonic

b) Hypertonic

d) None ofthe above.

145. Two solutions A and B are separated by asemipermeable membrane. As a result to osmosis,the level of solution A is found to rise. It impliesthat

a) solutionAis more concentrated than solutionB

b) solutionBis more concentrated than solutionA

c) the solute molecules of A are smaller thanthose of B

d) the solute molecules of B are smaller thanthose of A

146. Who was awarded Nobel Prize for chemistry in1901 for discovering laws of osmotic pressurefor solutions

a) van't Hoff b) Pauling

c) Berkeley d) Seaberg

147. Assuming each salt to be 90% dissociated whichof the following will have highest osmoticpressure

a) decinormal Al2(SO

4)

3

b) decinormal BaCl2

c) decinormal Na2SO

4

d) a solution obtained by mixing equal volumesof b) and c) and filtering

148. When a solution is separated from a solvent by





semipermeable membrane, then phenomenontaking place is called as

a) osmosis b) diffusion

c) solubility d) none

149. The osmotic pressure of a solution increases if

a) temperature is decreased

b) solution constant is increased

c) number of solute particles is increased

d) volume is increased.

150. A 0.6% solution of urea (molecular mass = 60)would be isotonic with

a) 0.1 M glucose

b) 0.1MKCI

c) 0.6% glucose

d) 0.6%KCI

151. Which of the following colligative properties canprovide molar mass of proteins (or polymers orcolloids) with greater precision?

a) Relative lowering of vapour pressure

b) Elevation of boiling point

c) Depression in freezing point

d) Osmotic pressure.

152. The outer shell of an egg was dissolved inhydrochloric acid and then placed in concentratedNaCI solution. Which one of the following willhappen?

a) The egg will swell

b) The egg will shrink

c) Nothing will happen to the egg

d) The inside of the egg will become saltish.

153. If a thin slice of sugar beet is placed Inconcentrated solution of NaCI then

a) sugar beet will lose water from its cells

b) sugar beet will absorb water from solutions

c) sugar beet will neither absorb nor lose water

d) sugar beet will dissolve in solution

154. As a result of osmosis, the volume of theconcentrated solution

a) gradually decreases

b) gradually increases

c) suddenly increases

d) none

155. As a result of osmosis, the volume of the solution

a) gradually decreases

b) gradually increases

c) is not affected

d) any of the three.

156. Which inorganic precipitate acts as a

semipermeable membrane?

a) Calcium phosphate

b) Nickel phosphate

c) Calcium sulphate

d) Copper ferrocyanide.

157. The value ofosmoticpressure doesnot dependupon

a) concentration of the solution

b) temperature of the solution

c) number ofthe particles of the solute present

d) structure of the solute particles.

158. A plant cell shrinks when it is kept in

a) hypotonic solution

b) a hypertonic solution

c) a solution nisotonic with cell sap

d) water.

159. Dissolution of a solute is an exothermic processif

a) Hydration energy > Lattice energy

b) Hydration energy < Lattice energy

c) Hydration energy = Lattice energy

d) None

160. The phenomenon in which cells are swelled upand then burst if placed in hypotonic solutions iscalled

a) Plasmolysis b) Haemolysis

c) Exosmosis d) None

161. Two aqueous solutions S1 and S

2 are separated

by a semi-permeable membrane. S2 has lower

vapour pressure than S1. Then

a) more solvent will flow fromS1 to S

2

b) more solvent will flow from S2 to S

1

c) solvent from S1and S

2will flow at equal rates

d) no flow will take place.

162. A solution which has higher osmotic pressurescompared to other solution is known as

a) Hypotonic b) Hyperonic

c) Isotonic d) Normal.

163. At low concentrations, the statement thatequimolal solutions under a given set ofexperimental conditions have equal osmoticpressure is true for

a) all solutions

b) solutions of non-electrolytes only

c) solutions of electrolytes only

d) none of these.

164. The phenomenon in which cells are shrinked downif placed in hypertonic solution is called





a) Plasmolysis b) Haemolysis

c) Endosmosis d) None

165. Which salt shown maximum osmotic pressure inits 1M solution

a) AgNO3

b) Na2SO

4

c) (NH4)

3PO

4d) MgC

2.

166. The natural semipermeable membrane is

a) Gelatinous Cu2Fe (CN)

6

b) Gelatinous Ca3(PO

4)

2

c) Plant cell

d) Phenol layer

167. An aqueous solution of sucrose, C12

H22

O11

containing 34.2 g/L has an osmotic pressure of2.38 atmospheres at 17°C. For an aqueoussolutions of glucose, C

6H

12O

6 to be isotonic with

this solution, it would have:

a) 34.2 glL b) 17.1 glL

c) 18.0 glL d) 36.0 g/L of glucose

168. Which involves osmosis

a) Crenation b) Plasmolysis

c) Haemolysis d) All

169. The plant cell will shrink when placed in

a) Water

b) a hypotonic solution

c) a hypertonic solution

d) an isotonic solution

170. The process of getting freshwater from sea wateris known as

a) Osmosis b) filtration

c) Diffusion d) Reverse osmosis

171. The osmotic pressure of a dilute solution is directlyproportional to the

a) diffusion rate ofthe solute

b) ionic concentration

c) boiling point

d) flow of solvent from a concentrated solution

172. The molecules which diffuse through a cellmembrane are of

a) Fructose b) Glycogen

c) Haemoglobin d) Catalase

173. Aperfectly semipermeable membrane when usedto separate a solution from its solvent permitsthrough it the passage of

a) solute only

b) solvent only

c) both (a) and b)

d) none

174. At low concentrations, the statement that

equimolal solutions under a given set ofexperimental conditions have equal osmoticpressure is true for

a) all solutions

b) solutions of non-electrolytes which neitherdissociates nor associates

c) solutions of electrolytes only

d) none

175. Blood cells retain their normal shapes in solutionswhich are

a) isotonic to blood

b) hypotonic to blood

c) hypertonic to blood

d) equinormal to blood

176. As a result of osmosis the volume of solution

a) remains constant

b) increases

c) decreases

d) increases or decreases

177. The osmotic pressure (rt) of a solution is givenby relation

a)RT

C b)

CT

R

c)RC

T d) RT

C

178. Which acts as semipermeable membrane?

a) Calcium phosphate (gelatinous)

b) Phenol layer

c) Copper ferrocyanide (gelationous)

d) All

179. Which statement is incorrect about osmoticpressure (P), volume (V) and temperature (T)

a) P 1

V , if T is constant

b) P T, if V is constant

c) P V,ifT is constant

d) PV is constant, if T is constant

180. Solute when dissolved in water

a) decreases the vapour pressure of water

b) increases the boiling point of water

c) decreases the freezing point of water

d) all of the above

181. The osmotic pressure of a dilute solution is givenby

a) P = Po × N

1, b) V = nRTT





c) P = P0N

0d)

0 S

0 0

P P1

V P

182. Blood has been found to be isotonic with

a) normal saline solution

b) saturated NaCI solution

c) saturated KCI solution

d) saturated solution of a 1 : 1 mixture of NaCI.and KCI

183. Isotonic solutions are those which have the:

a) same osmotic pressure

b) same molarity

c) same density

d) same normality

184. Osmosis is the spontaneous flow through asemipermeable membrane of

a) a less concentrated solution into moreconcentrated solution .

b) the solvent from a solution of lowerconcentration to one of higher concentration

c) solute particles from a solution of higherconcentration to one of lower concentration

d) none

185. Two solutions A and B are separated bysemipermeable membrane. If liquid flows fromA to B then

a) A is more concentrated than B

b) A is less concentrated than B

c) both solutions have same concentration

d) none

186. One mole each of urea, glucose and sodiumchloride were dissolved in one litre ofwater. Equalosmotic pressure will be produced by solutionsof

a) Urea and glucose

b) Sodium chloride and urea

c) Glucose and sodium chloride

d) None

187. Who proposed the concept, that solute particlein solution behaves like gaseous molecules

a) Boyle b) van't Hoff

c) Nollet d) Charles

188. Which of the following solutions will have thehighest boiling point at 1 atm pressure?

a) 0.l M FeCl3

b) 0.l M Ba Cl2

c) 0.l M NaCl d) 0.1 Murea

189. Which of the following aqueous solution hasminimum freezing point?

a) 0.01 m NaCl

b) 0.005 m C2H

5OH

c) 0.005 m Mgl2

d) 0.005 m MgSO4

190. Benzoic acid undergoes dimerisation in benzenesolution, the van't Hoff factor 'i' is related to thedegree of association 'x' of the acid as

a) i = (1 - x) b) i = (1 + x)

c) i = (1- x/2) d) i = (1+ x/2)

191. van't Hoff factor (i)

a) Is less than one in case of dissociation

b) Is more than one in case of association normalmolecular mass

c) i = normalmolecular mass

observed molecular mass

d) i = observed molecular mass

normalmolecular mass

192. Acetic acid on dissolution in benzene will show

a) two times of its normal molecular mass

b) its normal molecular mass

c) half of its normal molecular mass

d) none

193. On mixing 10 mL of acetone with 40 mL ofchloroform, the total volume of the solution is

a) < 50 mL b) > 50 mL

c) = 50 mL d) Cannot be predicted

194. The substance A when dissolved in solvent Bshows the molecular mass corresponding to A

3

The van't Hoff factor will be

a) 1 b) 2

c) 3 d) 1/2

195. Benzoic acid dissolved in benzene shows

a) Its normal molecular mass

b) Double of its normal molecular mass

c) Half of its normal molecular mass

d) Not definite.

196. Solutions A, B, C and D are respectively 0.1 Mglucose, 0.05 M NaCI, 0.05 M BaCl

2 and 0.1 M

AlCI3Which one ofthe following pairs is isotonic?

a) A and B b) Band C

c) A and D d) A and C.

197. Which of the following solution will have thehighest boiling point?

a) 1% solution of glucose in water.

b) 1% solution of sucrose in water.

c) 1% solution of sodium chloride in water.

d) 1% solution of calcium chloride in water.





198. On mixing 10 mL of carbon tetrachloride with 10mL of benzene the total volume of the solution is

a) > 20 mL

b) < 20 mL

c) = 20 mL

d) cannot be predicted

199. Which of the following is incorrect?

a) Molecular mass of NaCI found by osmoticpressure measurements is half of the theoreticalvalue

b) Molecular mass of CH3COOH in benzene

found by cryoscopic methods is double of thetheoretical value

c) Osmotic pressure of 0.1 M glucose solution ishalf of that of 0.1 M NaCI solution

d) Molecular mass of HCI found by anycolligative property will be same in the aqueoussolution and benzene solution.

200. Relation between degree of dissociation (a) andvant Hoff's factor for BaCl2 is

a) i = 1+ b) i = 1+ 2c) i = 1- d) i = 1- 2

201. The van't Hoff factor of NaCI assuming 100 %dissociation is

a) 1

2b) 2

c) 1 d) 3

202. The depression in freezing point of 0.1 M aqueoussolutions of HCI, CuSO

4 and K

2SO

4 are in the

ratio

a) 1 : 1 : 1 b) 1 : 2 : 3

c) 1: 1 : 1.5 d) 2 : 4 : 3

203. Which of the following compounds correspondsto van't Hoff factor (i) to be equal to 2 for dilutesolution?

a) K2SO

4b) NaHSO

4

c) Sugar d) MgSO4

204. The van't Hoff's factor (i) for a 0.2 molal aqueoussolution of urea is

a) 0.2 b) 0.1

c) 1.2 d) 1.0

205. The van't Hoff factor (i) for a dilute aqueoussolution of glucose is

a) Zero b) 1.0

c) 1.5 d) 2.0

206. van't Hoff factor more than unity indicates thatthe solute in solution has

a) dissociated

b) associated

c) both

d) cannot say anything

207. The van't Hoff factor (z) for a dilute solution ofK

3[Fe(CN)

6] is

a) 10 b) 4

c) 5 d) 0.25

208. van't Hoff factor for 0.1 M ideal solution is

a) 0.1 b) 1

c) 0.01 d) none of the three.

209. Which salt may show the same value of van'tHoff factor (i) at that of K

4Fe(CN)

6 in very dilute

solution state

a) A12(SO

4)

3b) NaCI

c) Al(NO3)

3d) Na

2SO

4

210. The experimental molecular mass of anelectrolyte will always be less than its calculatedvalue because the value ofvan't Hoff factor 'i' is:

a) less than 1 b) greater than 1

c) equivalent to 1 d) zero

211. The ratio of the value of any colligative propertyis KCI solution to that of AlCl

3 solution is:

a) 1 b) 0.5

c) 2 d) 4

NUMERICALS

I. Types of Solution and way of Expressing

Concentration

212. A solution has an osmotic pressure of8.314 Pa at300 K. It's concentration would be :

a) 0.056 M b) 0.56 M

c) 0.0034 M d) 0.034 M

213. In a solution of 7.8 g benzene (C6H

6 ) and 46.0 g

toluene (C6H

5CH

3) the mole fraction of benzene is :

a) 1/6 b) 1/5

c) 1/2 d) 1/3

214. An aqueous solution of urea containing 18g ureain 1500 cm3 of the solution has density equal to1.052. If the molecular mass of urea is 60, thenthe molality of the solution is

a) 0.200 b) 0.192

c) 0.100 d) 1.200

215. The mole fraction of water in a solution containing50 g of water and 50 g of ethyl alcohol is :

a) 50

50 50b)

18

18 46

c)1.09

1.09 2.78d)

2.78

1.09 2.78





216. The molarity o.f an aqueous solution of NaOHcontaining 8 g in 2 litre of the solution is

a) 0.1 M b) 0.2 M

c) 0.25 M d) 0.15 M

217. A solution containing 3.01 ×1023 HCI moleculesis diluted to a volume of 4 litres. The molarconcentration of the solution is

a) 1M b) 2 M

c) 0.125 M d) 0.25 M

218. 100 mL of 0.1 M solution of solute A are mixedwith 200 mL of 0.1 M solution of solute B. If Aand B are non-reacting substances, the molarityof the final solution will be

a) 0.3 M b) 0.4 M

c) 0.1 M d) 0.15 M

219. An aqueous solution of glucose is 10 % instrength. The volume in which 1 gm mole of it isdissolved will be

a) 18 litres b) 9 litres

c) 0.9 litres d) 1.8 litres

220. Mole fraction of glucose in 18 % (wt./wt.)solution of glucose is

a) 0.18 b) 0.1

c) 0.017 d) 0.021.

221. The molality of a solution having 18 g of glucose(Molar mass = 180 ) dissolved in 500 g of water is :

a) 1 m b) 0.5 m

c) 0.2 m d) 2 m

222. At 40°C the vapour pressure in torr, of methylalcohol - ethyl alcohol solution is represented bythe equation. P = 119X

A + 135 where X

A is

molefraction of methyl alcohol then the value of

A 1

A

XA

Plim

Xis

a) 254 torr b) 135 torr

c) 119 torr d) 140 torr

223. 150 mL of C2H

5OH (density = 0.78 g mL-1) is

diluted to one litre by adding water; molality ofthe solution is

a) 2.54 b) 11.7

c) 2.99 d) 29.9

224. 50 g. of a solute is dissolved in 0.95 kg. of thesolvent. The mass percent of the solution is

a) 5 b) 0.90

c) 0.52 d) 0.090

225. A solution is 0.25 % by mass. the weight ofsolventcontaining 1.25 g of solutes would be

a) 506 g b) 498.75 g

c) 580.25 g d) 581.25 g

226. The mole fraction of C2H

5OH (Molar mass =

46) in 5 molal aqueous ethyl alcohol solution is

a) 0.0826 b) 0.826

c) 5 d) 5

55.55227. A sugar syrup of weight 2.14.2 grams contains

34.2 grams of water. The molal concentration is

a) 0.55 b) 5.5

c) 55 d) 0.1.

228. To a 4L of 0.2 M solution of NaOH, 2L of 0.5 MNaOH are added. The molarity of resultingsolution is :

a) 0.9 M b) 0.3 M

c) 1.8 M d) 0.18 M.

229. 0.115 g of pure sodium metal was dissolved in500 mL distilled water. The normality of the abovesolution would be

a) 0.010 N b) 0.0115 N

c) 0.023 N d) 0.046 N

230. 200 g. of 5 solution (by mass) of the solute A ismixed with 300 g. of a 10 % solution (by mass)of solute B. The mass percent of A and B in themixtures are respectively

a) 3 and 5 b) 5 and 10

c) 2 and 6 d) 6 and 12

231. Equal volumes of 10 % solution (by wt) of thesolute A and 15% solution (by wt) of the soluteB are mixed. The mass percent of A and B inthe mixture would be respectively

a) 5 and 7.5 b) 10 and 25

c) 5 and 10 d) 20 and 30

232. 400 cm3 of water is added to 6 % of 600 g (molarmass = 36) of a solute. The molarity of solutionis

a) 3 b) 1.5

c) 0.25 d) 1

233. Volume of 0.2 M H2 SO

4 solution containint 20

millimoles of the solute is

a) 10 cm3 b) 100 cm3

c) 20 cm3 d) 200 cm3

234. The volume of 95 % H2SO

4(density = 1.85 g

cm-3) needed to prepare 100 cm3of 15 % solutionof H

2SO

4 (density = 1.10 g cm3) will be

a) 5 cc b) 7.5 cc

c) 9.4 cc d) 12.4 cc

235. Concentrated sulphuric acid is approximately 18molar. 5 cc of it are added to make 500 cc of thesolution. The approximately normality ofthesolution will be





a) 0.18 b) 0.09

c) 0.36 d) 0.27.

236. 2 mole of ehtanol is dis olved in 8 mole ofwater.The mole fraction of water in the solution is

a) 0.2 b) 0.8

c) 0.4 d) 0.1

237. 92 g. of ethanol is dissolved in 108 g. of water.The mole fraction of ethanol in the solution is

a) 0.25 b) 0.75

c) 0.50 d) 0.35

238. 1dm3 ofwater contains 90 g. ofglucose. The molefraction of glucose in the solution is

a) 0.33 b) 0.66

c) 0.5/56.05 d) 0.5/55.55

239. The number of moles of hydroxide (OH-) ion in0.3 litre of 0.005 M solution ofBa (OH)

2is

a) 0.0075 b) 0.0015

c) 0.0030 d) 0.0050240. Rectified spirit contains 95 % ethanol by mass.

The mole fraction of ethanol will be

a) 0.881 b) 0.99

c) 0.118 d) 0.81.

241. The molarity of pure water is

a) 55.6 b) 50

c) 100 d) 18.

242. If 18 g of glucose (C6H

12O

6) is present in 1018 g

of an aqueous solution of glucose, it is said to be

a) 1 molal b) 1.1 molal

c) 0.5 molal d) 0.1 molal.

243. The number of iodine atoms (N) present in 1 ern"of its 0.1 M solution is

a) 6.02 × 1023 b) 6.02 × 102

c) 6.02 × 1019 d) 1.204 ×1020

244. The mole fraction of a solute in its solution inacetic acid is 0.2. The mass of solute (molar mass= 40) in 120 g. of acetic acid would be

a) 2g b) 8gc) 10 g d) 20 g

245. 4.9 g of H2SO

4 is present in 500 cm3 of the

solution has molarity.

a) 0.2 b) 0.1

c) 0.01 d) 0.02

246. A centi-molar solution is diluted 10 times. Themolarity would become

a) 1

10b)

1

100

c) 1

1000d)

1

1

247. What is the molarity of H2SO

4 solution that has a

density 1.84 gm / cc at 35°C and contains 98 %H

2SO

4 by weight?

a) 4.18M b) 8.14M

c) 18.4M d) 18 M.

248. A l L of water sample has 0.1 g fluorideconcentration. What is the concentration offluorine in terms of ppm level?

a) 250 b) 100

c) 400 d) 1000.

249. If 20 g. of sodium hydroxide is dissolved in 1 dm3

of water, the molarity of the solution will be

a) 0.5 b) 0.25

c) 0.1 d) 0.2

250. The volume of water of be added to 50 ems of adecimolar solution to convert it to a centimolarsolution will be

a) 500 cm3 b) 450 cm3

c) 400 cm3 d) 100 cm3

251. 30 g. of acetic acid is dissolved in 1 dm3of asolvent. The molality ofthe solution will be (Given,density of solvent = 1.25 g cm-3)

a) 0.40 b) 0.35

c) 0.55 d) 0.25

252. If the density of a solvent is greater than 1kg.dnr",then the molarity (M) and molality (m) are relatedas

a) M > m b) m > M

c) m = M d) none of these

253. For a solution of dibasic acid the molarity (M)and normality (N.)are related as :

a) N = M / 2 b) 2 M = N

c) M = N d) M > N

254. The molality of a 1molar solution will be (Given,density of solvent = 1.5 kg. dm-3)

a) 1.5 b) 1

c) 0.66 d) 10.72

255. If the density ofthe solvent is 2.5 kg dm-3.The 2molal solution of a solute in this solvent will be

a) 5.M b) 2.5 M

c) 4M d) 1.25M

256. The molarity of solution obtained by mixing 800mL of 0.5 M HCI and 200 mL 1.6M HCI will be

a) 0.72 b) 0.36

c) 1.2 d) 2.1

257. A solution CaCl2 is 0.5 mol/litre, then the moles

of chloride ions in 500 mL will be

a) 0.25 b) 0.50

c) 0.75 d) 1.00





258. A molar solution that which contains one mole ofsolute in

a) 1000 g of solution

b) 1000 g of solvent

c) 1 litre of solution

d) 1 mL of solution

259. Mole fraction of glycerine in a solution of 36 g.of. water and 40 g of glycerine is (M. Wt ofglycerine = 92)

a) 0.2 b) 0.8

c) 0.46 d) 0.36

260. An X molal solution of a compound in benzenehas mole fraction of solute equal 0.2. The valueof X is

a) 14 b) 3.2

c) 0.46 d) 2.0

261. To 100 ml of a 0.5 M solution, 400 ml of water isadded, the final molarity would be

a) 0.125 `b) 0.1

c) 0.25 d) 0.15

262. 800 ml of 0.1 MH2SO

4 is mixed with 200 ml of

0.8 MH2SO

4The molarity of the mixture is

a) 0.32 b) 0.24

c) 0.12 d) 0.48

263. How many grams of CHpH would have to beadded to water to prepare 150 mL of a solutionthat is 2.0 M CH

3OH ?

a) 9.6 b) 2.4

c) 9.6 × 103 d) 4.3 x 102

264. If the density of pure water is 0.999 g cm3.Themolarity of pure water will be

a) more than 55.5 b) less than 55.5

c) equal to 55.5 d) equal to 1

265. The wt. of unhydrous sodium carbonate neededto prepare 500 ml of a decinormal solution wouldbe

a) 5.3 g b) 10.6 g

c) 1.06 g d) 2.65 g

266. The molarity of a 10 % NaOH solution is

a)2.5 b) 0.5

c) 0.25 d) 0.05

267. The amount of oxalic acid (Molar mass 63)required to prepare 500 mL of its 0.10 N solutionis

a) 0.315 g b) 3.150 g

c) 6.300 g d) 63.00 g

268. 120 g of urea is present in 5 L of solution, theactive mass of urea is

a) 0.2 b) 0.06

c) 0.4 d) 0.88

269. The number of moles of solute present in 2 dm3

of 0.5 M solution is

a) 2 b) 1

c) 0.5 d) 0.25

270. The mole of fraction of nitrogen, in a mixture of7 g of N

2 and 16 g of O

2 is

a) 0.5 b) 0.75

c) 0.66 d) 0.33

271. The wt. percent of the solute in a solution is 20.The volume of solvent containing 60 g of solute(d = 1.2 g/cc)

a) 0.24 dm3 b) 0.12 dm3 .

c) 1.2 dm3 d) 0.2 dm3

272. The molarity of in the solution after 2 litres of 3MAgNO

3 is mixed with 3 litres of 1M BaCl

2 is

a) 1.2M b) 1.8M

c) 0.5 M d) 0.4 M

273. 0.2 mole of HCI and 0.1 mole of calcium chloridewere dissolved in water to have 500 mL ofsolution.The molarity of CI- ions, in the solution is

a) .04M b) 0.8 M

c) 0.4M d) 0.08 M

II. Henry's Law

274. What is the concentration of dissolved oxygen at25°Cat 1atm pressure if partial pressure ofoxygenis 0.22 atm? (K

H= 1.3x 10-3mol dm-3atm -1)

a) 2.86 ×10-4M b) 5.9 × 10-3M

c) 1.7 × 10-3M d) 0

275. The millimoles of N2 gas that will dissolve in 1L

of water at 298 K when H2 is bubbled through

water and has a partial pressure of 0.96 bar willbe (Given that at 298 K

H = 76.8 k bar)

a) 0.85 b) 0.693

c) 0.981 d) 0.453

276. The mole fraction of saturated solution is 1.2 x10-6.The pressure ofthe above the solution is (K

H

= 1.44.97 bar)

a) 0.174bar b) 17.4bar

c) 27.4 bar d) 0.274 bar

277. N2 exerts a pressure of 0.987 bar. The mole

fraction of N2, is (K

H= 74.48 kbar)

a) 7.648 x 10-3 b) 9.87 x 10-5

c) 1.3 x 10-5 d) 2.6 X 10-5

278. KH value for Ar(g) , CO

2(g),CO

2(g), HCHO

(g) and

CH4(g)

are 40.39, 1.67, 1.83 × 10-5 and 0.413respectively. Arrange these gases in the order oftheir increasing solubility.





a) HCHO < CH4 < CO

2< Ar

b) HCHO < CO2< CH4 < Ar

c) Ar < CO2< CH

4 < HCHO

d) Ar < CH4< CO

2< HCHO

279. The solubility of methane in benzene at 298 Kunder 760 mm Hg if K

H= 4.27 X 105 mm Hg is:

a) 1.78 x 10-4 b) 1.78 x 10-5

c) 17.8 x 10-4 d) 1.78 X 10-6

280. Air contain O2 and N

2 in the ratio of 1 : 4. The

Henry constant for O2 and N

2 are 3.30 x 107 torr

and 6.60 ×107 torr respectively. Ratio of solubilityof O

2 and O

2 dissolved in water at atmospheric

pressure and room temperature is

a) 1 : 4 b) 4 : 1

c) 1: 2 d) 2 : 1

III. Lowering of Vapour Pressure and Raoult's

Law

281. Water and chlorobenzene are immiscible liquids.Their mixture boils at 90°C under a reducedpressure of 9.58 ×104 Pa. The vapour pressureof pure water at 90°C is 7.03 ×104Pa andmolecular mass of chlorobenzene is 112.5 Onwhat percent basis, cholorobenzene in thedistillate is equal to:

a) 50 b) 60

c) 70 d) 80

282. The vapour pressure of benzene at a certain temp.is 640 mm Hg. Anon-volatile-non-electrolyte solidweighing 2.175 gisadded to 39.0 gofbenzene. Thevapour pressure ofthe solution is 600mm Hg.Whatis the molecular mass of the soild substance?

a) 6.96

b) 65.3

c) 63.8

d) none of the above.

283. Liquid A and B form an ideal solution. Ifvapourpressure of pure A and Bare 500 Nm-2 and 200Nm-2 respectively, the vapour pressure of asolution ofA in B containing 0.2 mole fraction ofA would be

a) 700 Nm-2 b) 300 Nm-2

c) 260 Nm-2 d) 140 N m-2

284. The vapour pressure of pure benzene and tolueneare 160 and 60 torr respectively. The molefraction of toluene in vapour phase in contact withequimolar solution of benzene and toluene is

a) 0.50 b) 0.6

c) 0.27 d) 0.73

285. The ratio of the value of any colligative properly

for KCIsolution to that for sugar solution is nearly.......... times:

a) 1 b) 0.5

c) 2 d) 2.5

286. 6 g urea is dissolved in 90 g water. The relativelowering of vapour pressure is equal to:

a) 0.0196 b) 0.06

c) 1.10 d) 0.0202

287. Vapour pressure of CCl4, at 25°C is 143mm Hg.

0.5 g of a non-volatile solute (mol. wt. 65) isdissolved in 100 cm-3of CCl

4.Find the vapour

pressure of the solution. (Density of CCl4, = 1.58/

cm3).

a) 141.93 mm b) 94.39 mm

c) 199.34 mm d) 143.99 mm

288. The vapour pressure ofbenzene at 90°Cis 1020torr. A solution of 5 g of a solute in 58.5 g benzenehas vapour pressure 990 torr. The M.Wt. of soluteis:

a) 78.2 b) 178.2

c) 206.2 d) 220

289. The vapour pressure of ethanol and methanol a42.0 mm and 88.5 mm Hg respectively. An idealsolution is formed at the same temperature mixing46.0 g of ethanol with 16.0 g of methanol. Themole fraction of methanol in the vapour is

a) 0.467 b) 0.502

c) 0.513 . d) 0.556

290. One molar solution of sodium chloride will hasthe relative lowering of vapour pressure close to:

a) 5.8% (wt./vol) urea solution

b) 5.8% (wt./vol)glucose solution

c) 1.0 M glucose solution

d) 2.0 M urea solution

291. 34.2 g of canesugar is dissolved in 180 g of water.The relative lowering of vapour pressure will be

a) 0.0099 b) 1.597

c) 0.840 d) 0.9901

292. The vapour pressure of a pure liquid A is 70 torrat 27°C. It forms an ideal solution with anotherliquid B. The mole fraction of B is 0.2 and totalvapour pressure ofthe solution is 84 torr at 27°C.The vapour pressure of pure liquid B at 27°C.

a) 14 b) 56

c) 140 d) 70

293. At 88°C benzene has a vapour pressure of 900torr and toluene'has a vapour pressure of 360 torr.What is the mole fraction of benzene in themixture with toluene that will boil at 88°C at 1





atm pressure, benzene-toluene form an idealsolution:

a) 0.416 b) 0588

c) 0.68 d) 0.74

291. The relative lowering of vapour pressureproduced by dissolving 71.5 g of substance in1000 g of water is 0.0173. The molecular massof the substance will be:

a) 74.39 b) 18.0

c) 342 d) 60

295. The vapour pressure of water at roomtemperature is 23.8 mm Hg. The vapour pressureof an aqueous solution of sucrose with molefraction 0.1 is equal to

a) 2.9 mm Hg b) 24.2 Hg

c) 21.42 mm Hg d) 21.44 mm Hg.

296. The vapour pressure of two pure liquids (A) and(B) are 100 and 80 torr respectively. The totalpressure of solution obtained by mixing 2 mole of(A) and 3 mole of (B) would be:



297. Vapour pressure of CC14 at 25°C is 143 mm Hg.

0.5 g of a non-volatile solute (Molar mass 65) isdissolved in 100 cm3 of CC1

4 Find the vapour

pressure of the solution. (Density of CCl4 = 1.58/

cm3).

a) 141.93 mm b) 94.39 mm

c) 199.34 mm d) 143.99 mm.

298. An ideal solution was obtained by mixing methanoland ethanol. If the partial vapour pressure ofmethanol and ethanol are 2.619 × kP

a and a 4.556

kPu.respectively, the composition of vapour (interms of mole fraction) will be:

a) 0.635 MeOH, 0.365 EtOH

b) 0.365 MeOH, 0.635 EtOH

c) 0.574 MeOH, 0.326 EtOH

d) 0.173 MeOH, 0.827 EtOH

299. The vapour pressure of a solvent decreased by10mm of Hg when a non-volatile solute wasadded to the solvent. The mole fraction of solute.In solution is 0.2, what would be the mole fractionof solvent if decrease in vapour pressure is 20mm of Hg:

a) 0.8 b)0.6

c) 0.4 d) 0.2

300. The vapour pressure of solution of 5 g of non-electrolyte in 100 g of water at a particulartemperature is 2985 Nm-2. The vapour pressureof pure water at the temperature is 3000 Nm-2.

The molecular mass of the solute is

a) 180 b) 90

c) 270 d) 200

IV. Boiling Point Elevation

301. The molal elevation constant of water = 0.52K.molality:'. The boiling point of 1.0molal aqueousKCI solution (assuming complete dissociation ofKCI) should be:

a) -273.04 K b) 374.04 K

c) 37.404 K d) 273 K

302. The boiling point of a water containing nonvolatilesolute is 101.04°C of 2 molal solution, theebullioscopic constant of water is

a) 0.52 K . kg mol-1 b) 1.04 K . kg mol-1

c) 10.4 K . kg mol-1 d) 5.2 K . kg mol-1

303. An aqueous solution containing 1 g of urea boilsat 100.25°C. The aqueous solution containing 3 gof glucose in the same volume will boil at

a) 100.75°C b) 100.5°C

c) 100°C d) 100.25°C

304. At certain hill-station, pure water boils at99.725°C. If K

b, for water is 0.513°C kg mol",

the boiling point of 0.69 m solution of urea will be

a) 100.079°C b) 103°C

c) 100.359°C d) unpredictable.

305. Elevation in boiling point was 0.52°C when 6 g ofa compound X was dissolved in 100 g of water.Molecular mass X is: (K

b = 5.2 mol-1 100 g HP)

a) 120 b) 60

c) 180 d) 342

306. The molal elevation constant for water is 0.52 Kmolality-1 The elevation caused in the boiling pointof water by dissolving 0.2.5 mole of a non volatilesolute in 250 g of water will be:

a) 52°C b) 5.2°C

c) 0.52°C d) 0.052°C

307. The molal elevation constant for water is 0.56°Cper kg ofwater. The boiling point of solution madeby dissolving 6.0 g of water (NH

2CONH

2) in 200

g of water is

a) 10.028°C b) 100.28°C

c) 50.14°C d) none of these

308. Y g of non-volatile organic substance ofmolecularmass M is dissolved in 250 g benzene. Molalelevation constant of benzene is K

b Elevation in

its boiling point is given by: M 4KbY

a) b

M

K Y b)b4K Y

M





c) bK Y

4Md)

bK Y

M

309. The molal boiling point constant of water is0.53°C. When 2 mole of glucose are dissolved in4000 g of water, the solution will boil at:

a) 100.53°C b) lO1.06°C

c) 100.265°C d) 9.47°C

310. A solution containing 3.3 g of a substance in 125g ofbenzene (b.p 80°C) boils at 80.66°C. If K

b

for one litre of benzene is 3.28°C, the molecularmass of the substance shall be

a) 127.20 b) 131.20

c) 137.12 d) 142.72

311. The boiling point of an aqueous solution of anonvolatile solute is 100. 15°C. What is thefreezing point of an aqueous solution obtained bydiluting the above solution with an equal volumeof water? The values of K

b and K

f, for water are

0.S12°C and 1.86°CK molality-l.

a) -O.S44°C b) -O.S12°C

c) -.o.272°C d) -1.86°C

312. The boiling point of 0.1 molal aqueous solution ofurea is 100.18°C at 1 atm. The molal elevationconstant of water is

a) 1.8 b) 0.18

c) 18 d) 18.6

313. The 0.1 molal aqueous solution of glucose boilsat 100.16°C. The boiling point of O.S molalaqueous solution of sucrose will be

a) SOO.80°C b) 100.80°C

c) 20.16°C d) 20.8°C

314. The molal b.p. constant for water is 0.513°C kgmol-1. When 0.1 mole of sugar is dissolved in 200g of water, the solution boils under a pressure of1 atm at

a) 100.S13°C b) 100.0S13°C

c) 100.256°C d) 101.02SoC

315. For a solvent Kb = S kg mol-1 using this solvent,

the solution records the elevation of boiling pointof O.soC.The molality of the solution is

a) 0.2S b) 0.1

c) 10 d) unpredictable

316. If the elevation in boiling point of a solution of 10gm of solute (mol. mass = 100) in 100 gm of water

is Tb the ebullioscopic constant of water is

a) 10 b) 10 Tb

c) Tb

d) Tb /10

V. Freezing Point Depression

317. The freezing point of 0.1 M solution of glucose is-1.86°C. If an equal volume of 0.3 M glucosesolution is added, the freezing point of the mixturewill be

a) -7.44°C b) -5.S8°C

c) -3.72°C d) -2.79°C

318. Pure benzene freezes at 5.45°C at a certain placebut a 0.374 m solution of tetrachloroethane inbenzene freezes ar 3.SSoC.The Krfor benzeneis

a) 5.08 K kg mol-1 .

b) 508 K kg mol-1

c) 0.508 K kg mol-1

d) 5O.8°C kg mol-1

319. The freezing point of a O.OSmolal solution of anon-electrolyte in water is : (K

f= 1.86 Kmolality:')

a) -1.86°C b) -O.93°C

c) -O.093°C d) 0.093°C

320. The freezing point of 1 molal NaCI solutionassuming NaCI to be 100%dissociated in wateris : (K

f,= 1.86 K molality-1)

a) -1.86°C b) -3.72°C

c) +1.86°C d) +3.72°C

321. An aqueous solution of a non-electrolyte soluteboils at 100.52°C. The freezing point ofthe solutionwill be (K

f,= 1.86 K kg mol-1, (K

b = 0.52 K kg

mol-3)

a) O°C b) -1.86°C

c) 1.86°C d) none of the above.

322. Molal depression of freezing point of water is1.86° per 100 g of water. 0.02 mole of ureadissolved in 100 g of water will produce alowering of tempreature of:

a) 0.186° b) 0.372°

c) 1.86° d) 3.72°

323. What would be the freezing point of aqueoussolution containing 17 g of C

2H

5OH in 1000 g of

water (KfH

2O = 1.86 K molality-1)?

a) 272.31 K b) 273.69 K

c) 273 K d) 27.36 K

324. A solution of 1.5 g of non-electrolyte in 20 g ofwater freezes at 271.94 K. If K

f = 1.86 K kg

mol:' then the molecular mass of the solute willbe

a) 179.97 g mol-1 b) 207.8 g mol-1

e) 309.6 g mol-1 d) 109.6 g mol-1

325. A 0.5 molal solution of ethylene glycol in water isused as coolant in a car. If the freezing point





constant of water be 1.86°C per mole, the mixtureshall freeze at

a) 0.93°C b) -O.93°C

c) 1.86°C d) -1.86°C

326. A solution of 1.25 g of a non-electrolyte in 20 gof water freezes at 271.94 K. If K

f= 1.86

Kmolality-1 then the molecular wt. of the soluteis:

a) 207.8 g/mol b) 179.79 g/mol

c) 209.6 g/mol d) 109.6 g/mol

327. A solution containing 1 mole of ethylene glycoldissolved in 1000 g of water (K

f, = 18.6 K molality-

1) will freeze at:

a) 273 K b) 2.544 K

c) 254.4 K d) 25.44 K

328. What is the molality of ethyl alcohol (molar mass= 46) in aqueous solution which freezes at-10°C:(K

f for water = 1.86 K molality-1)

a) 3.540 b) 4.567

c) 5.376 d) 6.315

329. The molal depression constant for a solvent is4.9. The depression in freezing point for amillimolal solution of a non-electrolyte in thesolvent is

a) 0.49 b) 4.9

c) 4.9 + 0.001 d) 0.0049.

330. The amount of urea to be dissolved in 500 mL ofwater (K = 18.6 K mol-1 100 g solvent) to producea depression of 0.186°C in freezing point is:

a) 0.3 g b) 3 g

c) 6 g d) 9 g

331. The molecular mass of NaCI determined bystudying freezing point depression of it's 0.5%aqueous solution is 30. The apparent degree ofdissociation of NaCI is:

a) 0.95 b) 0.50

c) 0.60 d) 0.30

332. The depression in f.pt. of 0.01 m aqueous solutionof urea, sodium chloride and sodium sulphate isin the ratio:

a) 1 : 1 : 1 b) 1 : 2 : 3

c) 1 : 2 : 4 d) 2 : 2 : 3

333. 20 g of a binary electrolyte (mol. wt. = 100) aredissolved in 500 g of water. The freezing point ofthe solution is -0.74°C, K

f, = 1.86 K molality-1

The degree of ionization of the electrolyte is:

a) 50% b) 75%

c) 100% d) Zero

334. An aqueous solution freezes at-O.186°C (Kf=

1.86°; Kb = 0.512°). What is the elevation in boiling

point?

a) 0.186 b) 0.512

c) 0.152/1.86 d) 0.0512

335. The freezing point of a solution prepared from1.25 g of non-electrolyte and 20 g of water is271.9 K. If molar depression constant is .86 Kmol-1 then molar mass of the solute will be:

a) 105.7 b) 106.7

c) 115.3 d) 93.9

336. A 0.2 molal aqueous solution of a weak acid HX)is 20 percent ionised. The freezing point of thissolution is (K

f, = 1.86 Kim for water)

a) -O.45°C b) -0.90°C

c) -O.31°C d) -O.53°C

337. The freezing point of aqueous solution thatvcontains 5% by mass urea, 1.0% by mass KCIand 10% by mass of glucose is: (K

f,H

2O = 1.86

K molality-1)

a) 290.2 K b) 285.5 K

c) 269.93 K d) 250 K

338. The values of Kf for solvents, P, Q, R and S are

1.86, 1.99, 5.12 and 4.7 kg mol-1 resp. Theequimolal solutions of a solute in these solventswill have the freezing point in order of solvents

a) R> S > Q > P b) P> R> S > Q

c) P > Q > S > R d) R > Q > P > S

339. The solutions containing 6 g of urea (molecularmass = 60) per dm3 of water and anothercontaining 9 g of solute A per dm3 of water freezeat the same temp. The molecular mass of A is

a) 120 b) 90

c) 54 d) 150

340. If 15 gm of a solute in 100 gm of water makes asolution that freezes at -1.0°C, then 30 gm of thesame solute in 100 gm of water will make asolution the freezes at

a) -0.5°C b) -2.0°C

b) 0°C d) 2.0°C

341. How many grams of sucrose (Molar mass = 342)should be dissolved in 100 I? water in order toproduce a solution with a 105.0°C differencebetween the freezing point and the boilingtemperatures? (K

f = 1.86 C/m, K

b 0.51°C/m)

a) 34.2 g b) 72 g

c) 342 g d) 460 g.

342. The percentage composition by mass of anaqueous solution of a solute (molecular mass 150)which boils at 373.26 is (Kb = 0.52)





a) 5 b) 15

c) 7 d) none of the above.

343. 8g ofHBr is added in 100 g of H2O. The freezing

point will be (Kf, = 1.86, H = 1, Br = 80)

a) -O.75°C b) O°C

c) -3.67°C d) -7.6°C

VI. Osmosis and Osmotic Pressure

344. Osmotic pressure of blood is 7.65 atm at 310 KAn aqueous solution of glucose that will beisotonic with blood is wt.lvol:

a) 5.41% b) 3.54%

c) 4.53% d) 53.4%

345. The osmotic pressure of a solution at O°C is 4atmospheres. What will be its osmotic pressureat 546 K under similar conditions?

a) 4 atm. b) 2 atm.

c) 8 atm. d) 1 atm.

346. The osmotic pressure in atmospheres of 10%solution of cane sugar at 69°C is

a) 724 b) 824

c) 8.21 d) 7.21

347. The osmotic pressure of 0.2 molar solution of ureaat 27°C is en = 0.082 litre atm mol-1K-1) is

a) 4.92 atm b) 1 atm

c) 0.2 atm d) 27 atm.

348. The osmotic pressure of a 5% (wt.lvol.) solutionof cane sugar at 150°C is (Molar mas = 342)

a) 4 atm b) 3.4 atm

c) 5.078 atm d) 2.45 atm

349. Osmotic pressure of a solution containing 0.1 moleof solute per litre at 273 K is

a)0.1

1 × 0.082 × 273 atm

b) 0.1 × 2 × 0.082×273 atm

c)1

0.1× 0.082 × 273 atm 0.1 273

d)0.1

1×

273

0.082 atm

350. Osmotic pressure of 40% (wt.lvol.) urea solutionis 1.64 atm and that of 3.42% (wt./vol.) canesugar is 2.46 atm. When equal volumes of theabove two solutions are mixed, the osmoticpressure of the resulting solution is

a) 1.64 atm b) 2.46 atm

c) 4.10 atm d) 2.05 atm

351. Following solutions at the same temperature willbe isotonic.

a) 3.42 g of cane sugar in one litre water and0.18 g of glucose in one litre water

b) 3.42 g of cane sugar in one litre water and0.18 g of glucose in 0.1 litre water

c) 3.42 g of cane sugar in one litre water and0.585 g of NaCI in one litre water

d) 3.42 g of cane sugar in one litre water and1.17 g of NaCl in one litre water

352. 0.6 g of a soluts is dissolved in 0.1 litre of a solventwhich develops an osmotic pressure of 1.23 atmat 27°C. The molecular mass of the substance is

a) 149.5 g mol-1 b) 120 g mol-1

c) 430 g mol-1 d) None.

353. The osmotic pressure of decimolar solution ofglucose at 30°C is:

a) 24.88 atm b) 2.488 atm

c) 248.8 atm d) 2488 atm

354. Osmotic pressure of a solution of a solution(density is 1 g/mL) containing. 3 g of glucose(molecular mass = 180) in 63 g of water at 15°Cis: (R = 8.314 J K-l mol-1)

a) 41.570 kPa

b) 415.70 kPa

c) 41570 kPa

d) 4157kPa

355. 100 cc of 1.5% solution of urea is found to haveosmotic pressure of 6.0 atm and 100 cc of 3.42%solution of cane sugar is found to have an osmoticpressure of2.4 atm. If the two solutions are mixedthe osmotic pressure of the resulting solution willbe

a) 8.4 atm b) 4.2 atm

c) 16.8 atm d) 2.1 atm.

356. A solution containing 8.6 g urea in one litre wasfound to be isotonic with a 5%(wt./vol.) solutionof an organic non-volatile solute. The molecularmass of latter is:

a) 348.9 b) 34.89

c) 3489 d) 861.2

357. A solution containing 4 g of a non-volatile organicsolute per 100 mL was found to have an osmoticpressure equal to 500 em of mercury at 27°C.The molecular mass of solute is:

a) 14.97 b) 149.7

c) 1697 d) 1.497

358. If a 6.08%(wt./vol) solution of cane sugar (molarmass = 342) is isotonic with 1.52% (wt./vol)solution of compound B then the molecular massof compound B is:





a) 152 b) 76.5

c) 85.5 d) 180

359. What is the volume of solution containing 1 g moleof sugar that will give rise to an osmotic pressureof 1 atm at S.T.P.?

a) 224.0 litre b) 22.4 litre

c) 2.24 litre d) none of the above.

360. Osmotic pressure of a sugar solution at 27°C is2.46 atmosphere. The concentration of thesolution in mol per litre is:

a) 1M b) 0.01 M

c) Q.0125M d) 0.1 M

361. 1 litre of a solution containing 500 g of a proteinexerts an osmotic pressure of 0.82 atm at 27°C.The molecular mass of the protein is:

a) 82000 b) 50000

c) 41000 d) 15000

362. Osmotic pressure is 0.0821 atm at a temperatureof 300 K. Find concentration in molellitre

a) 0.033 b) 0.066

c) 0.33 x 10-2 d) 3.

363. The concentration of glucose (in g/litre) solutionwhich is isotonic with a solution of urea containing6 g per litre will be:

a) 6 b) 34.2

c) 18 d) 1.8

364. Solute A is a ternary electrolyte and solute B isnon-electrolyte. If 0.1 M solution of solute Bproduces an osmotic pressure of 2P, then 0.05 Msolution of A at the same temperature willproduces an osmotic pressure equal to:

a) P b) 1.5 P

c) 2 P d) 3 P

365. A 3.42%(wt./vol.) solution of cane sugar isisotonic with a 5.96% (wt./vol.) solution ofraffinose. The molecular mass of raffinose is:

a) 59.6 b) 596

c) 5.96 d) 5960

366. The osmotic pressure of a solution containing 4.0g solute (molar mass = 246) per litre at 27°C is(R = 0.082 1 atm. mol-1 K)

a) 0.1 atm b) 0.4 atm

c) 0.2 atm d) 0.8 atm

367. The vapour pressure of benzene at 80°C islowered by 10 mm by dissolving 2 g of anonvolatile substance in 78 g of benzene. Thevapour pressure of pure benzene at 80°C is 750mm. The moelcular mass of the substance willbe

a) 15 b) 14.8

c) 1500 d) 148

368. A solution containing 500 g of a protein per litreis isotonic with a solution containing 3.42 g ofsucrose per litre. The molecular mass of proteinis

a) 5 b) 146

c) 34200 d) 50000

369. The osmotic pressure a solution at O°Cis 2 atm.What will be its osmotic pressure at 273°C undersimilar conditions

a) 0.5 atm b) 2 × 273 atm

c) 4 atm d) 273/2 atm

370. A solution containing 4 g of polyvinyl chloride inlitre of dioxane was found to have an osmoticpressure of 6 x 10-4atm at 300 K. The molecularmass of the polymer is

a) 3 × 103 b) 16 × 105

c) 5 × 104 d) 6.4× 102

371. The relationship between osmotic pressure at 273Kwhen 10 g glucose (P

1), 10 g urea (P

2) and 10

g sucrose (P3) are dissolved in 250 mL of water.

a) P1> P

2 > P

3c) P

2> P

1 > P

3

b) P3 > P

1 > P

2d) P

2 > P

3 > P

1

372. Insulin (C2H

10O

5) is dissolved in a suitable solvent

and the osmotic pressure ( )of solutions ofvarious concentration (g/cm3) C is measured at20°C. The slope of a plot of against C is foundto be 4.65 ×10-3.The molecular mass of the insulinis

a) 4.8 ×105 b) 9 × 105

c) 3 × 105 d) 5.16 × 106

373. A solution of protein (extracted from crabs) wasprepared by dissolving 0.75 g in 125 cm3 of anaqueous solution. At 4°C an osmotic pressure riseof 2.6 mm of the solution was observed. Thenmolecular mass of protein is (Assume density ofsolution is 1.00 g/cm3)

a) 9.4 × 105 b) 5.4 × 105

c) 5.4 × 1010 d) 9.4 × 1010

374. If 1 is the osmotic pressure of solution containing

6g. of acetic acid per dm3 and 2 that of a solution

containing 5.85 g. of NaCl per dm3 at the sametemperature then

a) 1 2 b) 1 2

c) 1 2 d) 1 22

375. The osmotic pressure (in atm.) of aIM solution anon-electrolyte at O°Cwill be





a) 1 atm b) 22.4 atm

c) 0.0821 atm d) 76 atm

376. The osmotic pressure of a 0.5 M solution of NaClat 0°C will be

a) 11.2 atm

b) less than 11.7 atm

c) more than 11.2 atm

d) unpredictable

377. Solute A is a ternary electrolyte and solute B is anon-electrolyte. If 0.1 M solution of solute Bproduces an osmotic pressure of 2 P, then 0.05M solution of A at the same temperature willproduce an osmotic pressure equal to

a) 1.5 P b) 2 P

c) 3 P d) P

378. Which compound corresponds to van't Hofffactorvalue (i) to be equal to 2 for dilute solution

a) K2SO

4b) NaHSO

4

c) Sugar d) MgSO4

379. The values of observed and calculated molecularmasses of silver nitrate are 92.64 and 170respectively. The degree of dissociation of silvernitrate is

a) 60% b) 83.5%

c) 46.7% d) 60.23%

VII. Association and Dissociation

380. The values of observed and calculated molecularmasses of silver nitrate are 92.64 and 170respectively, The degree of dissociation of silvernitrate will be

a) 60% b) 83.5%

c) 46.7% d) 60.32%

381. The values of observed and calculated molarmasses of Ca(NO

3)

2 are respectively 65.6 and

161. The degree of dissociation of calcium nitratewill be

a) 25% b) 50%

c) 75% d) 60%

382. Van't Hoff factor of very dilute solution ofCa(NO

3)

2 is

a) 1 b) 2

c) 3 d) 4

383. KBr is 80% dissociated in solution. The freezingpoint of a 0.5 molal solution is (K

f water = 1.86°C/m)

a) 273 K b) 277 K

c) 271.326 K d) 269 K

384. The degree of dissociation ( ) of a weak

electrolyte AxB

y is related to van't Hoff factor (i)

by the x y expression

a)1

(x y 1)

i

b)1

(x y 1)

i

c)x y 1

1

i

d)x y 1

1

i

385. Acetic acid exists in benzene solution in thedimetric form. In an actual experiment, the van'tHofffactor was found to the 0.52. Then the degreeof dissociation of acetic acid is

a) 0.18 b) 0.88

c) 0.96 d) 0.52

386. 0.1 molal aqueous solution of sodium bromidefreezes at -0.335°C at atmospheric pressure. Kf

for water is 1.86°C. The percentage ofdissociation ofthe salt in solution is

a) 90 b) 80

c) 58 d) 98

OBJECTIVE TYPE QUESTIONS

1. The molal freezing point for water is 1.86°Cmo-1 If 342 g of cane sugar is dissolved in 1000mL of water the solution will freeze at

a) 1.86°C b) -1.86°C

c) 2.42°C d) -2.42°C

2. The BaCl2 ionises to an extent of 80 %in aqueous

solution, the value ofvan't Hoff factor is

a) 2.6 b) 0.4

c) 0.8 d) 2.4

3. Equal weight of methane and bxygen are mixedin an empty container at 25°C. The fraction ofthe total pressure exerted by oxygen is

a) 1/2 b) 1/3

c) 114 d) 115

4. An aqueous solution is 1.00 molal in K.I. Whichchange will cause the vapour pressure of thesolution of increase ?

a) Addition of NaCl

b) Addition of Na2SO

4

c) Addition of 1.00 molal Kl

d) Addition of water

5. A solution of sucrose (molar mass = 342 g mol-1)has been prepared by dissolving 68.5 g of sucrosein 1000 g of water. The freezing point of the





solution obtained will be

(Kf for water = 1.86 K Kg mol-1)

a) – 0.372°C b) - 0·520°C

c) + 0.372°C d) - 0.570°C

6. If sodium sulphate is considered to be completelydissociated into cations and anions in aqueoussolution, the change in freezing point of water

( Tf) when 0.01 mol of sodium sulphate is

dissolved in 1 kg of water, is

(Kf = 1.86 K kg mol-1)

a) 0.0744 K b) 0.0186 K

c) 0.0372 K d) 0.0558 K

7. If 10-4 dm3 of water is introduced into a 1.0dm-3 flask at 300 K, how many moles of waterare in the vapour phase when equilibrium isestablished ?

(Given: Vapour pressure of H2O at 300 K is 3170

Pa; R = 8.314 JK-l mol-1)

a) 4.46 × 10-2 mol b) 1.27 × 10-3 mol

c) 5.56 × 10-3mol d) 1.53 × 10-2 mol

8. On mixing, heptane and octane form an idealsolution. At 373 K, the vapour pressure of thetwo liquid components (heptane and octane) are105 KPa and 45 kPa respectively. Vapourpressure of the solution obtained by mixing 25.0g of heptane and 35 g of octane will be (molarmass of heptane = 100 g mol-1 and of octane =114 g mol-1)

a) 96.2 k Pa b) 144.5 k Pa

c) 72.0 k Pa d) 36.1 k Pa

9. Kb for water is 0.52 Km-l. Then 0.1 m solution of

NaCl will boil approximately at

a) 100.52°C b) 100.052°C

c) 101.04°C d) 100.104°C

10. 138 g of ethyl alcohol is mixed with 72 g of water.The ratio of mole fraction of alcohol of water is

a) 3 : 4 b) 1 : 2

c) 1 : 4 d) 1 : 4

11. Two solutions of a substance (none-electrolyte)are mixed as - 480 mL of 1.5 M first solution +520 mL of 1.2 M second solution

a) 2.70 M b) 1.344 M

c) 1.50 M d) 1.20M

12. Asolution of 10 g of non-volatile binary electrolyte(molar mass = 100) in 500 g of water freezes at- 0.74°C. What is the degree of ionisat ion ?(K

f of water = 1.85 Km-l)

a) 50 % b) 75 %

c) 100 % d) 0 %

13. Which one of the following in the ratio of thelowering of v.P. of 0.1 M aqueous solution ofBaCl

2, NaCl and Al

2(SO

4)

3 respectively ?

a) 2 : 3 : 5 b) 3 : 2 : 5

c) 5 : 2 : 3 d) 5 : 1 : 2

14. A 0.1 molal aqueous solution of a weak acid is 30% ionized. If Kr for water is 1.86 % C/m, thefreezing point of the solution will be

a) -0.18°C b) -0.54°C

c) -0.36°C d) -0.24°C

15. 200 mL of an aqueous solution of a proteincontains its 1.26 g. The osmotic pressure of thissolution at 300 K is found to be 2.57 × 10-3 bar.The molar mass of protein will be (R = 0.083 Lbar mol-1K-l)

a) 51022 g mol-1 b) 122044 g mol-1

c) 31011 g mol-1 d) 61038 g.mol-1

16. The freezing point depression constant for wateris = 1.86°C m-1. If 5.00 g Na

2SO

4 is dissolved in

45.0 g H2O, the freezing point is changed by

- 3.82°C. Calculate the van't Hoff factor forNa

2SO

4

a) 2.05 b) 2.63

c) 3.11 d) 0.381

17. The van't Hoff factor i for a compound whichundergoes dissociation in one solvent andassociation in other solvent is respectively

a) less than one and greater than one

b) less than one and l ess than one

c) greater than one and less than one

d) greater than one and greater than one

18. Mole fraction of solute in a 1.00 molal aqueoussolution is

a) 0.1770 b) 0.0177

c) 0.0344 d) 1.7700

19. The degree of dissociation ( ) of a weak

electroyte, Ax By is related to van't Hoff factor

(i) by the expression :

a)1

x y 1

i

b)x y 1

1

i

c)x y 1

1

i

d)1

(x y 1)

i





20. Ethylene glycol is used as an antifreeze in a coldclimate. Mass of ethylene glycol which shouldbe added to 4 kg of water to prevent it fromfreezing at - 6°C will be :

[Kf for water = 1.86 K kg mol-1, and molar mass

of ethylene glycol = 62 g mol-1]

a) 204.30 g b) 400.00 g

c) 304.60 g d) 804.32 g

21. A 5.2 molal aqueous solution of methyl alcohol,CH

3OH, is supplied. What is the mole fraction of

methyl alcohol in the solution ?

a) 0.190 b) 0.086

c) 0.050 d) 0.100

22. A 5%solution of cane sugar (molar mass 342) isisotonic with 1% of a solution of an unknownsolute. The molar mass of unknown solute in g/mol is

a) 136.2 b) 171.2

c) 68.4 d) 34.0

23. The molality of a urea solution in which 0.0100 gof urea,[(NH

2)

2CO] is added to 0.3000 dm3

ofwater at STP is

a) 0.555 m b) 5.55 × 10-4 m

c) 33.3 d) 3.33 × 10-2 m

24. Dissolving 120 g of urea (molar mass 60) in 1000g of water gave a solution of density 1.15 g/mL.The molarity of the solution is

a) 1.78M b) 2.00 M

c) 2.05 M d) 2.22 M

25. The freezing point (in °C) of a solution containing0.1 g of K

3[Fe (CN)

6](Mol. Wt. 329) in 100 g of

water (Kf = 1.86 K kg mol-1) is

a) - 2.3 × 10-2 b) - 5.7 × 10-2

c) - 5.7 × 10-3 d) - 1.2 × 10-2

26. The elevation in boiling point of solution of 10 gof solute (Molar mass = 100) in 100 g of water is

bT the the ebullioscopic constant of water is

a)bT

10

b) bT

c) 10 bT d) 100 bT

27. 1.2% NaCl solution is isotomic with 7.2%glucosesolution. What will be the van't Hoff's factor ?

a) 0.5 b) 1

c) 2 d) 6

28. The vapour pressure of two liquids P and Q are80 and 60 torr. respectively. The total V.P. ofsolution obtained by mixing 3 moles of P and 2

moles of Q would be



29. A solution of urea (molar mass = 56) boils at100.18°C at atmospheric pressure. If K

f, and K

b,

for water are 1.86 and 0.512 K. Kg mol-1

respectively. The above solution freezes at

a) -6.54°C b) 6.54°C

c) 0.654°C d) -0.654°C

30. Which one of the following solution has lowestfreezing point ?

a) 0.2 M Na2SO

4b) 0.1 M Urea

c) 0.2 M NaNO3

d) 0.1 M Ba Cl2

31. The weight in grams of a non-volatile solute(molar mass = 60) to be dissolved in 90g of waterto produce a relative lowering of V.P. of 0.02 is

a) 4 b) 8

c) 6 d) 10

32. The density of a solution prepared by dissolving120 g of urea (mol. mass = 60 u) in 1000 g ofwater is 1.15 g/mL. The molarity of this solutionis :

a) 2.05 M b) 0.50 M

c)1.78M d) 1.02M

33. Kf for water is 1.86 Kkg mol-1. If you automobile

radiator holds 1.0 kg of water, how many gramsof ethylene glycol (C

2H6O

2) must you add to get

the freezing point of the solution lowered to- 2.8°C ?

a) 27 g b) 72 g

c) 93 g d) 39 g

34. 29.2% (w/w) HCl stock solution has a density of1.25% g mL. The molecular mass of HCI is 36.5 gmol-1. The volume (ml.) of stock solution requiredto prepare a 200 mL solution of 0.4 MHCl is :

a) 2 mL b) 4 mL

c) 8 mL d) 6 mL

35. For a solution containing 2.5 g of a non-volatilenon-electrolyte solute in 100 g of water, theelevation in boiling point at 1 atm pressure is 2°C.Assuming concentration of solute is much lowerthan the concentration of solvent, the vapourpressure (mm of Hg) of the solution is(take K

b = 0.76 K

kg mol-1)

a) 724 b) 740

c) 736 d) 718

36. PA and P

B are the vapour pressure of pure liquid

components, A and B, respectively of an idealbinary solution. If x

A represents the mole fraction





of component A, the total pressure ofthe solutionwill be

a) PA + X

A (P

B - P

A)

b) PA + X

A (P

A - P

B)

c) PB+ x

A(P

B-P

A)

d) PB + x

A(P

A - P

B)

37. Vapour pressure of chloroform (CHCl3) and

dichloromethane (CH2Cl

2) at 25°C are 200 mm

Hg and 41.5 mm Hg respectively Vapourpressure of the solution obtained by mixing 25.5g or CHCl

3 and 40 g of CH

2Cl

2 at the same

temperature will be (Molecular mass ofCHCl

3 = 119.5 u and molecular mass of

CH2Cl

2 = 85 u)

a) 173.9 mm Hg b) 615.0 mm Hg

c) 347.9 mm Hg d) 90.34 mm Hg

38. The V.P in mm of Hg of an aqueous solutionobtained by adding 18 g of glucose to 180 g ofwater at 100°C

a) 7.60 b) 76.0

c) 759 d) 752.4

39. Which one of the following is an isotonic pair ofsolution ?

a) 0.15 M NaCl and 0.1 M Na2SO

4

b) 0.2 M urea and 0.1 M sugar

c) 0.1 M BaCl2 and 0.2 M urea

d) 0.2 M MgS04 and 0.1 M NH4Cl

40. The molarity of a solution obtained by mixing 750mL of 0.5 (M) HCl with 250 mL of (M) HCl willbe

a) 0.975 M b) 0.875 M

c) LOOM d) 1.75M

41. A solution of sucrose (molar mass = 342 g mol-1)is prepared by dissolving 68.4 g of it per litre ofsolution. What is its osmotic pressure (R = 0.082).1 atm K-l mol-1 at 273 ?

a) 3.92 atm b) 4.48 atm

c) 5.92 atm d) 29.4 atm

42. At 300 K, 36 g of glucose present per litre in itssolution has an osmotic pressure of 4.98 bar. Ifthe osmotic pressure of solution is 1.52 bar at thesame temperature what would be itsconcentration ?

(Molar mass of Glucose = 180 g mol-1)

a) Ll g L? b) 22 g L-l

c) 36gL-l d) 42 g L-l

43. The boiling point of solution containing 68.4 g ofsucrose (molar mass = 342 g mol-1) in 100g ofwater is (Kb for water = 0.512 K. kg mol-1)

a) 100.02°C b) 98.98°C

c) 101.02°C d) 100.512°C.

Answer Key

Q.No. Ans Q.No. Ans Q.No. Ans

1. b) 2. a) 3. b)4. d) 5. a) 6. d)7. b) 8. c) 9. b)10. a) 11. b) 12. c)13. b) 14. d) 15. d)16. b) 17. c) 18. b)19. d) 20. d) 21. b)22. c) 23. b) 24. c)25. a) 26. b) 27. c)28. d) 29. d) 30. b)31. c) 32. a) 33. c)34. c) 35. a) 36. d)37. d) 38. d) 39. a)40. b) 41. b) 42. a)43. c)






1. c) 2. c) 3. d)4. d) 5. d) 6. c)7. c) 8. b) 9. d)10. c) 11. c) 12 a)13. b) 14. a) 15. b)16. d) 17. d) 18. c)19. d) 20. b) 21. b)22. d) 23. d) 24. c)25. c) 26. b) 27. a)28. c) 29. d) 30. b)31. c) 32. c) 33. a)34. d) 35. b) 36. a)37. d) 38. c) 39. a)40. b) 41. c) 42. b)43. a) 44. c) 45. a)46. d) 47. d) 48. c)49. c) 50. b) 51. d)52. a) 53. b) 54. c)55. a) 56. b) 57. c)58. a) 59. d) 60. c)61. c) 62. a) 63. d)64. b) 65. a) 66. d)67. a) 68. a) 69. b)70. a) 71. a) 72. b)73. d) 74. d) 75. b)76. c) 77. b) 78. b)79. b) 80. d) 81. c)82. c) 83. a) 84. b)85. a) 86. d) 87. c)88. b) 89. c) 90. a)91. d) 92. d) 93. a)94. c) 95. a) 96. b)97. a) 98. b) 99. b)100. a) 101. c) 102. b)103. b) 104. c) 105. b)106. b) 107. d) 108. b)109. a) 110. b) 111. c)112. a) 113. d) 114. b)115. d) 116. c) 117. b)118. b) 119. d) 120. b)121. b) 122. a) 123. a)124. a) 125. b) 126. a)127. b) 128. b) 129. a)130. a) 131. a) 132. a)133. d) 134. b) 135. d)136. c) 137. b) 138. a)139. a) 140. c) 141. c)142. d) 143. a) 144. a)

Answer Key





Answer Key


145. a) 146. a) 147. a)148. a) 149. c) 150. a)151. d) 152. b) 153. a)154. b) 155. b) 156. d)157. d) 158. b) 159. a)160. b) 161. a) 162. b)163. b) 164. a) 165. c)166. c) 167. c) 168. d)169. c) 170. d) 171. b)172. a) 173. b) 174. b)175. a) 176. d) 177. d)178. d) 179. c) 180. d)181. b) 182. a) 183. a)184. b) 185. b) 186. a)187. b) 188. a) 189. a)190. c) 191. c) 192. c)193. a) 194. d) 195. b)196. a) 197. c) 198. c)199. d) 200. b) 201. b)202. c) 203. d) 204. d)205. b) 206. a) 207. b)208. b) 209. a) 210. b)211. b) 212. c) 213. a)214. b) 215. d) 216. a)217. c) 218. c) 219. d)220. d) 221. c) 222. a)223. c) 224. a) 225. b)226. a) 227. a) 228. b)229. a) 230. c) 231. a)232. c) 233. b) 234. c)235. c) 236. b) 237. a)238. c) 239. c) 240. a)241. a) 242. d) 243. d)244. d) 245. b) 246. c)247. c) 248. b) 249. a)250. b) 251. a) 252. a)253. b) 254. c) 255. a)256. a) 257. b) 258. b)259. a) 260. b) 261. b)262. b) 263. a) 264. c)265. d) 266. a) 267. b)268. c) 269. b) 270. d)271. d) 272. a) 273. b)274. a) 275. b) 276. a)277. c) 278. c) 279. c)280. c) 281. c) 282. b)283. c) 284. c) 285. c)





Answer Key


286. a) 287. a) 288. d)289. c) 290. d) 291. a)292. c) 293. d) 294. a)295. c) 296. c) 297. a)298. a) 299. b) 300. a)301. b) 302. a) 303. d)304. a) 305. b) 306. c)307. b) 308. b) 309. c)310. b) 311. c) 312. a)313. b) 314. c) 315. b)316. c) 317. c) 318. a)319. c) 320. b) 321. b)322. b) 323. a) 324. d)325. b) 326. d) 327. c)328. c) 329. d) 330. c)331. a) 332. c) 333. d)334. d) 335. a) 336. a)337. c) 338. b) 339. c)340. b) 341. b) 342. c)343. c) 344. a) 345. c)346. c) 347. a) 348. c)349. b) 350. d) 351. b)352. b) 353. b) 354. c)355. b) 356. a) 357. b)358. c) 359. b) 360. d)361. d) 362. c) 363. c)364. d) 365. b) 366. b)367. d) 368. d) 369. d)370. c) 371. c) 372. d)373. b) 374. a) 375. b)376. c) 377. c) 378. d)379. b) 380. b) 381. c)382. c) 383. c) 384. a)385. c) 386. b)




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02. solution and colligative properties

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