chapter 16 “ solutions ”
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Chapter 16 “ Solutions ”. Solvents and Solutes. Solution - a homogenous mixture , that is mixed molecule by molecule; made of: a Solvent - the dissolving medium a Solute - the dissolved particles Aqueous solution - a solution with water as the solvent. - PowerPoint PPT PresentationTRANSCRIPT
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Chapter 16
“Solutions”
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Solvents and Solutes Solution - a homogenous mixture, that is
mixed molecule by molecule; made of:1) a Solvent - the dissolving medium2) a Solute - the dissolved particles Aqueous solution- a solution with water
as the solvent. Particle size is less than 1 nm; cannot be
separated by filtration – Fig. 15.6, p.450
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1. the SoluteA solute is the dissolved substance in a solution.
A solvent is the dissolving medium in a solution.
2. the Solvent
Salt in salt water Sugar in soda drinksCarbon dioxide in soda drinks
Water in salt water Water in soda
Parts of a Solution:
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SolutionsKeep in mind that solutions do not have to contain water, but this is the type we are studying in this chapter = aqueous solutions–Example: air and jewelry are also types of solutions.
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Solvents
There are a tremendous number of solutions we use in our daily lives!
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Concentrated vs. DiluteConcentrated vs. Dilute
Lots of solute, but little solvent
Lots of solvent, but little solute
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Aqueous SolutionsWater dissolves ionic compounds and
polar covalent molecules very well.The rule is: “like dissolves like”Polar dissolves polar.Nonpolar dissolves nonpolar.Oil is nonpolar.
–Oil and water don’t mix.Salt is ionic- makes salt water.
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The Solution ProcessCalled “solvation”.Water 1) breaks the + and - charged
pieces apart, and 2) surrounds them.But, in some ionic compounds, the
attraction between ions is greater than the attraction exerted by water–Barium sulfate and calcium carbonate do
not dissolve in water!
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How Ionic solids dissolve in water
H HOH
H OH
HO
H HO
HHO
HH
O
HH
OH
HOH
HO
These ions have been surrounded by water, and are now dissolved!
These ions have been pulled away from the main crystal structure by water’s polarity.
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Solids will dissolve if the attractive force of the water molecules is stronger than the attractive force of the crystal.
If not, the solids are insoluble.Water doesn’t dissolve nonpolar molecules
(like oil) because the water molecules can’t hold onto them.
The water molecules hold onto other water molecules, and separate from the nonpolar molecules.
Nonpolars? No repulsion between them
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Electrolytes and NonelectrolytesElectrolytes- compounds that conduct
an electric current in aqueous solution, or in the molten state–all ionic compounds are electrolytes because they dissociate into ions (they are also called “salts”)
barium sulfate- will conduct when molten, but is insoluble in water!
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Electrolytes and NonelectrolytesDo not conduct? = Nonelectrolytes.
–Most are molecular materials, because they do not have ions
Not all electrolytes conduct to the same degree– there are weak electrolytes, and strong electrolytes
–depends on: the degree of ionization
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The ammeter measures the flow of electrons (current) through the circuit. If the ammeter measures a current and the
bulb glows, then the solution conducts. If the ammeter fails to measure a current and the bulb
does not glow, the solution is non-conducting.
Electrolytes vs. Nonelectrolytes
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Electrolytes and NonelectrolytesStrong electrolytes exist as nearly
100 % ionsWeak electrolytes have only a
fraction of the solute that exists as ions
How do you know if it is strong or weak? Refer to the rules on the handout sheet.
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Electrolyte SummarySubstances that conduct electricity when dissolved in water, or molten.
Must have charged particles that can move.
Ionic compounds break into charged ions:NaCl ® Na1+ and Cl1-
These ions can conduct electricity.
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Nonelectrolytes do not conduct electricity when dissolved in water or molten
Polar covalent molecules such as methanol (CH3OH) don’t fall apart into ions when they dissolve.
Weak electrolytes don’t fall completely apart into ions.
Strong electrolytes do ionize completely.
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Solution formation The “nature” (polarity, or composition)
of the solute and the solvent will determine…
1. Whether a substance will dissolve2. How much will dissolve
Factors determining rate of solution...1. stirring (agitation)2. surface area the dissolving particles3. temperature
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Making solutions In order to dissolve, the solvent
molecules must come in contact with the solute.
1. Stirring (agitation) moves fresh solvent into contact with the solute.
2. Smaller pieces increase the amount of surface area of the solute.- think of how fast a breath mint dissolves when you chew it
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Temperature and Solutions3. Higher temperature makes the
molecules of the solvent move faster and contact the solute harder and more often.– Speeds up dissolving.
Higher Temperature ALSO Usually increases the amount that will dissolve (an exception is gases, more on that later).
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- Page 474a. The solubility of the KNO3 increases as the temperature increases.b. Yb2(SO4)3 shows a decrease in solubility as the temperature increases, and NaCl shows the least change in solubility as temperature changes.c. Only a negligible amount of NaCl would go into solution, if any.
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Solids tend to dissolve best when:
•They are heated•They are stirred•Crushed into smaller particles
Gases tend to dissolve best when:
•The solution is cold•The pressure is high
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How Much? Solubility- is the maximum amount of
substance that will dissolve at a specific temperature. The units for solubility are: grams of solute/100 grams solvent
1) Saturated solution- Contains the maximum amount of solute dissolved. NaCl = 36.0 g/100 mL water
2) Unsaturated solution- Can still dissolve more solute (for example 28.0 grams of NaCl/100 mL)
3) Supersaturated- solution that is holding (or dissolving) more than it theoretically can; a “seed crystal” will make it come out; Fig. 16.6, page 475
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Saturation and Equilibrium
Solute is dissolving
More solute is dissolving, but some is crystallizing
Saturation equilibrium established
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Supersaturated
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Supersaturated ExampleEver heard of “seeding” the clouds
to make them produce rain?Clouds - mass of air
supersaturated with water vaporSilver Iodide (AgI) crystals are
dusted into the cloud as a “seed”The AgI attracts the water, forming
droplets that attract others
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LiquidsMiscible means that two liquids
can dissolve in each other–water and antifreeze–water and ethanol
Partially miscible- slightly–water and ether
Immiscible means they can’t–oil and vinegar
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Solubility?For solids in liquids, as the
temperature goes up-the solubility usually goes up (Fig. 16.4, p.474)
For gases in a liquid, the effect is the opposite of solids in liquids–As the temperature goes up, gas
solubility goes down–Think of boiling water bubbling?–Thermal pollution may result from
industry using water for cooling
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Gases in liquids...Henry’s Law - says the solubility of a
gas in a liquid is directly proportional to the pressure of the gas above the liquid– think of a bottle of soda pop, removing the lid releases pressure
Equation: S1 S2
P1 P2
Sample 16.1, page 477
=
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Concentration is...a measure of the amount of solute
dissolved in a given quantity of solventA concentrated solution has a large
amount of soluteA dilute solution has a small amount of
solute–These are qualitative descriptions
But, there are ways to express solution concentration quantitatively (NUMBERS!)
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Concentrated vs. Dilute
Lots of solute, in a small amount of solvent.
Small amount of solute in a
large amount of solvent.
Notice how dark the
solutions appears.
Notice how light
the solution appears.
CONCENTRATED DILUTE
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Molarity: a unit of concentrationMolarity = moles of solute
liters of solution•Abbreviated with a capital M, such as 6.0 M
•This is the most widely used concentration unit used in chemistry.
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- Page 481
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Making solutions1) Pour in a small amount of the
solvent, maybe about one-half2) Then add the pre-massed solute
(and mix by swirling to dissolve it)3) Carefully fill to final volume.
– Fig. 16.8, page 481, and shown on next slide.
Can also solve: moles = M x L Sample Problem 16.3, page 482
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Dilution• Adding water to a solution will reduce the
number of moles of solute per unit volume• but the overall number of moles
remains the same!• Think of taking an aspirin with a small
glass of water vs. a large glass of water• You still have one aspirin in your body,
regardless of the amount of water you drank, but a larger amount of water makes it more diluted.
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DilutionThe number of moles of solute in
solution doesn’t change if you add more solvent!
The # moles before = the # moles afterFormula for dilution: M1 x V1 = M2 x V2 M1 and V1 are the starting
concentration and volume; M2 and V2 are the final concentration and volume.
Stock solutions are pre-made solutions to known Molarity. Sample 16.4, p.484
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Percent solutions can be expressed by a) volume or b) massPercent means parts per 100, soPercent by volume:
= Volume of solute x 100% Volume of solution
indicated %(v/v)Sample Problem 16.5, page 485
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Percent solutionsPercent by mass:
= Mass of solute(g) x 100% Volume of solution (mL)
Indicated %(m/v)More commonly used4.8 g of NaCl are dissolved in 82 mL of
solution. What is the percent of the solution?
How many grams of salt are there in 52 mL of a 6.3 % solution?
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Percent solutionsAnother way to do mass percentage is as
mass/mass:
Percent by mass: = Mass of solute(g) x 100% Mass of solution (g)
Indicated %(m/m)
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Colligative Properties -These depend only on the number
of dissolved particles-Not on what kind of particle-Three important colligative properties
of solutions are:1) Vapor pressure lowering2) Boiling point elevation3) Freezing point lowered
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Glucose will only have one particle in solution for each one particle it starts with.
NaCl will have two particles in solution for each one particle it starts with.
CaCl2 will have three particles in solution for each one particle it starts with.
Colligative Properties
Some particles in solution will IONIZE (or split), while others may not.
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Vapor Pressure is LOWERED1) Surface area is reduced, thus less
evaporation, which is a surface property2) The bonds between molecules keep
molecules from escaping. So, in a solution, some of the solvent is busy keeping the solute dissolved.
This lowers the vapor pressure Electrolytes form ions when they are
dissolved, making more pieces. NaCl ® Na+ + Cl- (this = 2 pieces) More pieces = a bigger effect
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Boiling Point is ELEVATEDThe vapor pressure determines the
boiling point. (Boiling is defined as when the vapor pressure of liquid = vapor pressure of the atmosphere).
Lower vapor pressure means you need a higher temperature to get it to equal atmospheric pressure
Salt water boils above 100ºCThe number of dissolved particles
determines how much, as well as the solvent itself.
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Freezing Point is LOWEREDSolids form when molecules make an
orderly pattern called “crystals”The solute molecules break up the
orderly pattern. –Makes the freezing point lower.–Salt water freezes below 0ºC–Home-made ice cream with rock salt?
How much lower depends on the amount of solute dissolved.
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The addition of a solute would allow a LONGER temperature range, since freezing point is lowered and boiling point is elevated.
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Molality (abbreviated m)a new unit for concentrationm = Moles of solute
kilogram of solventm = Moles of solute
1000 g of solvent
Sample Problem 16.6, p. 492
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Mole fractionThis is another way to express
concentrationIt is the ratio of moles of solute to
total number of moles of solute plus solvent (Fig. 18-19, p.522)
na
na + nbX = Sample 16.7,
page 493
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Freezing Point DepressionThe size of the change in freezing
point is also determined by molality.
DTf = -Kf x m x nDTf is the change in freezing pointKf is a constant determined by the
solvent (Table 16.2, page 494).n is the number of pieces it falls
into when it dissolves.
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- Page 495
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Boiling Point ElevationThe size of the change in boiling
point is determined by the molality.DTb = Kb x m x n
DTb is the change in the boiling pointKb is a constant determined by the
solvent (Table 16.3, page 495).n is the number of pieces it falls into
when it dissolves.Sample Problem 16.9, page 496