acids in daily-life ethanoic acid( in vinegar) ch 3 cooh citric acid ( in fruit) carbonic acid ( in...
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AcidsIn daily-life• Ethanoic acid( in vinegar) CH3COOH• Citric acid ( in fruit)• Carbonic acid ( in soft drink) H2CO3
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Common acids in lab
Hydrochloric acid
Sulphuric acid
Nitric acid
HCl H2SO4 HNO3
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Mineral acids (in organic acids)• Hydrochloric acid, HCl • Sulphuric acid, H2SO4
• Nitric acid,HNO3
• Carbonic acid, H2CO3
Others mainly are organic acids
Acids – H containing covalent molecules
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Pure acids can be in different states (g)/(l)/(s) at different temperatures.
• e.g HCl is in gas state at room temperature. Citric acid is in solid state at room temper
ature.
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Dilute acid Concentrated acid
Acid molecule
Acid used in lab are usually aqueous solutions.
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Physical Properties of Dilute Acids
a) sourb) acidic; it turn blue litmus paper to redc) it conduct electricity only in aqueous
state.
a) Tasteb) pH c) Electrical conductivity
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a) Reaction with metal (KPb)b) Reaction with oxides/ hydroxidesc) Reaction with carbonates/ Hydroge
ncarbonates
Chemical Properties of Dilute Acids
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acid + metal salt + hydrogen
H2SO4(aq) + Mg(s) MgSO4(aq) + H2(g)
2HCl(aq) + Zn(s) ZnCl2(aq) + H2(g)
Reaction with metalsReaction with metals
For example,
They react with metals higher than copper in the reactivity series, liberating hydrogen gas:
Dilute acids: Only dilute HCl, H2SO4,very dilute HNO3
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acid + metal oxide salt + water
e.g. H2SO4(aq) + CuO(s) CuSO4(aq) + H2O(l)
acid + metal hydroxide salt + water
e.g. H2SO4(aq) + 2NaOH(aq) Na2SO4(aq) + 2H2O(l)
Action on metal oxides and hydroxidesAction on metal oxides and hydroxides
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acid + carbonate salt + carbon dioxide + water
For example,
2HCl(aq) + CaCO3(s) CaCl2(aq) + CO2(g) + H2O(l)
For example,
HNO3(aq) + NaHCO3(s) NaNO3(aq) + CO2(g) + H2O(l)
acid + hydrogencarbonate salt + carbon dioxide + water
Action on carbonates and hydrogencarbonatesAction on carbonates and hydrogencarbonates
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How to test for the existence of carbon dioxide?
How to test for the existence of carbon dioxide?
Limewater test
Limewater test
15.2 Characteristics and chemical properties of acids15.2 Characteristics and chemical properties of acids
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15.2 Characteristics and chemical properties of acids15.2 Characteristics and chemical properties of acids
Limewater test for carbon dioxide
Carbon dioxide is a colourless gas. It turns limewater milky.
Ca(OH)2(aq) + CO2(g) CaCO3(s) + H2O(l)Ca(OH)2(aq) + CO2(g) CaCO3(s) + H2O(l)lime water
colourless solution white solid
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Na2CO3(s) + H2SO4(aq) Na2SO4(aq) +
***Soluble in water
Na+ CO32- 2H+ SO4
2-
Na2SO4 H2CO3
H2O(l) + CO2(g)
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2NaHCO3(s)+H2SO4(aq) Na2SO4(aq)+
***Soluble in water
2Na+ 2HCO3- 2H+ SO4
2-
Na2SO4 2H2CO3
2H2O(l)+2CO2(g)
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• All oxides are insoluble, (s)• All hydroxides except gp 1 are insoluble, (s)• All carbonates except gp 1 are insoluble, (s)• AgX and PbX2 are insoluble, (s) (X= Cl-, Br-, I-)• CaSO4, PbSO4, BaSO4 are insoluble, (s)
•All hydrogencarbonates are soluble ---(aq)
***Even though some compounds are soluble in water, we may use its solid form for a reaction.
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SULPHURIC ACID AND NITRIC ACID IN WATER
Pure sulphuric acid and nitric acid are colourless liquids. They bot
h consist of covalent molecules. When they dissolve in water, ions
are formed. Acids are also electrolytes.
H2SO4(l)H2SO4(l)
H+(aq)H+(aq)
SO42(aq)SO42(aq)
H+(aq)H+(aq)
water moleculeswater molecules
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HNO3(l)HNO3(l) H+ (aq)H+ (aq)
NO3(aq)NO3(aq)
water moleculeswater molecules
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When acid molecules dissolve in water, ions are formed.
ionization
H+ (aq) + Cl- (aq)
2H+ (aq) + SO42- (aq)
H+ (aq) + NO3- (aq)
HCl(aq)H2SO4 (aq)
HNO3 (aq)
Acid is a H containing covalent compound, when dissolved in water, it forms H+ ions.^ o
nly
Is NaHSO4 / NaHCO3 an acid?
(as an only kind of positive ion)
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HYDROGEN CHLORIDE IN WATER AND IN
METHYLBENZENE
HCl in water
HCl(aq) H+(aq) + Cl-(aq)
HCl in methlybenzene (non-aqueous solvent)
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no gas evolved
(no apparent reaction)
bubbles of carbon dioxide evolved:
Na2CO3(s) + 2H+(aq) 2Na+(aq) + CO2(g) + H2O(l)
Action on solid sodium carbonate
no gas evolved
(no apparent reaction)
bubbles of hydrogen evolved:
Mg(s) + 2H+(aq) Mg2+(aq) + H2(g)
Action on magnesium
nonegoodElectrical conductivity
no colour changeturns to red colourEffect on dry blue litmus paper
Hydrogen chloride in dry methylbenzene
Hydrogen chloride in water (hydrochloric acid)
Test
15.3 The role of water for acids15.3 The role of water for acids
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Hydrogen ions (H+(aq)) are responsible for all the acidic
properties. Without water, acids cannot ionize to form H+(aq) and
hence do not have acidic properties.
15.3 The role of water for acids15.3 The role of water for acids
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Ingredients: solid acid
+ solid carbonate/hydrogencarbonate
Fizzy drink tablet
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CO32-(aq) + 2H+ (aq) CO2 (g) + H2O(l)
HCO3- (aq) + H+ (aq) CO2 (g) +
H2O(l)
H+
H+H+
HCO3-
HCO3-
HCO3-
CO32-
CO32-
CO32-
CO32-
Without water, acids do not have acidic properties.
Ingredients: solid acid + solid carbonate/hydrogencarbonate
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When acid dissolves in waterIonization
H+ (aq) + Cl- (aq) 2H+ (aq) + SO4
2- (aq)
H+ (aq) + NO3- (aq)
HCl(aq)H2SO4(aq)
HNO3(aq)
CH3COOH(aq) H+ (aq) + CH3COO- (aq) H3PO4(aq) 3H+ (aq) + PO4
3- (aq)
Basicity = no.of ionizable H+ in an acid
molecule
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15.4 BASICITY OF AN ACID
Different acids may give different numbers of hydrogen ions per
molecule in aqueous solution.
15.4 Basicity of an acid 15.4 Basicity of an acid
The BASICITY of an acid is the number of hydrogen ions
produced by one molecule of the acid.
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H2SO4(aq) 2H+(aq) + SO42-(aq)
H2SO3(aq) 2H+(aq) + SO32-(aq)
H2CO3(aq) 2H+(aq) + CO32-(aq)
H2C2O4(aq) 2H+(aq) + C2O42-(aq)
3(tribasic)
H3PO4(aq) 3H+(aq) + PO43-(aq)Phosphoric acid
2
(dibasic)
1
(monobasic)
HCl(aq) H+(aq) + Cl-(aq)
HNO3(aq) H+(aq) + NO3-(aq)
HNO2(aq) H+(aq) + NO2-(aq)
CH3COOH(aq) H+(aq) + CH3COO-(aq)
Hydrochloric acid
Nitric acid
Nitrous acid
Ethanoic acid
Basicity of acidIonization in waterAcid
Sulphuric acid
Sulphurous acid
Carbonic acid
Oxalic acid
Acids in “red” are strong acids. Acids in “red” are strong acids.
15.4 Basicity of an acid 15.4 Basicity of an acid
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only this hydrogen atom (connected with O) can form hydrogen ion, H+.
Figure 15.12 Ethanoic acid (CH3COOH) is monobasic because each molecule can onl
y give one hydrogen ion.
15.4 Basicity of an acid 15.4 Basicity of an acid
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Strong acid exists mainly as ions. It ionizes completely in water.
Weak acid exists mainly in molecular forms, it contains less ions since it only slightly ionizes in water.
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15.5 CORROSIVE NATURE OF CONCENTRATED ACIDS
All concentrated mineral acids are highly corrosive.All concentrated mineral acids are highly corrosive.
Figure 15.13 This hazard warning label
means ‘corrosive’. Concentrated mineral
acids always carry this label.
15.5 Corrosive nature of concentrated acids15.5 Corrosive nature of concentrated acids
High acidity(High
concentration of H+ ions)
High acidity(High
concentration of H+ ions)
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Figure 15.14 Holes appear in clothes in contact with concentrated sulphuric acid.
15.5 Corrosive nature of concentrated acids15.5 Corrosive nature of concentrated acids
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Figure 15.15 Concentrated mineral acids are highly corrosive.
15.5 Corrosive nature of concentrated acids15.5 Corrosive nature of concentrated acids
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CONCENTRATED HYDROCHLORIC ACID
15.5 Corrosive nature of concentrated acids15.5 Corrosive nature of concentrated acids
gives out white fumes (acid mist) in air.
a colourless liquid
35% by mass (~11 M)
an aqueous solution of hydrogen chloride gas
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Con HCl reacts with metals, carbonates, oxide in the sa
me way as the dilute acid, but at a faster rate.
Corrosiveness explainedCorrosiveness explained
The acidity increases as concentration increases.
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CONCENTRATED NITRIC ACID
Ordinary concentrated nitric acid (about 16 M) contains about 7
0 % nitric acid by mass. It is a colourless liquid, but often turns
yellow on storage.
15.5 Corrosive nature of concentrated acids15.5 Corrosive nature of concentrated acids
4HNO3 (aq) 2H2O (l) + 2NO2 (g) + O2 (g)4HNO3 (aq) 2H2O (l) + 2NO2 (g) + O2 (g)a yellowish brown gas
light
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Figure 15.17 Concentrated nitric acid is a colourless or pale yellow liquid. It is kept
in a brown bottle since it would decompose much more quickly in light.
15.5 Corrosive nature of concentrated acids15.5 Corrosive nature of concentrated acids
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15.5 Corrosive nature of concentrated acids15.5 Corrosive nature of concentrated acids
Corrosiveness explainedCorrosiveness explained
Conc. nitric acid shows the usual acidic properties, except
towards metals
Conc. nitric acid is highly
corrosive
Conc. nitric acid is highly
corrosive
oxidizing properties
Very dilute nitric acid is not corrosive, but concentrated nitric acid is very corrosive.
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CONCENTRATED SULPHURIC ACID
Ordinary concentrated sulphuric acid (about 18 M) is a colourless
oily liquid.
Figure 15.18 Concentrated sulphuric acid is a colourless oily liquid.
15.5 Corrosive nature of concentrated acids15.5 Corrosive nature of concentrated acids
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Corrosiveness explainedCorrosiveness explained
15.5 Corrosive nature of concentrated acids15.5 Corrosive nature of concentrated acids
Concentrated sulphuric acid has the usual acidic properties, e
xcept towards metals.
Dilute sulphuric acid is irritant, but concentrated sulphuric acid is very corrosive.
Corrosiveness
Dehydrating property
Oxidizing property
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15.6 IONIC EQUATIONS
For writing ionic equations from full equations, the formulae of ele
ctrolytes in aqueous solution should be rewritten as separate for
mulae of cations and anions.
For writing ionic equations from full equations, the formulae of ele
ctrolytes in aqueous solution should be rewritten as separate for
mulae of cations and anions.
15.6 Ionic equations15.6 Ionic equations
Formula of cations
Formula of cations
Formula of anions
Formula of anions
Formulae of electrolyte
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15.6 Ionic equations15.6 Ionic equations
Ionic compounds are electrolytes. Most of them are soluble in wat
er, but some are insoluble (e.g. lead(II) sulphate).
Acids are usually soluble electrolytes.