Quantitative Chemical Analysis 7e

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Harris Quantitative Chemical Analysis, Eight
Edition
CHAPTER 06 CHEMICAL EQUILIBRIUM
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CaCO3(s) CO2(aq) H2O(l) Ca2(aq) 2HCO3 -
(aq) HCO3 - (aq) H(aq) s --- gt CO2(g)
H2O(l)
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aA bB cC dD in its standard state
HA H A- K1 HA- / HA
?? ??? ??? ??? ? K?? ?? K?? ??? ??. H
A- HA K1' HA / HA- 1/K1
HA H A- K1 H C
CH K2 -----------------
----------------- HA C A- CH
K3
K3 K1K2 HA- / HA CH / HC
A- CH / HA C
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Le Chˆateliers principle
Reaction quotient
Because Q gt K, the reaction must go to the left
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When the temperature changes
The term including e ?S/R is independent of T.
The term e- ?H/RT increases with increasing
temperature if ?Ho is positive, and decreases if
it is negative. K of the endothermic reaction
increases if T is raised. K of the exothermic
reaction decreases if T is raised.
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6-3 Solubility product
Ion pair
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Disproportionation an element in an intermediate
oxidation state gives products.
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Common ion effect
A salt will be less soluble if one of its
constituent ions is already present in the
solution.
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Separation by Precipitation
Q lt Ksp for PbI2, Pb ions will not precipitate.
Co-precipitation foreign ions adsorbed on the
precipitate.
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6-4 Complex Formation
Lewis Acid and Bases
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Effect of Complex Ion Formation on Solubility
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When I- 1.0 M, Pbtotal 3.2 x 10-4 M
6-5 Protic Acids and Bases
- Hydronium ion H3O
Brønsted-Lowry Acids and Bases Acid proton
donor, Base proton acceptor
Salt Any ionic solid
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Conjugate Acids and Bases
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- Structure of Hydronium ion
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The Nature of H and OH-
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Autoprotolysis
- Protic solvents have a reactive H
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6-6 pH
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Is There Such a Thing as Pure Water?
6-7 Strength of Acids and Bases
Strong Acids and Bases
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Weak Acids and Bases
Ka Acid dissociation constant
Kb Base hydrolysis constant
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Common Classes of Weak Acids and Bases
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Polyprotic Acids and Bases
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Kal (?? K1) ? ?? ?? ???? ?? ?? ???? ?? ???, Kbl?
?? ?? ???? ?? ??? ???? ?? ???.
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Relationship between Ka and Kb
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Carbonic Acid
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6-8 Solving Equilibrium Problems