chapter 06: chemical equilibrium harris: quantitative chemical analysis, eight edition
TRANSCRIPT
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CHAPTER 06: CHEMICAL
EQUILIBRIUM
Harris: Quantitative Chemical Analysis, Eight Edition
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CaCO3(s) + CO2(aq) + H2O(l) = Ca2 + (aq) + 2HCO3 - (aq)
HCO3 - (aq) + H + (aq) s --- > CO2(g) + H2O(l)
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aA + bB = cC + dD in its standard state
HA = H + + A - K1 = [H + ][A - ] / [HA] 만약 반응의 방향을 바꾸면 새 K 값은 처음 K 값의 역수가 된다 .H + + A - = HA K1′ = [HA] / [H + ][A- ] = 1/K1 HA = H + + A - K1
H + + C = CH + K2
----------------------------------HA + C = A - + CH + K3
K3 = K1K2 = [H + ][A - ] / [HA] ·[CH + ] / [H + ][C] = [A - ] ·[CH + ] / [HA] [C]
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Le Chˆatelier’s principle:
Reaction quotient:
Because Q > K, the reaction must go to the left
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When the temperature changes:
The term including e ᅀ S/R is independent of T. The term e- ᅀ H/RT increases with increasing temperature if ᅀ 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
Co-precipitation: foreign ions adsorbed on the precipitate.
Q < Ksp for PbI2, Pb ions will not precipitate.
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Lewis Acid and Bases
6-4 Complex Formation
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Effect of Complex Ion Formation on Solubility
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6-5 Protic Acids and Bases
- Hydronium ion: H3O+
Brønsted- Lowry Acids and Bases: Acid: proton donor, Base: proton acceptor
Salt: Any ionic solid
When [I-] = 1.0 M, [Pb]total = 3.2 x 10-4 M
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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 ( 또는 K1) 은 가장 많은 양성자를 가진 산성 화학종에 대한 것이고 , Kbl 은 가장 적은 양성자를 가진 염기성 화학종에 대한 것이다 .
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Relationship between Ka and Kb
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Carbonic Acid
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6-8 Solving Equilibrium Problems