(a) Interpretation: From the given K a values, p K a of weak acids should be calculated. Concept introduction: The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium. For a general reaction of ionization of weak acid as follows: HA ⇌ H + + A − The expression for dissociation constant of the reaction is as follows: K a = [ H + ] [ A − ] [ HA ] The p K a of a weak acid is defined as negative log of K a or, p K = − log K a
(a) Interpretation: From the given K a values, p K a of weak acids should be calculated. Concept introduction: The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium. For a general reaction of ionization of weak acid as follows: HA ⇌ H + + A − The expression for dissociation constant of the reaction is as follows: K a = [ H + ] [ A − ] [ HA ] The p K a of a weak acid is defined as negative log of K a or, p K = − log K a
Solution Summary: The author explains that the ionization equation of weak acids is in equilibrium. The pK_a of a weak acid is negative log of acid dissociation constant.
Definition Definition Transformation of a chemical species into another chemical species. A chemical reaction consists of breaking existing bonds and forming new ones by changing the position of electrons. These reactions are best explained using a chemical equation.
Chapter 13, Problem 36QAP
Interpretation Introduction
(a)
Interpretation:
From the given Ka values, pKa of weak acids should be calculated.
Concept introduction:
The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.
For a general reaction of ionization of weak acid as follows:
HA⇌H++A−
The expression for dissociation constant of the reaction is as follows:
Ka=[H+][A−][HA]
The pKa of a weak acid is defined as negative log of Ka or,
pK=−logKa
Interpretation Introduction
(b)
Interpretation:
From the given Ka values, pKa of weak acids should be calculated.
Concept introduction:
The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.
For a general reaction of ionization of weak acid as follows:
HA⇌H++A−
The expression for dissociation constant of the reaction is as follows:
Ka=[H+][A−][HA]
The pKa of a weak acid is defined as negative log of Ka or,
pK=−logKa
Interpretation Introduction
(c)
Interpretation:
From the given Ka values, pKa of weak acids should be calculated.
Concept introduction:
The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.
For a general reaction of ionization of weak acid as follows:
HA⇌H++A−
The expression for dissociation constant of the reaction is as follows:
Ka=[H+][A−][HA]
The pKa of a weak acid is defined as negative log of Ka or,
Given that acetic acid has Ka = 1.8 x 10–5, what is the pH of a solution that contains the molar ratio of conjugate base-to-acid: [CH3CO2–]/[CH3CO2H] = 1/10?
Complete the sentence
for a strong acid, the equilibrium constant Ka is
A. So small that HA is not completely dissociated
b. So large that HA is completely dissociates into H3O+ and A-
c. Neutral
Benozic acid (C6H5COOH) has a pKa of 4.20.
a. What is the ratio of the acid to its conjugate base at a pH of 2.20?
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