(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,
When talking about the acidity of carboxylic acids, is it the same thing to say higher or stronger acidity?
Using the following two half-reactions, determine the pH range in which $NO_2^-\ (aq)$ cannot be found as the predominant chemical species in water.* $NO_3^-(aq)+10H^+(aq)+8e^-\rightarrow NH_4^+(aq)+3H_2O(l),\ pE^{\circ}=14.88$* $NO_2^-(aq)+8H^+(aq)+6e^-\rightarrow NH_4^+(aq)+2H_2O(l),\ pE^{\circ}=15.08$
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