CHEM 1F92 Assignment 13. Acid-Base Equilibrium
Assignment 13, Version # 34
1. What are the conjugate acids for the following bases?
(a) OCN(b) HCO2- 2. What are the conjugate bases of the following acids?:
(a) H2SO3
(b) HN3 3.
In each of the following acid-base reactions, identify the Bronsted acid and base on the left, and their
conjugate partners on the right:
(a) OBr- + H2O → HOBr + OH(b) H2AsO4- + CH3NH3+ → CH3NH2 + H3AsO4
(c) HSeO4- + SO32- → HSO3- + SeO424.
In a Bronsted acid-base reaction, the stronger acid reacts with the stronger base to produce a weaker
acid and a weaker base. Thus, whether a reaction “goes” or “does not go” can be used to determine the
relative strength of the Bronsted acids and bases in the reaction. From the data below, determine the order of
the strengths of the three Bronsted acids.
Reaction 1: HOCl + HO2- → H2O2 + ClOgoes
Reaction 2: NH3OH+ + HO2- → H2O2 + NH2OH
goes
+
Reaction 3: HOCl + NH2OH → NH3OH + ClO
does not go
5.
Make the following conversions. Report answers to 2 decimal places.In each case, tell whether the
solution is acidic or basic.
pH
[H3O+]
[OH-]
acidic or basic?
(a) 9.36
(b)
6.07 x 10-5
(c)
6.41 x 10-11
6.
A 0.33 M solution of a weak acid HA is 0.15 % ionized. What are the H+, A-, and HA concentrations
at equilibrium? What is Ka?
7.
The Ka for propanoic acid, HC3H5O2 is 1.4 x 10-5. What is the pH of a 0.30 M solution of the acid?
What is the % ionization of the acid at this concentration?
8. A 0.17 M solution of a weak base B has a pH of 9.09. The equation for ionization is
B (aq) + H2O → BH+ + OHWhat are the BH+, OH-, and B concentrations at equilibrium? Calculate Kb for the base.
9.
The base trimethylamine, (CH3)3N, has a pKb equal to 4.20. Calculate the hydroxide concentration,
the pH, and the % ionization for a 0.34 M solution.

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