Page 808 - Chemistry--atom first
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798 Chapter 14 | Acid-Base Equilibria
56. From the equilibrium concentrations given, calculate Ka for each of the weak acids and Kb for each of the weak bases.
(a) CH3CO2H: = 1.34 10−3 M; = 1.34 10−3 M;
[CH3CO2H] = 9.866 10−2 M; (b) ClO−: [OH−] = 4.0 10−4 M; [HClO] = 2.38 10−5 M; [ClO−] = 0.273 M;
(c) HCO2H: [HCO2H] = 0.524 M; = 9.8 10−3 M;
= 9.8 10−3 M;
(d) = 0.233 M;
[C6H5NH2] = 2.3 10−3 M; = 2.3 10−3 M
57. From the equilibrium concentrations given, calculate Ka for each of the weak acids and Kb for each of the weak bases.
(a) NH3: [OH−] = 3.1 10−3 M; = 3.1 10−3 M;
[NH3] = 0.533 M;
(b) HNO2: = 0.011 M;
= 0.0438 M; [HNO2] = 1.07 M;
(c) (CH3)3N: [(CH3)3N] = 0.25 M; [(CH3)3NH+] = 4.3 10−3 M;
[OH−] = 4.3 10−3 M;
(d) =0.100M;
[NH3] = 7.5 10−6 M; [H3O+] = 7.5 10−6 M
58. Determine Kb for the nitrite ion, In a 0.10-M solution this base is 0.0015% ionized.
59. Determine Ka for hydrogen sulfate ion, In a 0.10-M solution the acid is 29% ionized.
60. Calculate the ionization constant for each of the following acids or bases from the ionization constant of its
conjugate base or conjugate acid:
(a) F−
(b)
(c)
(d)
(e)
(f) (as a base)
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