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Chemistry, 7/e
Raymond Chang, Williams College
Acid-Base Equilibria and Solubility Equilibria

Self Assessment B



1

What molar ratio of sodium acetate to acetic acid should be used to prepare a buffer with pH = 4.5? Ka acetic acid = 1.8 x 10-5.
A)1.6 parts sodium acetate to 1.0 part acetic acid.
B)0.20 parts sodium acetate to 1.0 part acetic acid.
C)0.63 parts sodium acetate to 1.0 part acetic acid.
D)-0.20 parts sodium acetate to 1.0 part acetic acid.
E)We cannot determine the pH of the buffer solution unless we know the actual concentrations of the buffer components.
2

Which of the chemical equations below represents the chemical reaction responsible for determining the solution pH at the equivalence point of the titration of 25 mL of 0.12 M acetic acid (HC2H3O2) with 0.10 M NaOH?
A)H2(l) ----> H+(aq) + OH-(aq)
B)C2H3O2-(aq) + H2O(l) ----> HC2H3O2(aq) + OH-(aq)
C)Na+(aq) + H2O(l) ----> NaOH(aq) + H+(aq)
D)C2H3O2-(aq) + Na+ ----> NaOH(aq) + C2H2O-(aq)
E)Because the neutralization is complete at the equivalence point of a titration, no further reaction occurs in the solution.
3

Calculate the pH at the equivalence point for the titration of 0.20 M aniline (C6H5NH2, Kb = 3.8 x 10-10) with 0.20 M HCI. [Hint: remember the dilution factor caused by addition of titrant to the aniline solution.]
A)2.79
B)5.58
C)5.21
D)8.79
E)None of the above.
4

Calculate the pH of a saturated Mg(OH)2 solution Ksp of Mg(OH) 2 = 1.2 x 10-11.
A)3.84
B)3.54
C)10.16
D)10.46
5

The molar solubility of PbCl2 is 3.9 x 10-2 M. What is the Ksp of PbCl2?
A)5.9 x 10-5
B)4.1 x 10-5
C)1.5 x 10-3
D)2.4 x 10-4
E)3.9 x 10-2
6

If 100 ml of 0.002 M Pb(NO3)2 is added to 50 ml of 0.35 M NaCl, will PbCl2 precipitate from solution? Ksp of PbCl2 = 4.1 x 10-5.
A)Yes.
B)No.
C)There's really no way to tell without mixing the solutions and observing what happens.
7

Calculate the molar solubility of Ag3PO4 in 1 M AgNO 3. Ksp of Ag3PO4 = 2.6 x 10-18.
A)2.6 x 10-18 M
B)2.9 x 10-19 M
C)6.6 x 10-7 M
D)1.4 x 10-6 M
8

Calculate the NaOH concentration necessary to precipitate Ca(OH)2 from a solution in which [Ca2+] = 1.0 Ksp of Ca(OH)2 = 8 x 10-6.
A)6.7 x 10-8 M
B)6.7 x 10-9 M
C)1.5 x 10-7 M
D)0.10 M
9

Which of the following compounds is not appreciably more soluble in 1 M HNO3 than in pure water?
A)Ca(OH)2
B)ZnS
C)Pbl2
D)Ca3(PO4)2
E)MgCO3
10

Which of the following compounds would be more soluble in 1 M NH3 than in pure water?
A)BaSO4
B)AgBr
C)Pbl2
D)BaF2
E)Ca(OH)2








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