1. What is the solubility (in M) of PbCl2 in a 0.15 M solution of HCl?
(Ksp PbCl2 = 1.6 x 10-5)
a. 7.1 x 10-4
b. 1.1 x 10-4
c. 2.0 x 10-3
d. 1.8 x 10-4
e. 1.6 x 10-5
2. In which aqueous system is PbI2 least soluble?
b. 0.2 M HI
c. 0.5 M HI
d. 1.0 M HNO3
e. 0.8 M KI
3. AgCl dissolves in aqueious solutions of ammonia via formation of a
AgCl(s) + 2NH3(aq) → Ag(NH3)2+(aq) + Cl-(aq).
Let z denote the molar solubility of AgCl in 2.0 M NH3. Given that
Kc = KspKf (where Ksp is for AgCl and Kf is for Ag(NH3)2+), the
value of z can be calculated according to which of the following
a. KspKf = (2.0 + 2z)2/z
b. KspKf = z/(2.0 + 2z)2
c. KspKf = z2/(2.0 - z)
d. KspKf = z/(2.0 - z)2
e. KspKf = z2/(2.0 - 2z)2
4. Which one of the following compounds will increase in solubility if
the pH of a saturated solution of the compound is lowered?
5. Consider a solution containing 0.181 M lead ions and 0.174 M
mercury(II) ions. The Ksp for lead sulfide is 3.4 x 10-28 and that
for mercury(II) sulfide is 4.0 x 10-53. Calculate the concentration
(in M) of sulfide ions required to reduce the concentration of
mercury(II) ions to 1.0 x 10-6 M.
a. 3.4 x 10-22
b. 1.2 x 10-25
c. 4.0 x 10-47
d. 5.6 x 10-13
e. 3.4 x 10-28
6. If treatment of a solution, known to contain at least one type of
cation, with dilute HCl did not result in the formation of a
precipitate, which ion below might the solution contain?
e. The solution could contain any of these
Multiple Choice questions on solubility