8.4 Practice Problems
Attempt these problems as if they were real exam questions in an exam environment.
Only look up information if you get severely stuck. Never look at the solution until you have exhausted all efforts to solve the problem.
What is the solubility of MgF2 (m.m. = 62.30 g mol–1) in 1 L of water? Ksp = 5.2 × 10–11
- 1.29 × 10–5
- 4.49 × 10–4
- 0.0146
- 0.0886
- 0.115
Solution
Answer: C
Which of the following could you add to a saturated Ca3(PO4)2 aqueous solution to cause the solute to precipitate?
- AgCl
- Na3PO4
- KBr
- MgBr2
- H2O
Solution
Answer: B
CaSO3 (m.m. = 120.17 g mol–1) has a solubility of 0.043 g L–1 in water. What is the solubility product for CaSO3?
- 4.22 × 10–11
- 1.28 × 10–7
- 3.60 × 10–4
- 2.30 × 10–3
- 10.3
Solution
Answer: B
The solubility product of CuCl is 1.20 × 10–6. What is the solubility of CuCl (in g L–1)?
- 1.09 × 10–3
- 3.41 × 10–2
- 0.26
- 1.44
- 43.21
Solution
Answer: C
Which compound is the least soluble in 1 L of water (at 25 °C)?
- HgS, Ksp = 1.8 × 10–53
- PbS, Ksp = 7.0 × 10–29
- AgI, Ksp = 1.5 × 10–16
- CuBr, Ksp = 1.5 × 10–9
- CuCl, Ksp = 1.2 × 10–6
Solution
Answer: A
A saturated solution is prepared by dissolving Fe(OH)3 in pure water (at 25 °C). Adding which of the following would result in an unsaturated Fe(OH)3 solution?
- BaCO3
- Fe(OH)2
- NH3
- HCl
- PbF2
Solution
Answer: D
Which reaction quotient would indicate that the following reaction would proceed to the left (towards reactants)?
\[\mathrm{AgCl}(s) \rightleftharpoons \mathrm{Ag^+}(aq) + \mathrm{Cl^-}(aq) \quad K_{\mathrm{sp}} = 1.8 \times 10^{-10}\]
- 1.5 × 10–11
- 1.6 × 10–10
- 1.7 × 10–10
- 1.8 × 10–10
- 1.9 × 10–10
Solution
Answer: E