6.4 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. Having to look up information or the solution should be an indicator that the previous layers (1–5) in the Structured Learning Approach have not been mastered.

  1. What is the solubility of MgF2 (m.m. = 62.30 g mol–1) in 1 L of water? Ksp = 5.2 × 10–11

    1. 1.29 × 10–5
    2. 4.49 × 10–4
    3. 0.0146
    4. 0.0886
    5. 0.115

    Solution


  2. Which of the following could you add to a saturated Ca3(PO4)2 aqueous solution to cause the solute to precipitate?

    1. AgCl
    2. Na3PO4
    3. KBr
    4. MgBr2
    5. H2O

    Solution


  3. 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?

    1. 4.22 × 10–11
    2. 1.28 × 10–7
    3. 3.60 × 10–4
    4. 2.30 × 10–3
    5. 10.3

    Solution


  4. The solubility product of CuCl is 1.20 × 10–6. What is the solubility of CuCl (in g L–1)?

    1. 1.09 × 10–3
    2. 3.41 × 10–2
    3. 0.26
    4. 1.44
    5. 43.21

    Solution


  5. Which compound is the least soluble in 1 L of water (at 25 °C)?

    1. HgS, Ksp = 1.8 × 10–53
    2. PbS, Ksp = 7.0 × 10–29
    3. AgI, Ksp = 1.5 × 10–16
    4. CuBr, Ksp = 1.5 × 10–9
    5. CuCl, Ksp = 1.2 × 10–6

    Solution


  6. 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?

    1. BaCO3
    2. Fe(OH)2
    3. NH3
    4. HCl
    5. PbF2

    Solution


  7. 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. 1.5 × 10–11
    2. 1.6 × 10–10
    3. 1.7 × 10–10
    4. 1.8 × 10–10
    5. 1.9 × 10–10

    Solution




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