In this set of practice problems, we will work on calculating the solubility product constant (*K*_{sp}) from the molar solubility of the compound, and vice versa, the *K*_{sp} of compounds in pure water, in the presence of salts with common ions, and when the pH of the solution is changed.

#### Practice

Write balanced equations for the dissolution reactions and solubility product expressions for the following* c*ompounds.

**a.** Ca(OH)_{2} **b. **Al(OH)_{3} **c. **Ba_{3}(PO_{4})_{2} **d. **Pb(IO_{3})_{2} **e. **FeCO_{3} **f. **Ag_{2}S

Calculate the *K _{sp}* for calcium oxalate, CaC

_{2}O

_{4}given its solubility in water is 4.8 x 10

^{-5}mol/L.

Calculate the *K _{sp}* for silver sulfate, Ag

_{2}SO

_{4}given its solubility in water is 0.0162 mol/L.

* *

Determine the *K*_{sp} for calcium hydroxide, Ca(OH)_{2} if its saturated solution has a pH of 12.35.

Calculate the concentration of phosphate ions in a saturated solution of Ca_{3}(PO_{4})_{2} given that *K*_{sp} for Ca_{3}(PO_{4})_{2} is 1.3 x 10^{-32} mol/L.

The *K*_{sp} for Hg_{2}Cl_{2 }is 1.1 x 10^{-18}. Calculate the molar solubility of Hg_{2}Cl_{2 }at 20 ^{o}C.

The concentration of Cl^{–} ions in a solution saturated with PbCl_{2}(*s*) is 0.0318 *M*. Calculate *K*_{sp} for PbCl_{2}.

Calculate the solubility of silver phosphate, Ag_{3}PO_{4} in grams per liter of water, given that *K*_{sp }is 1.8 x 10^{-18}. Ignore any acid–base properties of the ions.

The *K*_{sp} for chromium (III) hydroxide, Cr(OH)_{3} is 6.7 x 10^{-31}. Calculate the solubility of Cr(OH)_{3} in g/L of water.

Calculate the molar solubility of Al(OH)_{3} (*K*_{sp} = 2.0 x 10^{-32}) in each of the following solutions.

**a)** Pure water

**b)** a solution buffered at pH = 6.0

**c)** a solution buffered at pH = 10.0

The *K*_{sp} for silver chromate (Ag_{2}CrO_{4}) is 9.0 x 10^{-12}. Calculate the solubility of silver chromate in each of the following solutions.

**a)** Pure water

**b) **0.15 *M *AgNO_{3}

**c) **0.20 *M *Na_{2}CrO_{4}

Calculate the solubility of solid Ba_{3}(PO_{4})_{2} (*K*_{sp} = 6.0 x 10^{-39}) in a 0.10 *M *K_{3}PO_{4} solution.

The *K*_{sp} for zinc hydroxide, Zn(OH)_{2} is 4.5 x 10^{-17}. Determine the pH of a saturated solution of zinc hydroxide.

If 30.0 mL of 0.10 *M *Ba(NO_{3})_{2} are added to 50.0 mL of 0.10 *M *Na_{2}SO_{4}, will there be any precipitation observed? *K*_{sp} for BaSO_{4} is 1.5 × 10^{−}^{9}

Will a precipitate form when 200. mL of 0.035 *M *Pb(NO_{3})_{2} is added to 200. mL of 0.065 *M *NaCl? *K*_{sp} for PbCl_{2} is 1.6 × 10^{−}^{5}.

Check Also

- Buffer Solutions
- The Henderson–Hasselbalch Equation
- The pH of a Buffer Solution
- Preparing a Buffer with a Specific pH
- The Common Ion Effect
- The pH and p
*K*a Relationship - Strong Acid–Strong Base Titrations
- Titration of a Weak Acid by a Strong Base
- Titration of a Weak Base by a Strong Acid
- Titration of Polyprotic Acids
- Buffer Solutions Practice Problems
*K*sp and Molar Solubility- The Effect of a Common Ion on Solubility
- The Effect of pH on Solubility
- Will a Precipitate Form?
*K*sp and*Q*