Solubility product constant (Ksp) Knowledge-Based Download PDF

Questions

1. 1.

   A solution contains barium ions at a concentration of $1.0 \times 10^{-3}\text{ M}$. Given that the solubility product constant ($K_{\text{sp}}$) of barium sulfate ($\text{BaSO}_4$) is $1.1 \times 10^{-10}$ at $25^\circ\text{C}$, what is the minimum concentration of sulfate ions ($\text{SO}_4^{2-}$) required to initiate the precipitation of $\text{BaSO}_4$?

   • A) $1.1 \times 10^{-7}\text{ M}$
   • B) $1.1 \times 10^{-13}\text{ M}$
   • C) $1.0 \times 10^{-5}\text{ M}$
   • D) $9.1 \times 10^{-8}\text{ M}$
2. 2.

   What is the molar solubility of silver chloride ($\text{AgCl}$) in a $0.10\text{ M}$ sodium chloride ($\text{NaCl}$) solution at $25^\circ\text{C}$? (Assume $K_{\text{sp}}$ for $\text{AgCl}$ is $1.8 \times 10^{-10}$ at $25^\circ\text{C}$.)

   • A) $1.3 \times 10^{-5}\text{ M}$
   • B) $1.8 \times 10^{-8}\text{ M}$
   • C) $1.8 \times 10^{-9}\text{ M}$
   • D) $3.6 \times 10^{-10}\text{ M}$
3. 3.

   Which of the following expressions correctly represents the solubility product constant ($K_{\text{sp}}$) in terms of the molar solubility ($s$) for a sparingly soluble salt with the general formula $\text{A}_3\text{B}_2$?

   • A) $K_{\text{sp}} = 6s^5$
   • B) $K_{\text{sp}} = 36s^5$
   • C) $K_{\text{sp}} = 72s^5$
   • D) $K_{\text{sp}} = 108s^5$
4. 4.

   The molar solubility of calcium fluoride ($\text{CaF}_2$) in water at $25^\circ\text{C}$ is $2.0 \times 10^{-4}\text{ M}$. What is the solubility product constant ($K_{\text{sp}}$) of $\text{CaF}_2$ at this temperature?

   • A) $1.6 \times 10^{-11}$
   • B) $3.2 \times 10^{-11}$
   • C) $8.0 \times 10^{-12}$
   • D) $4.0 \times 10^{-8}$