Precipitation reactions and solubility rules Knowledge-Based Download PDF

Questions

1. 1.

   When an aqueous solution containing 0.45 mol of calcium chloride, $\text{CaCl}_2$, is mixed with an aqueous solution containing 0.40 mol of potassium phosphate, $\text{K}_3\text{PO}_4$, a precipitation reaction occurs. What is the maximum amount of precipitate, in moles, that can form?

   • A) 0.45 mol
   • B) 0.30 mol
   • C) 0.20 mol
   • D) 0.15 mol
2. 2.

   Which of the following anions will form an insoluble precipitate with $\text{Ag}^+$ ions but remain soluble with $\text{Cu}^{2+}$ ions in an aqueous solution?

   • A) $\text{Cl}^-$
   • B) $\text{NO}_3^-$
   • C) $\text{S}^{2-}$
   • D) $\text{CO}_3^{2-}$
3. 3.

   When aqueous solutions of iron(III) chloride, $\text{FeCl}_3$, and sodium hydroxide, $\text{NaOH}$, are mixed, a precipitate forms. Which of the following is the correct net ionic equation for this reaction?

   • A) $\text{Na}^+(aq) + \text{Cl}^-(aq) \rightarrow \text{NaCl}(s)$
   • B) $\text{Fe}^{3+}(aq) + \text{OH}^-(aq) \rightarrow \text{FeOH}^{2+}(s)$
   • C) $\text{Fe}^{3+}(aq) + 3\text{OH}^-(aq) \rightarrow \text{Fe(OH)}_3(s)$
   • D) $\text{FeCl}_3(aq) + 3\text{NaOH}(aq) \rightarrow \text{Fe(OH)}_3(s) + 3\text{NaCl}(aq)$
4. 4.

   When aqueous solutions of barium chloride, $\text{BaCl}_2$, and sodium sulfate, $\text{Na}_2\text{SO}_4$, are mixed together, a precipitate forms. Which of the following correctly identifies the spectator ions in this reaction?

   • A) $\text{Ba}^{2+}$ and $\text{SO}_4^{2-}$
   • B) $\text{Ba}^{2+}$ and $\text{Cl}^-$
   • C) $\text{Na}^+$ and $\text{Cl}^-$
   • D) $\text{Na}^+$ and $\text{SO}_4^{2-}$
5. 5.

   Which of the following pairs of aqueous solutions produces an insoluble precipitate when mixed together?

   • A) $\text{AgNO}_3\text{(aq)}$ and $\text{NaCl(aq)}$
   • B) $\text{CuSO}_4\text{(aq)}$ and $\text{NH}_4\text{Cl(aq)}$
   • C) $\text{K}_2\text{CO}_3\text{(aq)}$ and $\text{NaNO}_3\text{(aq)}$
   • D) $\text{Ba(NO}_3\text{)}_2\text{(aq)}$ and $\text{LiCl(aq)}$