Question

When the following solutions are mixed together, what precipitate (if any) will form? a. \(\mathrm{FeSO}_{4}(a q)+\mathrm{KCl}(a q)\) b. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q)\) c. \(\mathrm{CaCl}_{2}(a q)+\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)\) d. \(\mathrm{K}_{2} \mathrm{~S}(a q)+\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q)\)

Short answer

The precipitates formed for each reaction are: a. No precipitate b. \(Al(OH)_3\) c. \(CaSO_4\) d. \(NiS\)

Step-by-step solution

Identify ions present in each solution

Write the ionic forms of each compound: a. \(FeSO_4 (aq) \) = \(Fe^{2+}\) + \(SO_4^{2-}\) \\ \(KCl (aq) \) = \(K^+\) + \(Cl^-\) b. \(Al(NO_3)_3 (aq) \) = \(Al^{3+}\) + \(3NO_3^-\) \\ \(Ba (OH)_2 (aq) \) = \(Ba^{2+}\) + \(2OH^-\) c. \(CaCl_2 (aq) \) = \(Ca^{2+}\) + \(2Cl^-\) \\ \(Na_2 SO_4 (aq)\) = \(2Na^+\) + \(SO_4^{2-}\) d. \(K_2 S (aq) \) = \(2K^+\) + \(S^{2-}\) \\ \(Ni (NO_3)_2 (aq) \) = \(Ni^{2+}\) + \(2NO_3^-\)

Apply solubility rules

Determine which of the possible products of the combinations of solutions are insoluble. a. Possible products: \(FeCl_2\) and \(K_2SO_4\) \\ b. Possible products: \(Al(OH)_3\) and \(Ba(NO_3)_2\) \\ c. Possible products: \(CaSO_4\) and \(2NaCl\) \\ d. Possible products: \(K_2(NO_3)_2\) and \(NiS\) For each combination, check the solubility rules: a. \(FeCl_2\) is soluble and \(K_2SO_4\) is soluble. \\ b. \(Al(OH)_3\) is insoluble, and \(Ba(NO_3)_2\) is soluble. \\ c. \(CaSO_4\) is slightly insoluble, and \(2NaCl\) is soluble. \\ d. \(K_2(NO_3)_2\) is soluble, and \(NiS\) is insoluble.

Identify precipitates

Based on the solubility rules, identify which reactions form precipitates: a. No precipitate is formed. b. A precipitate of \(Al(OH)_3\) is formed. c. A slightly insoluble precipitate of \(CaSO_4\) is formed. d. A precipitate of \(NiS\) is formed. The precipitates formed for each reaction are: a. No precipitate \\ b. \(Al(OH)_3\) \\ c. \(CaSO_4\) \\ d. \(NiS\)