Multiple Choice
Which of the following statements is true about the solubility of O_2 (g) in H_2O (l)?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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In which of the following aqueous solutions would you expect AgCl to have the lowest solubility?
A
Pure water
B
0.10 M NaNO_3
C
0.10 M NaCl
D
0.10 M Na_2SO_4
Verified step by step guidance1
Understand that the solubility of AgCl in aqueous solution is affected by the common ion effect, which occurs when a solution already contains one of the ions present in the salt (Ag^+ or Cl^-).
Identify the ions present in each solution: Pure water has no additional ions; 0.10 M NaNO_3 provides Na^+ and NO_3^- ions, which do not affect AgCl solubility; 0.10 M NaCl provides Na^+ and Cl^- ions, introducing a common ion (Cl^-) that will reduce AgCl solubility; 0.10 M Na_2SO_4 provides Na^+ and SO_4^{2-} ions, which do not share ions with AgCl.
Recall the solubility equilibrium for AgCl: $\mathrm{AgCl (s) \rightleftharpoons Ag^{+} (aq) + Cl^{-} (aq)}$ and the solubility product constant expression: $K_{sp} = [Ag^{+}][Cl^{-}]$.
Recognize that adding Cl^- ions from NaCl shifts the equilibrium to the left (Le Chatelier's principle), decreasing the concentration of dissolved Ag^+ and thus lowering the solubility of AgCl.
Conclude that among the given solutions, 0.10 M NaCl will cause the lowest solubility of AgCl due to the common ion effect from Cl^- ions.
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