Multiple Choice
Which one of the following compounds will not be soluble in water?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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In which of the following solutions will AgCl be most soluble?
A
A solution containing aqueous NH3
B
Pure water
C
A solution containing AgNO3
D
A solution containing NaCl
Verified step by step guidance1
Recall that the solubility of a salt like AgCl depends on the common ion effect and complex ion formation. AgCl dissociates as: $\$AgCl_{(s)} \rightleftharpoons Ag^{+}_{(aq)} + Cl^{-}_{(aq)}$.
In pure water, AgCl dissolves to a limited extent based on its solubility product constant ($K_{sp}$), with no additional ions affecting the equilibrium.
In a solution containing AgNO$_3$, there is an increase in $Ag^{+}$ ions, which shifts the equilibrium to the left (Le Chatelier's principle), decreasing AgCl solubility due to the common ion effect.
In a solution containing NaCl, there is an increase in $Cl^{-}$ ions, which also shifts the equilibrium to the left, decreasing AgCl solubility due to the common ion effect.
In a solution containing aqueous NH$_3$, $Ag^{+}$ ions form a complex ion with NH$_3$ (e.g., $[Ag(NH_3)_2]^+$), effectively removing free $Ag^{+}$ ions from solution and shifting the equilibrium to the right, increasing AgCl solubility.
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