Multiple Choice
In which of the following solutions will AgCl be most soluble?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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Which of the following compounds is more soluble in an acidic solution than in pure water?
A
KNO_3
B
CaCO_3
C
NaCl
D
BaSO_4
Verified step by step guidance1
Identify the nature of each compound and whether it can react with H+ ions in an acidic solution. Compounds that contain basic anions (like carbonate CO_3^{2-}) can react with H+ and thus increase solubility in acid.
Recall that KNO_3 and NaCl are salts of strong acids and strong bases, so their solubility is generally unaffected by pH changes.
Recognize that CaCO_3 contains the carbonate ion (CO_3^{2-}), which can react with H+ ions according to the equilibrium: $\mathrm{CO_3^{2-} + 2H^+ \rightleftharpoons H_2CO_3}$, shifting the equilibrium and increasing solubility in acidic solution.
Understand that BaSO_4 is a salt of a strong acid (H_2SO_4) and a strong base (Ba(OH)_2), and its solubility is not significantly affected by acidic conditions.
Conclude that CaCO_3 is more soluble in acidic solution than in pure water due to the reaction of carbonate ions with H+, which removes carbonate from solution and drives dissolution.
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