객관식
Which type of salts will generally be more soluble in an acidic solution than in pure water?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
객관식
Which of the following compounds will be more soluble in acidic solution than in pure water?
A
BaSO_4
B
KNO_3
C
CaCO_3
D
NaCl
검증된 단계별 안내1
Step 1: Understand the concept of solubility and how it can be affected by pH. Some compounds contain anions that can react with H\_3O\^+ (acidic protons), shifting the equilibrium and increasing solubility in acidic solutions.
Step 2: Identify the anions in each compound: BaSO\_4 contains SO\_4\^{2-}, KNO\_3 contains NO\_3\^-, CaCO\_3 contains CO\_3\^{2-}, and NaCl contains Cl\^-.
Step 3: Recognize that carbonate ion (CO\_3\^{2-}) is a base that reacts with acids to form bicarbonate (HCO\_3\^-) or carbonic acid (H\_2CO\_3), which decomposes to CO\_2 and water. This reaction reduces the concentration of CO\_3\^{2-} in solution, shifting the dissolution equilibrium to dissolve more CaCO\_3.
Step 4: Write the dissolution equilibrium for CaCO\_3: \(\mathrm{CaCO_3 (s) \rightleftharpoons Ca^{2+} (aq) + CO_3^{2-} (aq)}\) and the acid-base reaction: \(\mathrm{CO_3^{2-} + H_3O^+ \rightarrow HCO_3^- + H_2O}\), which consumes carbonate ions and drives more CaCO\_3 to dissolve.
Step 5: Conclude that compounds like BaSO\_4, KNO\_3, and NaCl do not have anions that react significantly with acid, so their solubility is not enhanced in acidic solution, unlike CaCO\_3.
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