Altering the pH of a solution of which of the following will change the solubility of that substance?
A.
\[ K_{sp}(\text{PbSO}_4) = 1.6 \times 10^{-8} \]
B.
\[ K_{sp}(\text{PbF}_2) = 3.6 \times 10^{-8} \]
C.
\[ K_{sp}(\text{PbCl}_2) = 1.7 \times 10^{-5} \]
D.
\[ K_{sp}(\text{PbI}_2) = 7.9 \times 10^{-9} \]
Exam No：AP Chemistry Problem Set 8 Year：2024 Question No：APChemistry2024AP0272
Answer:
A
Knowledge points:
8.3 Weak Acid and Base Equilibria
8.4 Acid-Base Reactions and Buffers
Solution:
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