A) both\[AgCl\]and\[AgI\]are sparingly soluble
B) the\[{{K}_{sp}}\]of\[AgI\]is lower than\[{{K}_{sp}}\]of\[AgCl\]
C) the\[{{K}_{sp}}\]of\[AgI\]is higher than\[{{K}_{sp}}\]of\[AgCl\]
D) both\[AgCl\]and\[AgI\]have same solubility product
Correct Answer: B
Solution :
On adding KI, the equilibrium\[AgCl+KIKCl+AgI\]is shifted towards right. This means that\[AgI\]is less soluble than\[AgCl\]. In other words.\[{{K}_{sp}}\]of \[AgI\]is less than\[{{K}_{sp}}\]of\[AgCl\].
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