Question

$AgCl+KIKCl+AgI$ In the above reaction as KI is added, the equilibrium is shifted towards right giving more. $AgI$ precipitate, because

• 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

Answer 1

Answer: (B)

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 $AgCl$ .