Question

Which of the following statements are true for a solution saturated with AgCl & AgBr. If their solubilities in mole/litre present in separate solutions are x & y respectively. The solubility product values of AgBr and AgCl are $5\times {10}^{-13}$ and $5\times {10}^{-10}$ respectively.

• A. $\left[A{g}^{+}\right]=\left[B{r}^{-}\right]+\left[C{l}^{-}\right]$
• B. $\left[C{l}^{-}\right]>\left[B{r}^{-}\right]$
• C. $\left[B{r}^{-}\right]>x$
• D. $\left[A{g}^{+}\right]=x+y$

Answer 1

Answer: (B)

$\left[C{l}^{-}\right]>\left[B{r}^{-}\right]$

The solubility product of AgBr is $5\times {10}^{-13}$.
The solubility product of AgCl is $5\times {10}^{-10}$.
Hence, the solubility product of AgBr is lower than the solubility product of AgCl and the solubility of AgBr is lower than the solubility of AgCl. So $\left[C{l}^{-}\right]>\left[B{r}^{-}\right]$.