Question

If the solubility(s) of ${\left(AgCl\right)}_{(s)}$ in $0.1MNaCl$ solution is $aX10^{-10}$ , then what will be the value of ${}^{\prime }{a}^{\prime }$ if the given solubility product of $AgCl$ is $1.6x10^{-10}$ ?

Answer 1

Answer: 16

${\left(AgCl\right)}_{(s)}\_{(aq)}^{+}+C{l}_{(aq)}^{-}$
Concentration $-$
$SS+0.1$ $\left(M\right)$
$K_{sp}=\left[A{g}^{+}\right]\left[C{l}^{-}\right]$
$\therefore 1.6\times {\left(10\right)}^{-10}=(S)(S+0.1)$
$\therefore 1.6\times {\left(10\right)}^{-10}=S\times 0.1(\because S<<0.1)$
$\therefore S=16\times 10^{-10}M$