The $K_{sp}$ of $AgCl$ is $1.8 \times 10^{-10}$. The concentration of $Cl^-$ required to initiate the precipitation of $AgCl$ in a solution containing $4 \times 10^{-3} \ M \ Ag^+$ is:

Solubility products $(K_{sp})$ of the salts of types $MX, MX_2$ and $M_3X$ at temperature $T$ are $4.0 \times 10^{-8}, 3.2 \times 10^{-14}$ and $2.7 \times 10^{-15}$ respectively. Solubilities (in $mol \text{ dm}^{-3}$) of the salts at temperature $T$ are in the order:

Which compound does not dissolve in acetic acid?

Which of the following precipitates does not dissolve even in a large excess of $NH_4OH$?

The solubility of a sparingly soluble salt $A_x B_y$ in water at $25\,^{\circ}C$ is $1.4 \times 10^{-4} \ M$. The solubility product is $1.1 \times 10^{-11}$. The values of $x$ and $y$ may be

In a qualitative analysis, $Bi^{3+}$ is detected by the appearance of a precipitate of $BiO(OH)(s)$. Calculate the $pH$ when the following equilibrium exists at $298 \text{ K}$:
$BiO(OH)(s) \rightleftharpoons BiO^{+}(aq) + OH^{-}(aq)$,
$K = 4 \times 10^{-10}$
(Given: $\log 2 = 0.3010$)