When $NH_4Cl$ is added to $NH_4OH$ solution,the dissociation of $NH_4OH$ is reduced. This is due to:

The solubility product of $AgCl$ is $8 \times 10^{-6}$. Find its new solubility in the presence of $0.01 \ M \ NaCl$.

The addition of $HCl$ will not suppress the ionization of

Calculate the solubility of $AgCl(s)$ in $0.1 \ M \ NaCl$ at $25 \ ^oC$. Given ${K_{sp}}(AgCl) = 2.8 \times 10^{-10}$.

We have taken a saturated solution of $AgBr$. The $K_{sp}$ of $AgBr$ is $12 \times 10^{-14}$. If $10^{-7} \ mol$ of $AgNO_3$ are added to $1 \ L$ of this solution,find the conductivity (specific conductance) of this solution in terms of $10^{-7} \ S \ m^{-1}$ units.
Given: $\lambda^{\circ}_{(Ag^{+})} = 6 \times 10^{-3} \ S \ m^2 \ mol^{-1}$,$\lambda^{\circ}_{(Br^{-})} = 8 \times 10^{-3} \ S \ m^2 \ mol^{-1}$,$\lambda^{\circ}_{(NO_3^-)} = 7 \times 10^{-3} \ S \ m^2 \ mol^{-1}$.

Assertion $(A) :-$ When a small amount of strong acid or strong base is added to pure water,its $pH$ undergoes a change.
Reason $(R) :-$ Addition of an acid or base increases the degree of ionisation of water.