Ionic Equilibrum - Physical Chemistry - Chemistry Previous Year Questions

The \([\mathrm{OH}]^{-}\) in a solution is \(1 \mathrm{~mol} \mathrm{~L}^{-1}\). The \(\mathrm{pH}\) of the solution is

The solubility of \(\mathrm{Fe}(\mathrm{OH})_3\) is \(x \mathrm{~mol} \mathrm{~L}^{-1}\). Its \(K_{\mathrm{sp}}\) would be

What is the degree of dissociation of \(0.05 \mathrm{~M~NH}_3\) if its \(\mathrm{pK}{ }_a\) is 4.75 and \(\mathrm{pH}\) is 11 ?

Using the Gibbs free energy change, $\Delta G^{\circ}=+63.3 \mathrm{~kJ}$. For the reaction,

$$\mathrm{Ag}_2 \mathrm{CO}_3 \longrightarrow 2 \mathrm{Ag}^{+}(a q)+\mathrm{CO}_3^{2-}(a q)$$

The $K_{\text {sp }}$ of $\mathrm{Ag}_2 \mathrm{CO}_3(s)$ in water at $25^{\circ} \mathrm{C}$ is

A 0.02 M solution of pyridinium hydrochloride has $\mathrm{pH}=3.44$. The ionisation constant of pyridine is