Ionic Equilibrium

Assertion : Some salts are sparingly soluble in water at room temperature. Reason : The entropy increases on dissolving the salts.

Which of the following has maximum solubility at low $\mathrm{pH}$ ?

Calculate ionisation constant for pyridinium hydrogen chloride. (Given that $\mathrm{H}^{+}$ion concentration is $3.6 \times 10^{-4} \mathrm{M}$ and its concentration is $0.02 \mathrm{M}$.)

When $50 \mathrm{~mL}$ of $0.1 \mathrm{M} \mathrm{NH}_3$ is mixed with $10 \mathrm{~mL}$ of $0.1 \mathrm{M} \mathrm{HCl}$ then what is the $\mathrm{pH}$ of resultant solution? $\left(\mathrm{p} K_b=4.75\right)$

$\mathrm{ZnO}$ is white when cold and yellow when heated. It is due to the development of

Calculate the overall complex dissociation equilibrium constant for the $\left[\mathrm{Cu}\left(\mathrm{NH}_3\right)_4\right]^{2+}$ ions, given that stability constant $\left(\beta_4\right)$ for this complex is $2.1…

Assertion : $\mathrm{H}_2 \mathrm{~S}$ is stronger acid than $\mathrm{PH}_3$. Reason : $S$ is more electronegative than $\mathrm{P}$, conjugate base $\mathrm{HS}^{-}$is more stable than $\mathrm{H}_2 \mathrm{P}^{-}$.

Assertion: $\mathrm{Sb}_2 \mathrm{~S}_3$ is not soluble in yellow ammonium sulphide. Reason : The common ion effect due to $S^{2-}$ ions reduces the solubility of $\mathrm{Sb}_2 \mathrm{~S}_3$.

The pair of amphoteric hydroxides is

Assertion: Mixture of $\mathrm{CH}_3 \mathrm{COOH}$ and $\mathrm{CH}_3 \mathrm{COONH}_4$ is an example of acidic buffer. Reason: Acidic buffer contains equimolar mixture of weak acid and its salt with weak base.

What will be the solubility product of $A X_3$ ?

Which has the highest $\mathrm{pH}$ ?