Seema Saini Solutions for Chapter: Ionic Equilibrium, Exercise 5: DPP 7.5

The $\mathrm{pH}$ of a buffer is $4.745$. When $0.01$ mole of $\mathrm{NaOH}$ is added to $1$ litre of it, the $\mathrm{pH}$ changes to $4.832$, calculate its buffer capacity.

What is the $\mathrm{pH}$ of the solution when $0.2$ mole of hydrochloric acid is added to one litre of a solution containing $1 \mathrm{M}$ acetic acid and acetate ion? Assume that the total volume is one litre. $\left({\mathrm{K}}_{\mathrm{a}}\text{ for }{\mathrm{CH}}_3\mathrm{COOH}=1.8\times \right.{10}^{-5})$

Which of the following can be used as a buffer solution?

On diluting a buffer solution, its $\mathrm{pH}$:

Choose the correct statement.

Which of the following will function as buffer?

In a buffer solution consisting of ${\mathrm{NaH}}_2{\mathrm{PO}}_4$ and ${\mathrm{Na}}_2{\mathrm{HPO}}_4$

$\left(1\right) {\mathrm{NaH}}_2{\mathrm{PO}}_4$ is a acid and${\mathrm{Na}}_2{\mathrm{HPO}}_4$ is salt.

$\left(2\right)$ The $\mathrm{pH}$ of the solution can be calculated using the relation: $\mathrm{pH}={\mathrm{K}}_{{\mathrm{a}}_2}+{\log }_{10}\frac{\left[{\mathrm{HPO}}_4^{2-}\right]}{\left.{\mathrm{H}}_2{\mathrm{PO}}_4^{-}\right]}$.

$\left(3\right)$ The ${\mathrm{Na}}_2{\mathrm{HPO}}_4$ is acid and ${\mathrm{NaH}}_2{\mathrm{PO}}_4$ is salt.

$\left(4\right)$ The $\mathrm{pH}$ cannot be calculated.

In a buffer solution of ${\mathrm{NaH}}_2{\mathrm{PO}}_4$ and ${\mathrm{Na}}_2{\mathrm{HPO}}_4$,