Buffer Solutions

The pH of the solution can be kept constant with the help of

Which among the following pairs constitute a buffer?

Addition of sodium hydroxide solution to a weak acid (HA) results in a buffer of pH 6. If ionization constant of HA is ${10}^{-5}$, the ratio of salt to acid concentration in the buffer solution will be:

Which of the following pairs will not constitute a buffer solution?

A buffer solution can be prepared by mixing equal volumes of

Among the following, the correct statement is

What is the concentration of sodium acetate that needs to be added to a $0.01 \mathrm{M}$ solution of acetic acid with equal volumes to give a solution of $\mathrm{pH}=5.5?$

$\left({\mathrm{pK}}_{\mathrm{a}}\text{ of }{\mathrm{CH}}_3\mathrm{COOH}=4.5\right)$

Choose the wrong statement from the following:

For preparing a buffer solution of $\mathrm{pH}=9$, by mixing ammonium chloride and ammonium hydroxide, the ratio of concentrations of salt and base should be_______ $\left({\mathrm{K}}_{\mathrm{b}}={10}^{-3}\right)$

A student prepares 2 L buffer solution of 0.3 M NaH₂PO₄ and 0.3 M Na₂HPO₄. The solution is divided in half between the two compartments (each containing 1 L buffer) of an electrolysis cell, using Pt electrodes. Assume that the only reaction is the electrolysis of water and the electrolysis is carried out for 200 min with a constant current of 0.965 A.

$\left[\text{Assume that}{\text{ pK}}_{\text{a}\left({\text{H}}_2{\text{PO}}_4^{\ominus }\right)}=\text{7.2}\right]$  [Given log 2.33 = 0.37]

pH at anode is

For next two question please follow the same

A student prepares 2 L buffer solution of 0.3 M NaH₂PO₄ and 0.3 M Na₂HPO₄. The solution is divided in half between the two compartments (each containing 1 L buffer) of an electrolysis cell, using Pt electrodes. Assume that the only reaction is the electrolysis of water and the electrolysis is carried out for 200 min with a constant current of 0.965 A.

$\left[\text{Assume that}{\text{ pK}}_{\text{a}\left({\text{H}}_2{\text{PO}}_4^{\ominus }\right)}=\text{7.2}\right]$  [Given log 2.33 = 0.37]

pH at cathode is

$100 \mathrm{mL}$ of $0.10 \mathrm{M}$ ${\mathrm{NH}}_4\mathrm{OH}$ mixed with $100 \mathrm{mL}$ of $0.05 \mathrm{M}$ $\mathrm{HCl}$ solution

The $\mathrm{pH}$ of $100 \mathrm{mL}$ of $0.10 \mathrm{M}$ $\mathrm{NaOH}$ mixed with $100 \mathrm{mL}$ $0.10 \mathrm{M}$ ${\mathrm{CH}}_3\mathrm{COOH}$ solution is

Blood is a buffer of H2CO3 and HCO3- with pH of 7.4. What will be the ratio of HCO3- to H2CO3 in blood.

Identify the buffer solution among the following.

Calculate the $\mathrm{pH}$ of a buffer solution prepared by adding $10 \mathrm{mL}$ of  $0.1 \mathrm{M} {\mathrm{CH}}_3\mathrm{COOH}$ and $20 \mathrm{mL}$ of $0.1 \mathrm{M}$ sodium acetate.
(Given: ${\mathrm{pK}}_{\mathrm{a}}$  of ${\mathrm{CH}}_3\mathrm{COOH}=4.74$)

What will be the $\mathrm{pH}$ of resultant mixture when $20\mathrm{ml}$ of $0.1\mathrm{M}{\mathrm{H}}_2{\mathrm{SO}}_4$ solution is added to $30\mathrm{mL}$ of $0.2\mathrm{M}{\mathrm{NH}}_4\mathrm{OH}$ solution ?

Given:- $\left[{\mathrm{pk}}_{\mathrm{b}}\mathrm{ }\mathrm{of}\mathrm{ }{\mathrm{NH}}_4\mathrm{OH}=4.7\right]$

Calculate $\mathrm{pH}$ of solution containing $0.3 \mathrm{M}$  ${\mathrm{NH}}_4^{+}$ , $0.2 \mathrm{M}$ ${\mathrm{NH}}_4\mathrm{OH}$ $\left({\mathrm{p}}_{{\mathrm{K}}_{\mathrm{b}}}=4.74\right)$ and  $0.01 \mathrm{M} \mathrm{HCl}$ having volume $100 \mathrm{ml}$ is

A basic buffer is prepared with maximum buffer capacity. Calculate the ratio of base to salt to be taken to increase its $\mathrm{pOH}$ by two.

A buffer solution contains equal concentration of ${\mathrm{X}}^{-}$ and $\mathrm{HX}, {\mathrm{K}}_{\mathrm{b}}$ for ${\mathrm{X}}^{-}$ is ${10}^{-10}.$ Calculate the $\mathrm{pH}$ of the buffer.