Buffer Solutions

Penicillin preparations are stabilised by the addition of sodium _____ as a buffer.

Write the uses of buffer solutions.

Write the use of buffer solutions in the human body.

Write any one use of buffer solutions.

What are simple buffers?

What is the mixed buffer solution?

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.

The ionisation constant of $\mathrm{NH}_{4}^{+}$ in water is $5.6 \times 10^{-10} \mathrm{at}$ $25^{\circ} \mathrm{C} .$ The rate constant for the reaction of $\mathrm{NH}_{4}^{+}$ and $\mathrm{OH}^{-}$ to form $\mathrm{NH}_{3}$ and $\mathrm{H}_{2} \mathrm{O}$ at $25^{\circ} \mathrm{C}$ is $3.4 \times 10^{10}$ litre

$\mathrm{mol}^{-1} \mathrm{sec}^{-1} .$ If equilibrium constant of water at $25^{\circ} \mathrm{C}$ is $1.8 \times 10^{-16},$ thenThe $\mathrm{pH}$ of a mixture of

$0.1 \mathrm{M} {\mathrm{NH}}_4\mathrm{OH}$ and
$0.1\mathrm{M} {\left({\mathrm{NH}}_4\right)}_2{\mathrm{SO}}_4$ solution is $\left[{\mathrm{K}}_{\mathrm{a}} \text{of }{\mathrm{NH}}_4^{+}\text{ is} 5.6\times {10}^{-10} \text{and} \log 1.78=0.25\right]$ 

A buffer of acetic acid $({\mathrm{pK}}_{\mathrm{a}}=4.8)$ with sodium acetate, when ${\mathrm{CH}}_3\mathrm{COOH}$ and ${\mathrm{CH}}_3\mathrm{COONa}$ are present in equivalent amounts, has a$\mathrm{pH}$ range of

Consider the titration of weak monobasic acid HA using 0.1 M NaOH. If initially 100 mL of 0.1 M HA is taken then find the volume of NaOH (in mL) added so that pH of mixture become equal to 5.