Problem 1
An example of an acid buffer is a solution of (a) ammonium acetate (b) a mixture of \(\mathrm{NH}_{4} \mathrm{OH}+\mathrm{NH}_{4} \mathrm{Cl}\) (c) a mixture of \(\mathrm{CH}_{3} \mathrm{COOH}+\mathrm{CH}_{3} \mathrm{COONa}\) (d) a solution of \(\mathrm{CH}_{3} \mathrm{COONa}\)
Problem 2
An example of a basic buffer is a solution of (a) \(\mathrm{NH}_{4} \mathrm{OH}+\mathrm{NH}_{4} \mathrm{Cl}\) (b) \(\mathrm{NH}_{4} \mathrm{OH}+\mathrm{HCl}\) (c) \(\mathrm{CH}_{3} \mathrm{COONH}_{4}\) (d) \(\mathrm{NH}_{4} \mathrm{OH}+\mathrm{NaOH}\)
Problem 3
In spite of various acid and base-producing reactions in our body, the pH of our blood is (a) \(5.4\) (b) \(6.4\) (c) \(7.4\) (d) \(8.4\)
Problem 4
The \(\mathrm{pH}\) of an acidic buffer according to the Henderson equation is given by (a) \(\mathrm{p} K_{a}-\log \frac{[\mathrm{Salt}]}{[\mathrm{Acid}]}\) (b) \(\mathrm{pK}_{a}+\log \frac{[\mathrm{Salt}]}{[\mathrm{Acid}]}\) (c) \(\mathrm{p} \boldsymbol{K}_{a}+\log \frac{[\mathrm{Acid}]}{[\mathrm{Salt}]}\) (d) \(-p k_{a}+\log \frac{[\text { Salt }]}{[\text { Acid }]}\)
Problem 5
Choose the correct statement from the following: (a) \(\mathrm{pOH}=-\mathrm{p} K_{b}+\log \frac{[\mathrm{Salt}]}{[\text { Base }]}\) (b) \(\mathrm{pOH}=\mathrm{p} K_{b}+\log \frac{[\mathrm{Base}]}{[\mathrm{Salt}]}\) (c) \(\mathrm{pOH}=-\mathrm{p} K_{b}-\log \frac{[\text { Salt }]}{[\text { Base }]}\) (d) \(\mathrm{pOH}=\mathrm{p} K_{b}+\log \frac{[\mathrm{Salt}]}{[\mathrm{Base}]}\)
Problem 6
The \(\mathrm{pH}\) value of a solution obtained by mixing \(5 \mathrm{~g}\) of acetic acid and \(7.5 \mathrm{~g}\) of sodium acetate and making the volume to \(500 \mathrm{~mL}\left(\mathrm{~K}_{\mathrm{CH}_{3} \mathrm{COOH}}=1.8 \times 10^{-5}\right)\) is (a) \(4.78\) (b) \(3.78\) (c) \(5.78\) (d) zero
Problem 7
The pH of a solution of strong acid and weak base at the equivalence point is (a) 7 (b) more than 7 (c) less than 7 (d) none of the above
Problem 8
Heat of neutralisation of a strong acid and weak base is less than \(57.3 \mathrm{~kJ} \mathrm{~mol}^{-1}\). This is because (a) all the acid is not ionised (b) all the base is not ionised (c) the ionisation is complete but further reaction does not take place (d) some of the heat is transferred to the surroundings
Problem 9
Both anionic and cationic hydrolysis occur in the case of (a) salts of strong acid and strong base (b) salts of strong acid and weak base (c) salts of weak acid and strong base (d) salts of weak acid and weak base
Problem 10
The \(\mathrm{pH}\) of a solution of salt of strong acid and weak base is given by a) \(\frac{1}{2}\left(\log K_{w^{\prime}}+\log K_{b}+\log C\right)\) (b) \(\frac{1}{2}\left(\log K_{w}-\log K_{b}-\log C\right)\) c) \(\frac{1}{2}\left(\log K_{w^{\prime}}-\log K_{b}+\log C\right)\) d) \(\frac{1}{2}\left(-\log K_{w^{\prime}}-\log K_{b}-\log C\right)\)
