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Chapter 17: 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 \(\mathrm{CH}_{3} \mathrm{COONa}\)

Short Answer

Expert verified
Therefore, the correct answer is (c) a mixture of \(\mathrm{CH}_{3} \mathrm{COOH}+\mathrm{CH}_{3} \mathrm{COONa}\)

Step by step solution

01

Rule out single component solutions

First, note that an acid buffer cannot consist of a single substance. This is because a buffer requires a weak acid and its conjugate base to effectively mitigate changes in pH. Therefore, choices (a) and (d) can be eliminated because they consist of ammonium acetate and sodium acetate respectively, which are single substances.
02

Identifying the correct mixture

Next, let's consider the remaining choices, (b) a mixture of \(\mathrm{NH}_{4} \mathrm{OH}+\mathrm{NH}_{4} \mathrm{Cl}\) and (c) a mixture of \(\mathrm{CH}_{3} \mathrm{COOH}+\mathrm{CH}_{3} \mathrm{COONa}\). Neither component in choice (b) is a weak acid, so it does not fit the definition of an acid buffer. Both acetate acid and sodium acetate exist in choice (c). Since acetate acid is a weak acid and sodium acetate is its conjugate base, this mixture does qualify as an acid buffer.

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Most popular questions from this chapter

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) \(-p k_{a}+\log \frac{[\text { Salt }]}{[\text { Acid }]}\)

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) \(8.4\)

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

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

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) \(\frac{1}{2}\left(-\log K_{w^{\prime}}-\log K_{b}-\log C\right)\)
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