$pH$ of a buffer solution decreases by $0.02$ units when $0.12\,g$ of acetic acid is added to $250\, mL$ of a buffer solution of acetic acid and potassium acetate at $27^{\circ} C$. The buffer capacity of the solution is
- 0.1
- 10
- 1
- 0.4
The Correct Option is D
Solution and Explanation
where, $d C_{ HA }=$ no. of moles of acid added per litre
$d_{ pH } =$ change in $pH $
$d C_{ HA } =\frac{\text { moles of acetic acid }}{\text { volume }} $
$=\frac{0.12 / 60}{250 / 1000}=\frac{1}{125} $
$\therefore \beta =\frac{1 / 125}{0.02}=\frac{1}{2.5}=0.4$
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Concepts Used:
Buffer solutions
The buffer solution is a solution that is able to maintain its Hydrogen ion concentration (pH) with only minor changes on the dilution or addition of a small amount of either acid or base. They are used in fermentation, food preservatives, drug delivery, printing, the activity of enzymes and many more.
Buffer solutions are aqueous solutions containing a weak acid and its salt - acid buffer or a weak base and its salt - base buffer.
Types of Buffer Solution
Acidic Buffers
These solutions are used to maintain acidic environments. Also, it has acidic pH and is prepared by mixing a weak acid and its salt with a strong base. An aqueous solution of an equal concentration of acetic acid and sodium acetate has a pH of 4.74.
Alkaline Buffers
These solutions are used to maintain basic conditions. It has a basic pH and is prepared by mixing a weak base and its salt with strong acid. The aqueous solution of an equal concentration of ammonium hydroxide and ammonium chloride has a pH of 9.25.