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 , $dC_{HA}$ = no. of moles of acid added per litre
$d_{pH}$ = change in pH.
$dC_{HA} = \frac{\text{moles of acetic acid}}{\text{volume}}$
$ = \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.