The pH of a buffer solution containing 0.2 m | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) The $pH$ of an acidic buffer is calculated using the Henderson-Hasselbalch equation: $pH = pK_a + \log \frac{[Salt]}{[Acid]}$ Given: $[Salt] = [CH

Vedclass · Accepted Answer

$3.86$

Vedclass · Answer

(A) The $pH$ of an acidic buffer is calculated using the Henderson-Hasselbalch equation: $pH = pK_a + \log \frac{[Salt]}{[Acid]}$ Given: $[Salt] = [CH_3COONa] = 0.2 \ mol/L$ $[Acid] = [CH_3COOH] = 1.5 \ mol/L$ $K_a = 1.8 	imes 10^{-5}$ $pK_a = -\log(1.8 	imes 10^{-5}) = 5 - \log(1.8) = 5 - 0.255 = 4.745$ Now,substitute the values into the equation: $pH = 4.745 + \log(\frac{0.2}{1.5})$ $pH = 4.745 + \log(0.1333)$ $pH = 4.745 - 0.875 = 3.87$ Rounding to the nearest provided option,the answer is $3.86$.

The $pH$ of a buffer solution containing $0.2 \ mol/L$ $CH_3COONa$ and $1.5 \ mol/L$ $CH_3COOH$ is ($K_a$ for acetic acid is $1.8 \times 10^{-5}$).

Similar Questions

Which of the following is a buffer solution?

An acidic buffer solution is prepared by mixing a proportionate quantity of

$A$ solution is prepared by mixing $0.01 \ mol$ each of $H_2CO_3$,$NaHCO_3$,$Na_2CO_3$,and $NaOH$ in $100 \ mL$ of water. The $pH$ of the resulting solution is. . . . . . .
[Given : $pK_{a1}$ and $pK_{a2}$ of $H_2CO_3$ are $6.37$ and $10.32$,respectively; $\log 2=0.30$ ]

$2 \ g$ acetic acid and $3 \ g$ sodium acetate are present in $100 \ mL$ aqueous solution. What will be the $pH$ of the solution if the ionisation constant of acetic acid is $1.8 \times 10^{-5}$?

The buffer system which helps to maintain the $pH$ of blood between $7.26$ to $7.42$ is:

Vedclass Test Series

Exam Paper Generator

Online Exam Module