pH of a mixture which is 0.1 M in CH_3COOH a | vedclass

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

Question

(A) The mixture contains a weak acid $(CH_3COOH)$ and its salt with a strong base,$(CH_3COO)_2Ba$,forming an acidic buffer.The Henderson-Hasselbalch e

Vedclass · Accepted Answer

$4.74$

Vedclass · Answer

(A) The mixture contains a weak acid $(CH_3COOH)$ and its salt with a strong base,$(CH_3COO)_2Ba$,forming an acidic buffer.The Henderson-Hasselbalch equation is: $pH = pK_a + \log \left( \frac{[Salt]}{[Acid]} ight)$.$(CH_3COO)_2Ba$ dissociates completely: $(CH_3COO)_2Ba ightarrow 2CH_3COO^- + Ba^{2+}$.Concentration of $[CH_3COO^-] = 2 	imes 0.05 \ M = 0.1 \ M$.Given $[CH_3COOH] = 0.1 \ M$.Substituting the values: $pH = 4.74 + \log \left( \frac{0.1}{0.1} ight)$.Since $\log(1) = 0$,$pH = 4.74 + 0 = 4.74$.

$pH$ of a mixture which is $0.1 \ M$ in $CH_3COOH$ and $0.05 \ M$ in $(CH_3COO)_2Ba$ is [$pK_a$ of $CH_3COOH$ = $4.74$]

Similar Questions

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

In which of the following does a buffer solution play an important role?

What is a buffer solution? Explain the types of buffer solutions with examples and state their biological importance.

To prepare a buffer solution of $pH = 6$ by mixing sodium acetate and acetic acid,what should be the ratio of the concentration of salt to acid? $(K_a = 10^{-5})$

$A$ weak acid with a dissociation constant of $10^{-5}$ is being titrated with an aqueous $NaOH$ solution. The $pH$ at the point of one-third neutralization of the acid will be:

Vedclass Test Series

Exam Paper Generator

Online Exam Module