A solution of formic acid is half-neutralized | vedclass

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

Question

(A) The reaction is: $HCOOH + KOH \rightarrow HCOOK + H_2O$. Since the acid is half-neutralized,the concentration of the salt $[HCOOK]$ is equal to th

Vedclass · Accepted Answer

$3.6990$

Vedclass · Answer

(A) The reaction is: $HCOOH + KOH ightarrow HCOOK + H_2O$. Since the acid is half-neutralized,the concentration of the salt $[HCOOK]$ is equal to the concentration of the remaining acid $[HCOOH]$. Using the Henderson-Hasselbalch equation for an acidic buffer: $pH = pK_a + \log \frac{[Salt]}{[Acid]}$. Given $K_a = 2 	imes 10^{-4}$,so $pK_a = -\log(2 	imes 10^{-4}) = 4 - \log 2 = 4 - 0.3010 = 3.6990$. Since $[Salt] = [Acid]$,the ratio $\frac{[Salt]}{[Acid]} = 1$. Therefore,$pH = 3.6990 + \log(1) = 3.6990 + 0 = 3.6990$.

$A$ solution of formic acid is half-neutralized by the addition of a $KOH$ solution. If $K_a (HCOOH) = 2 \times 10^{-4}$,what is the $pH$ of the solution? (Given: $\log 2 = 0.3010$)

Similar Questions

$0.1 \ M, 60 \ mL$ $NH_4Cl$ $(K_h = 10^{-9})$ is titrated against $0.2 \ M$ $NaOH$. What is the $pH$ at the $\frac{1}{3}$ equivalence point?

At a constant temperature,the $pK_b$ of $NH_4OH$ is $4.74$. What is the $pH$ of a basic buffer containing equimolar concentrations of $NH_4OH$ and $NH_4Cl$?

The $pH$ of an aqueous solution containing $1 \ M$ benzoic acid $(pK_{a}=4.20)$ and $1 \ M$ sodium benzoate is $4.5$. The volume of benzoic acid solution in $300 \ mL$ of this buffer solution is . . . . . . $mL$.

What is the $pH$ of $10 \ L$ of a buffer solution containing $0.01 \ M \ NH_4Cl$ and $0.1 \ M \ NH_4OH$ having $pK_b$ of $5$?

Which of the following is a buffer solution?

Vedclass Test Series

Exam Paper Generator

Online Exam Module