0.1 M NaOH is titrated with 0.1 M HA till the end point; Ka for HA is 5.6×10−6 and degree of hydrolysis is less compared to 1 . Calculate pH of the resulting solution at the end point.

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Class 11

Chemistry

Equilibrium

The acid base titration using indicators

0.1 {~M~} {NaOH} is titrated with 0.1 {~M~} {H} A till the end

Question

Hard

Solving time: 5 mins

$0.1 M NaOH$ is titrated with $0.1 M H A$ till the end point; $K_{a}$ for $H A$ is $5.6 \times 1 0^{- 6}$ and degree of hydrolysis is less compared to 1 . Calculate $pH$ of the resulting solution at the end point.

8.0

8.5

9.5

9.0

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0.1 M NaOH

is titrated with

0.1 M H A

till the end point;

K_{a}

for

H A

5.6 \times 1 0^{- 6}

and degree of hydrolysis is less compared to 1 . Calculate

pH

of the resulting solution at the end point.

5 mins ago

Discuss this question LIVE

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Text solutionVerified

H A + NaOH ⟶ Na A + H_{2} O

At the end point, the solution contains only

N a A

whose concentration is

0.1/2 = 0.05

M
Since, the salt

Na A

is formed by strong alkali

(NaOH)

and weak acid

H A

(indicated by its low

K_{a}

value), its

pH

can be evaluated by the following relation.

pH = \frac{1}{2} (p K_{w} + p K_{a} + lo g C) = \frac{1}{2} [14 + 5.3010 + (- 1.3010)] = 9

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Question Text	$0.1 M NaOH$ is titrated with $0.1 M H A$ till the end point; $K_{a}$ for $H A$ is $5.6 \times 1 0^{- 6}$ and degree of hydrolysis is less compared to 1 . Calculate $pH$ of the resulting solution at the end point.
Topic	Equilibrium
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1
Upvotes	90

$0.1 M NaOH$ is titrated with $0.1 M H A$ till the end point; $K_{a}$ for $H A$ is $5.6 \times 1 0^{- 6}$ and degree of hydrolysis is less compared to 1 . Calculate $pH$ of the resulting solution at the end point.

Text solutionVerified

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0.1 M NaOH is titrated with 0.1 M HA till the end point; Ka​ for HA is 5.6×10−6 and degree of hydrolysis is less compared to 1 . Calculate pH of the resulting solution at the end point.

Text solutionVerified

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$0.1 M NaOH$ is titrated with $0.1 M H A$ till the end point; $K_{a}$ for $H A$ is $5.6 \times 1 0^{- 6}$ and degree of hydrolysis is less compared to 1 . Calculate $pH$ of the resulting solution at the end point.