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Henderson Hassleback Equation

What will be ...

Question

What will be the $p H$ and $% α$ (degree of hydrolysis) respectively for the salt $B A$ of $0.1 M$ concentration? Given: $K_{a}$ for $H A = 10^{- 6}$ and $K_{b}$ for $B O H = 10^{- 6}$

A

5, 1%

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B

7, 10%

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C

9, 0.01%

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D

7, 0.01%

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Solution

The correct option is B $7, 10%$

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Similar questions

Q. What will be the

p H

% α

(degree of hydrolysis) respectively for the salt of weak acid and weak base

(B A)

0.1 M

concentration?
Given :

K_{a}

H A = 10^{- 6}

K_{b}

B O H = 10^{- 6}

Q. Calculate the hydrolysis constant of a salt of weak acid

(K_{a} = 2 \times 10^{- 6})

(K_{b} = 5 \times 10^{- 7})

.

0.1 M

N a O H

is titrated with

0.1 M

H A

till the end point;

K_{a}

H A

5.6 \times 10^{- 6}

and degree of hydrolysis is less compared to

1

. Calculate pH of the resulting solution at the end point.

Q. The degree of hydrolysis of

0.15 M

solution of ammonium acetate is:

K_{a}

{C H}_{3} C O O H

1.8 \times 10^{- 5}

K_{b}

{N H}_{3}

1.8 \times 10^{- 9}

The degree of hydrolysis and pH of $0.1 M$ sodium acetate solution are: Also calculate the concentration of all the ions at equilibrium. Hydrolysis constant of sodium acetate is $5.6 \times 10^{- 10}$ .

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