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Byju's Answer

Standard XII

Chemistry

Salt of Weak Acid and Strong Base

In the titrat...

Question

In the titration of a solution of a weak acid $H A$ and $N a O H$ , the $p H$ is $5.0$ after $10 m L$ of $N a O H$ solution has been added and $5.60$ after $20 m L N a O H$ has been added.
What is the value of $p K_{a}$ for $H A$ ?

5.15

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5.3

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5.6

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None of these

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Solution

The correct option is B $5.3$
$p H = p K_{a} + l o g [s a l t] / [b a s e]$
$5 = p K_{a} + l o g x$
$5.6 = p K_{a} + l o g (1 / x)$
$p K_{a} = (5 + 5.6) / 2 = 5.3.$

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Similar questions

Q. In the titration of a solution of a weak acid

H X

with

N a O H

, the

p H

5.8

after

10.0 m L

N a O H

solution has been added and

6.402

after

20.0 m L

N a O H

has been added. What is the ionization constant of

H X

Q. A solution of weak acid

H A

was titrated with base

N a O H

. The equivalence point was reached when

36.12 m L

0.1 M

N a O H

has been added. Now

18.06 m L

0.1 M

H C l

were added to titrated solution, the

p H

was found to be

4.92

. What will be the

p H

of the solution obtained by mixing

10 m L

0.2 M

N a O H

and

10 m L

0.2 M

H A

Q. The equivalent point in a titration of

40.0 m L

of a solution of a weak monoprotic acid occurs when

35.0 m L

of a

0.10 M

N a O H

solution has been added. The pH of the solution is

5.75

after the addition of

20.0 m L

N a O H

solution. What is the dissociation constant of the acid?

100

mL of

0.02 M

benzoic acid

(p K_{a} = 4.2)

is titrated using

0.02 M N a O H

. The pH after

50

mL of

N a O H

has been added is:

Q. A

30 m L

solution of

0.2 M C H_{3} C O O H

is titrated with

0.2 M N a O H

. Find the

p H

of the solution when

10 m L

N a O H

has been added.
Given

p K_{a} (C H_{3} C O O H) = 4.74

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In the titration of a solution of a weak acid HA and NaOH, the pH is 5.0 after 10 mL of NaOH solution has been added and 5.60 after 20 mL NaOH has been added.What is the value of pKa for HA?

The correct option is B 5.3pH=pKa+log[salt]/[base]5=pKa+logx5.6=pKa+log(1/x)pKa=(5+5.6)/2=5.3.

In the titration of a solution of a weak acid $H A$ and $N a O H$ , the $p H$ is $5.0$ after $10 m L$ of $N a O H$ solution has been added and $5.60$ after $20 m L N a O H$ has been added.
What is the value of $p K_{a}$ for $H A$ ?

The correct option is B $5.3$
$p H = p K_{a} + l o g [s a l t] / [b a s e]$
$5 = p K_{a} + l o g x$
$5.6 = p K_{a} + l o g (1 / x)$
$p K_{a} = (5 + 5.6) / 2 = 5.3.$