You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Salt of Strong Acid and Weak Base

A 25.0 mL s...

Question

A $25.0 m L$ sample of $0.10 M H C l$ is titrated with $0.10 M N a O H$ . What is the $p H$ of the solution at the points where $24.9$ and $25.1 m L$ of $N a O H$ have been added?

3.70, 10.70

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

3.30, 10.30

No worries! We‘ve got your back. Try BYJU‘S free classes today!

3.70, 10.30

No worries! We‘ve got your back. Try BYJU‘S free classes today!

3.0, 11.0

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A $3.70, 10.70$
Molarity is 0.1M so its each ml contains $10^{- 4}$ moles of ions. At 24.9 ml, hydrogen ion is excess so pH is $3.7$ and at 25.1 ml, hydroxide ion are in excess so pH is $10.7$

Suggest Corrections

Similar questions

Q. A weak acid

(50.0 m L)

was titrated with

0.1 M

N a O H

. The

p H

values when

10.0 m L

and

25.0 m L

of base have been added are found to be

4.16

and

4.76

respectively. Calculate

K_{a}

of the acid and

p H

at the equivalence point.

Q. A solution of weak acid 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

have 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 is

K_{a}

of acid?

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

p H

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?

A 25.0 ml sample of 0.105 M $H C l$ was titrated with 315 ml of $N a O H$ . What is the concentration of the $N a O H$ ?

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

Join BYJU'S Learning Program

A 25.0 mL sample of 0.10 M HCl is titrated with 0.10 M NaOH. What is the pH of the solution at the points where 24.9 and 25.1 mL of NaOH have been added?

The correct option is A 3.70, 10.70Molarity is 0.1M so its each ml contains 10−4 moles of ions. At 24.9 ml, hydrogen ion is excess so pH is 3.7 and at 25.1 ml, hydroxide ion are in excess so pH is 10.7

A $25.0 m L$ sample of $0.10 M H C l$ is titrated with $0.10 M N a O H$ . What is the $p H$ of the solution at the points where $24.9$ and $25.1 m L$ of $N a O H$ have been added?

The correct option is A $3.70, 10.70$
Molarity is 0.1M so its each ml contains $10^{- 4}$ moles of ions. At 24.9 ml, hydrogen ion is excess so pH is $3.7$ and at 25.1 ml, hydroxide ion are in excess so pH is $10.7$