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

Byju's Answer

Standard XII

Chemistry

Solubility Product

Calculate pH ...

Question

Calculate pH of an aqueous solution of 1M $H C O O N H_{4}$ assuming complete dissociation.
$p K_{a} (H C O O H) = 3.8 a n d p K_{b} = 4.8$

7.5

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

6.4

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

6.5

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

5.5

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

Open in App

Solution

The correct option is C 6.5
$p H = 7 + \frac{p K_{a}}{2} - \frac{p K_{b}}{2}$
$p H = 7 + \frac{1}{2} \times 3.8 - \frac{1}{2} \times 4.8$
$= 7 + 1.9 - 2.4 = 6.5. p H = 6.5$

Suggest Corrections

Similar questions

Calculate the pH of an aqueous solution of $1.0 M$ ammonium formate assuming complete dissociation. ( $p_{K a}$ of formic acid = 3.8 and $p_{K b}$ of ammonia = 4.8)

Q. Calculate the pH of an aqueous solution of

1 M

ammonium formate, assuming complete dissociation.

(p K_{a} = 3.8, p K_{b} = 4.8)

Q. Calculate

p H

1.0 M P O_{4}^{3 -}

in aqueous solution. Given

p K_{b} o f P O_{4}^{3 -} = 1.62

Q. What will be the

p H

of an aqueous solution of

0.1 M

ammonium formate

25^{o} C

Given : p K_{a} (H C O O H) = 3.8 a n d p K_{b} (N H_{4} O H) = 4.8

Q. What will be the

p H

of an aqueous solution of

1.0 M

ammonium formate?

Given:

p K_{a} = 3.8

and

p K_{b} = 4.8

Join BYJU'S Learning Program

Calculate pH of an aqueous solution of 1M HCOONH4 assuming complete dissociation. pKa(HCOOH)=3.8 and pKb=4.8

The correct option is C 6.5pH=7+pKa2−pKb2 pH=7+12×3.8−12×4.8 =7+1.9−2.4=6.5. pH=6.5

Calculate pH of an aqueous solution of 1M $H C O O N H_{4}$ assuming complete dissociation.
$p K_{a} (H C O O H) = 3.8 a n d p K_{b} = 4.8$

The correct option is C 6.5
$p H = 7 + \frac{p K_{a}}{2} - \frac{p K_{b}}{2}$
$p H = 7 + \frac{1}{2} \times 3.8 - \frac{1}{2} \times 4.8$
$= 7 + 1.9 - 2.4 = 6.5. p H = 6.5$