CameraIcon

SearchIcon

MyQuestionIcon

1

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

Salt of Weak Acid and Strong Base

Calculate the...

Question

Calculate the pH of an aqueous solution of $1 M$ ammonium formate, assuming complete dissociation.
$(p K_{a} = 3.8, p K_{b} = 4.8)$

Open in App

Solution

Ammonium formate is a salt of weak acid and weak base.
So $p H = 7 + \frac{1}{2} (p K_{a} - {p K}_{b})$
$p H = 7 + \frac{1}{2} (3.8 - 4.8)$
$p H = 6.5$

Suggest Corrections

thumbs-up

0

Similar questions

Q. Calculate the pH of an aqueous solution of

1.0 M

ammonium formate assuming complete dissociation.

p K_{a}

for formic acid

= 3.8

p K_{b}

= 4.8

Q. What will be the

p H

of an aqueous solution of

1.0 M

ammonium formate?

p K_{a} = 3.8

p K_{b} = 4.8

Q. Find the pH of an aqueous solution of 1.0 M ammonium formate assuming complete dissociation.

({pK}_{a} {of formic acid = 3.8 and pK}_{b} of ammonium hydroxide = 4.8.)

Q. 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

Q. Determine the pH value of

0.1 M

aqueous solution of ammonium cyanide

(p K_{a} = 9.04, p K_{b} = 4.73)

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

Hydrolysis

CHEMISTRY

Watch in App

explore_more_icon

Explore more

Salt of Weak Acid and Strong Base

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon