O Calculate the pH of 500 ml of buffer solution containing .2M of ammonium sulphate and 0.3M ammonium hydroxide which 5 2.1% ionized in dilute solution. (kb of ammonium hydroxide is 1.8×10^-5) ​

Answer

Correct option is

A

9

pK

b

=−logK

b

=−log10

−5

=5

A mixture of ammonium hydroxide and ammonium chloride forms basic buffer solution.

The Hendrson's equation for he basic buffer solution is as given below.

pOH=pK

b

+log

[acid]

[salt]

Substitute values in the above expression.

pOH=5+log

0.1

0.1

=5

Hence, the pH of the solution is pH=14−pOH=14−5=9

Explanation:

hope it help brainliest pls

the correct answer is option d

explanation:

i was wrong its d because they dont use cm when calculating square roots