Question

The ph of neutralization point of point 1 normal ammonium hydroxide with point 1 normal hcl is

Answer 1

Answer:

A solution of a strong acid and a weak base gives rise to cationic hydrolysis.

In this particular reaction, NH4OH + HCl →NH4Cl + H2O

NH4Cl  is formed, which undergoes cationic hydrolysis.

The pH of the solution undergoing cationic hydrolysis can be calculated by :

pH=12(pKw−pKb−log C)

where Kb= Dissociation constant of base.

C= Concentration.

Kw= Ionisation constant of water.

Taking, Kw= 10−14

Kb= 1.8 ×10−5

C =0.1

pH =12(−log(10−14)−(−log(1.8×10−5))−(log(0.1)))

= 12(14−4.74+1)

=12(10.26)

=5.13