Question

Ph of 0.1 m solution of nh4cn solution is x. If its concentration is increased to 0.2 m then ph of the solution will be

Answer 1

Calculate the pH of a 0.7M solution of NH4CN. KbNH3=1.79*10-5, KaHCN=7.9*10-10.

The reactions are:

NH4++H2O ::equil:: NH3+H3O+ Ka=Kh=Kw/Kb=5.59*10-10

0.7 x x

CN-+H2O ::equil:: HCN+OH- Kb=Kw/Ka=1.27*10-5

0.7 y y

[H+]=x=1.98*10-5

[OH-]=y=2.98*10-3

There are more OH- ions :rarrow: y-x≈2.98*10-3

pOH=2.52

pH=14-2.52=11.48 but in my book it is 9.18.

Answer 2

Answer:

Will remain same....-x

Explanation:

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