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The ionization constant of nitrous acid ...

The ionization constant of nitrous acid is `4.5 xx 10^(-4)`. Calculate the pH of 0.04 M sodium nitrite solution and also its degree of hydrolysis.

Text Solution

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Given: `[NaNO_(2)]=0.04M , K_(a) of HNO_(2)=4.5xx10^(-4)`
Note that `NaNO_(2)` is a salt of strong base, NaOH and weak acid, `HNO_(2)`.
Using standard result for the pH of a solution of salt of Strong base and Weak acid:
`pH=7 + (pK_(a) + logC)/2`
`pK_(a)=4-0.6532=3.3468 approx 3.35 implies pH=7 + (3.35+log0.04)/2 =7.98`
Degree of hydrolysis,`h=sqrt(K_(w)/(K_(a)C))=sqrt(10^(-4)/(4.5xx10^(-4)xx0.04))implies h = 2.36xx10^(-5)`
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