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The ionization constant of chloroacetic ...

The ionization constant of chloroacetic acid is `1.35 × 10^(-3)`. What will be the pH of 0.1M acid and its 0.1M sodium salt solution?

Text Solution

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`CH_(2)ClCOOH + H_(2)O to CH_(2)ClCOO^(-) + H_(3)O^(+), K_(a)=1.35 O^(-3)`
(a) `pK_(a)=-logK_(a)=-log[1.35xx10^(-3)]=2.87`
By Oswald’s dilution law :`[H_(3)O^(+)]=sqrt(K_(a).C) = sqrt(1.35xx10^(-3)xx0.1)=1.16xx10^(-2)M`
pH acid = `– log[H_(3)O^(+)] = – log (1.6xx10^(-2))M=1.94`
(b) A `0.1M CH_(2)ClCOONa)` aqueous solution (sodium chloro-acetate) is basic due to hydrolysis.
`CH_(2)ClCOO^(-) + H_(2)O to CH_(2)ClCOOH + OH^(-)`
Using standard result for pH of a salt of strong base and weak acid:`pH=7 + (pK_(a) + logC)/2= (2.87+log0.1)/2= 7.94`
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