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  4. Ammonium acetate which is 0.01 M , is hydrolysed to 0.001 M concentration. Calculate the change in pH in 0.001 M solution, if initially pH = pKa

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Q. Ammonium acetate which is $ 0.01 \,M $ , is hydrolysed to $ 0.001\, M $ concentration. Calculate the change in $ pH $ in $ 0.001\, M $ solution, if initially $ pH = pK_a $

MHT CETMHT CET 2010Equilibrium

Solution:

$\underset{0.01 \,M}{CH_3COONH_4} + H_2O \rightarrow \underset{0.001\,M}{CH_3COOH} + NH_4OH$

$pH = p K_{a}+\log \frac{\left[ CH _{3} COONH _{4}\right]}{\left[ CH _{3} COOH \right]} $

$= p K_{a}+\log \left[\frac{0.01}{0.001}\right]$

$= p K_{a}+\log 10 $

$= p K_{a}+1$

$\therefore $ Change in $pH =1$