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How much water must be added to `300 mL` of a `0.2M` solution of `CH_(3)COOH` for the degree of dissociation of the acid to double ? ( Assume `K_(a)` of acetic is of order of `10^(-5)M)`A. `900 ml`B. `300ml`C. `600 ml`D. `1200ml` |
Answer» Correct Answer - 1 Initially degree of dissociation `alpha=sqrt((K_(a))/(C))` Now degree of dissociation, `alpha_(1)=2alpha=sqrt((4K_(a))/(C))=sqrt((K_(a))/(C_(1)))` so `" "C_(1)=(C)/(4)" "rArr" "` Hence we have `300xx0.2rArrV_(1)xx(0.2)/(4)" "`so `V_(f)=1200ml` Hence water added `=1200-300=900ml` |
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