Acetic acid has a pk*of 2 x 10-s m at 25"c approximatety. approximately what fraction of a 0 .l m solution of acetic acid wilt be dissociated
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[A-] is the concentration of anions or salt i.e. dissociated form. [HA] is the concentration of the acid.
According to Henderson- Hasselbalch equation,
This means log( [A-]/[HA]) = 2
so, [A-]/[HA] = 10^2 = 100
[A-] = 100 * [HA]
The dissociated form is 100 times more than the associated form.
Therefore, percentage dissociated=
([A-]/([A-]+[HA]))*100%
= (100[HA]/(100[HA]+[HA]))*100%
=(100/101) *100%
=99.009%
According to Henderson- Hasselbalch equation,
This means log( [A-]/[HA]) = 2
so, [A-]/[HA] = 10^2 = 100
[A-] = 100 * [HA]
The dissociated form is 100 times more than the associated form.
Therefore, percentage dissociated=
([A-]/([A-]+[HA]))*100%
= (100[HA]/(100[HA]+[HA]))*100%
=(100/101) *100%
=99.009%
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