explain why pH = –log ɑH+ is a more accurate calculation than pH = –log [H+],...
explain why pH = –log ɑH+ is a more accurate calculation than pH = –log [H+], when dealing with non-dilute solutions
Homework Answers
In case of non dilute solution it is possible that all of the hydrogen ion is not dissociated and stay in associated form . In that case we have to multiply it's concentration from alpha(degree of dissociation) to get actual amount of ion which is contributing and is responsible for pH. So pH will be negative log of alpha multiplied H+ ion concentration .
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explain why pH = –log ɑH+ is a more accurate calculation than pH
= –log [H+],...
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pH= 4.75 + log (5/5)= 4.75 pH= 4.75 + log (1/5)= 4.05 pH= 4.75 + log...
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Consider the function pH = -log[H+], where [H+] is the molarity of H+. Find [H+] and...
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