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OpenStudy (anonymous):
How would I find the pH of 0.25 M carbonic acid? also the pH for 0.075 M CN^-?
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OpenStudy (aaronq):
you would use the dissociation constants \(K_A\) and \(K_B\) and find the concentrations for the respective species that contribute to the pH.
OpenStudy (onepieceftw):
pH=-log_10 [H3O+]
OpenStudy (onepieceftw):
Substitute H3O+ for your molarity value.
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