For a solution equimolar in HCN and NaCN, which statement is false? A. [H+] is larger than it would be if only the HCN were in solution. B. C. D. E. Addition of more NaCN will shift the acid-dissociation equilibrium of HCN to the left. Addition of NaOH will increase [CN*] and decrease [HCN]. [H+] is equal to Ka- This is an example of the common-ion effect.
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![For a solution equimolar in HCN and NaCN, which statement is false?
A. [H+] is larger than it would be if only the HCN were in solution.
B.
C.
D.
E.
Addition of more NaCN will shift the acid-dissociation equilibrium of HCN to the left.
Addition of NaOH will increase [CN] and decrease [HCN].
[H+] is equal to Ka.
This is an example of the common-ion effect.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb209d90c-1c14-40b1-bcc0-74d529362312%2Fb8ff2da6-47af-4b9e-b66e-736d16092ce3%2Fkisckwl_processed.jpeg&w=3840&q=75)
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