For a solution equimolar in HCN and NaCN, which statement is false? A. [H+] is larger...

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.	Addition of NaOH will increase [CN^–] and decrease [HCN].
	C.	[H⁺] is equal to K_a.
	D.	This is an example of the common-ion effect.
	E.	Addition of more NaCN will shift the acid-dissociation equilibrium of HCN to the left.

Expert Solution

Answer is

[H⁺] is equal to K_a this statement is false

regarding common ion effect all other state ments are correct

Ka is the percentage of the dissociation of H+ which will depend on concentration of HCN whic was not equal to H+

queen_honey_blossom answered 2 years ago

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