For a solution equimolar in HCN and NaCN,which statement is false? September 21, 2022 by 8i9x6 This is an example of the common ion effect. The [HS1U1P1+S1S1P0] is larger than it would be if only the HCN was in solution. The [HS1U1P1+S1S1P0] is equal to the KS1U1B1aS1U1B0. Addition of more NaCN will shift the acid dissociation equilibrium of HCN to the left. Addition of NaOH will increase [CNS1U1P1-S1S1P0] and decrease [HCN]. See Answer The [HS1U1P1+S1S1P0] is larger than it would be if only the HCN was in solution.