Problem: Consider the following reaction: HF(aq) + CN-(aq) ⇌ HCN(aq) + F-(aq) a. Identify the acid-base conjugate pairs.   Given the Ka values below HCN(aq) ⇌ H+(aq) + CN-(aq)    Ka= 6.2x 10-16 HF(aq) ⇌ H+(aq) + F-(aq)          Ka= 6.6x 10-4 Is HF or HCN the strongest acid? Why? If I have 1M HCN in a flask A and 1M of HF in flask B, which solution will conduct more electricity? Why? Will equilibrium at the start of this question favor the formation of reactants (left side) or product (right side)? What is the value for K for the equilibrium at the start of this question (looking for number)?  

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Problem Details

Consider the following reaction:
HF(aq) + CN-(aq) ⇌ HCN(aq) + F-(aq)

a. Identify the acid-base conjugate pairs.

Given the Ka values below
HCN(aq) ⇌ H+(aq) + CN-(aq)    Ka= 6.2x 10-16
HF(aq) ⇌ H+(aq) + F-(aq)          Ka= 6.6x 10-4

Is HF or HCN the strongest acid? Why?


If I have 1M HCN in a flask A and 1M of HF in flask B, which solution will conduct more electricity? Why?


Will equilibrium at the start of this question favor the formation of reactants (left side) or product (right side)?


What is the value for K for the equilibrium at the start of this question (looking for number)?

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Based on our data, we think this problem is relevant for Professor Stenson's class at USOUTHAL.