Question

In a (rather dangerous) reaction, a 0.175M (aq) soln. of KCN is being titrated with a 0.250M soln. of (aq) HCL.

a) Write the balanced net ionic rxn. that occurs during this titration.

The answer is: CN^- (aq) + H3O^+(aq) => HCN(aq) + H2O(l)

Can someone explain to me why this is step by step. Really confused.

And

b) calculate the pH of the 0.175M (aq) soln. of KCN before the titration begins.

Also why is the equation for the ICE table: CN^-(aq) +H2O(l) =>HCN (aq)+H2O(l)

And how to solve this problem too. This is the last question on hw and I am completely confused. Please help. Thanks.

Answer 1