Question

Given the following information: hydrofluoric acid = HF hydrocyanic acid - HCN HF is a stronger acid than HCN (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.074 M aqueous hydrofluoric acid and sodium cyanide are mixed. It is not necessary to include states such as (aq) or ($). (2) Which is the stronger base. For CN? (3) At equilibrium the y will be favored.

Answer 1

Given that HF is stronger acid than HCN the reaction between HF and NaCN is HF (aq) + NaCN (aq) ----------> HCN (aq) + NaF (aq) The net ionic equation is HF (aq) + CN- (aq) ----------> HCN (aq) + F(aq) Since HF is a stronger acid than HCN, it donates proton to CN-. So, According to Bronsted-Lowry theory, stronger the acid, weaker is its conjugate base. weaker the acid, stronger is its conjugate base. Since HF is a strong acid, F- will be weak conjugate base HCN is a weak acid, CN- will be stronger conjugate base. (b) CN is a strong base. Since HF is a stronger acid than HCN. That is HF donates proton more easier than HCN HF donates proton to CN-to form HCN and F- Hence (c) At equilibrium, PRODUCTS (FORWARD REACTION) will be favored.