Question

consider the reaction of a 20.0 ml of 0.220 m c₅h₅nhcl (ka = 5.9 x 10⁻⁶) with 12.0 ml of 0.241 m csoh.
write the net ionic equation for the reaction that takes place. be sure to include the proper phases for all species within the reaction.

Explanation:

• First, identify the acid - base reaction. \(C_5H_5NHCl\) is a salt of a weak base \(C_5H_5N\) (pyridine) and a strong acid \(HCl\). In aqueous solution, \(C_5H_5NHCl\) dissociates into \(C_5H_5NH^{+}\) (the conjugate acid of \(C_5H_5N\)) and \(Cl^{-}\). \(CsOH\) is a strong base and dissociates completely into \(Cs^{+}\) and \(OH^{-}\) in aqueous solution.
• The net ionic equation for an acid - base reaction involves the reaction of the acidic species and the basic species. Here, \(C_5H_5NH^{+}\) (acidic species) reacts with \(OH^{-}\) (basic species).
• \(Cl^{-}\) and \(Cs^{+}\) are spectator ions (they do not participate in the actual chemical reaction) and are excluded from the net ionic equation.

Answer:

\(C_5H_5NH^{+}(aq)+OH^{-}(aq)
ightleftharpoons C_5H_5N(aq) + H_2O(l)\)