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:

Step1: Analyze the reactants

\(C_5H_5NHCl\) is a salt of a weak base (\(C_5H_5N\)) and a strong acid (\(HCl\)). In solution, \(C_5H_5NHCl\) dissociates into \(C_5H_5NH^+\) and \(Cl^-\). \(CsOH\) is a strong base and dissociates completely into \(Cs^+\) and \(OH^-\).

Step2: Write the neutralization reaction

The \(OH^-\) from \(CsOH\) reacts with the \(C_5H_5NH^+\) (the acidic species from the salt). The \(Cl^-\) and \(Cs^+\) are spectator ions (they do not participate in the reaction).
The reaction is \(C_5H_5NH^+(aq)+OH^-(aq)
ightleftharpoons C_5H_5N(aq) + H_2O(l)\)

Answer:

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