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…

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.\nwrite the net ionic equation for the reaction that takes place. be sure to include the proper phases for all species within the reaction.

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.\nwrite the net ionic equation for the reaction that takes place. be sure to include the proper phases for all species within the reaction.

Answer

Brief Explanations:

  • 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)\rightleftharpoons C_5H_5N(aq) + H_2O(l))