Balance the following equations and write the corresponding ionic and net ionic equations (if appropriate). (a) \( \mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{KOH}(a q) \longrightarrow \) (b) \( \mathrm{H}_{2} \mathrm{CO}_{3}(a q)+\mathrm{NaOH}(a q) \longrightarrow \) (c) \( \mathrm{HNO}_{3}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \longrightarrow \)

Below are the balanced molecular equations along with their complete (total) ionic and net ionic equations. ────────────────────────────── (a) Reaction: CH₃COOH (aq) + KOH (aq) → CH₃COOK (aq) + H₂O (l) • Molecular Equation:   CH₃COOH (aq) + KOH (aq) → CH₃COOK (aq) + H₂O (l) • Complete Ionic Equation:   CH₃COOH (aq) + K⁺ (aq) + OH⁻ (aq) → CH₃COO⁻ (aq) + K⁺ (aq) + H₂O (l)   (Note: Acetic acid is a weak acid and remains in its molecular form.) • Net Ionic Equation:   CH₃COOH (aq) + OH⁻ (aq) → CH₃COO⁻ (aq) + H₂O (l)   (Canceled spectator ion: K⁺) ────────────────────────────── (b) Reaction: H₂CO₃ (aq) + NaOH (aq) → NaHCO₃ (aq) + H₂O (l) • Molecular Equation:   H₂CO₃ (aq) + NaOH (aq) → NaHCO₃ (aq) + H₂O (l)   (This represents the neutralization of one acidic proton; carbonic acid is diprotic, so further neutralization is possible.) • Complete Ionic Equation:   H₂CO₃ (aq) + Na⁺ (aq) + OH⁻ (aq) → Na⁺ (aq) + HCO₃⁻ (aq) + H₂O (l)   (Again, H₂CO₃ is a weak acid and is not dissociated.) • Net Ionic Equation:   H₂CO₃ (aq) + OH⁻ (aq) → HCO₃⁻ (aq) + H₂O (l)   (Canceled spectator ion: Na⁺) ────────────────────────────── (c) Reaction: HNO₃ (aq) + Ba(OH)₂ (aq) → Ba(NO₃)₂ (aq) + H₂O (l) Since barium hydroxide gives 2 OH⁻ per formula unit, two moles of nitric acid are required. • Molecular Equation:   2 HNO₃ (aq) + Ba(OH)₂ (aq) → Ba(NO₃)₂ (aq) + 2 H₂O (l) • Complete Ionic Equation:   2 H⁺ (aq) + 2 NO₃⁻ (aq) + Ba²⁺ (aq) + 2 OH⁻ (aq) →    Ba²⁺ (aq) + 2 NO₃⁻ (aq) + 2 H₂O (l)   (HNO₃ and Ba(OH)₂ are strong electrolytes and are fully dissociated.) • Net Ionic Equation:   2 H⁺ (aq) + 2 OH⁻ (aq) → 2 H₂O (l)   (Spectator ions Ba²⁺ and NO₃⁻ are canceled.)   This can also be written in its simplest form as:    H⁺ (aq) + OH⁻ (aq) → H₂O (l)   if one recognizes that the equation is the basic acid–base neutralization process. ────────────────────────────── These are the balanced equations with their corresponding ionic and net ionic forms.