KOH + CH3COOH = H2O + CH3COOK

KOH (potassium hydroxide) + CH_3CO_2H (acetic acid) ⟶ H_2O (water) + CH_3COOK (potassium acetate)

Balance the chemical equation algebraically: KOH + CH_3CO_2H ⟶ H_2O + CH_3COOK Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 CH_3CO_2H ⟶ c_3 H_2O + c_4 CH_3COOK Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O and C: H: | c_1 + 4 c_2 = 2 c_3 + 3 c_4 K: | c_1 = c_4 O: | c_1 + 2 c_2 = c_3 + 2 c_4 C: | 2 c_2 = 2 c_4 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | KOH + CH_3CO_2H ⟶ H_2O + CH_3COOK

+ ⟶ +

potassium hydroxide + acetic acid ⟶ water + potassium acetate

Construct the equilibrium constant, K, expression for: KOH + CH_3CO_2H ⟶ H_2O + CH_3COOK Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: KOH + CH_3CO_2H ⟶ H_2O + CH_3COOK Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i KOH | 1 | -1 CH_3CO_2H | 1 | -1 H_2O | 1 | 1 CH_3COOK | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 1 | -1 | ([KOH])^(-1) CH_3CO_2H | 1 | -1 | ([CH3CO2H])^(-1) H_2O | 1 | 1 | [H2O] CH_3COOK | 1 | 1 | [CH3COOK] The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([KOH])^(-1) ([CH3CO2H])^(-1) [H2O] [CH3COOK] = ([H2O] [CH3COOK])/([KOH] [CH3CO2H])

Construct the rate of reaction expression for: KOH + CH_3CO_2H ⟶ H_2O + CH_3COOK Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: KOH + CH_3CO_2H ⟶ H_2O + CH_3COOK Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i KOH | 1 | -1 CH_3CO_2H | 1 | -1 H_2O | 1 | 1 CH_3COOK | 1 | 1 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term KOH | 1 | -1 | -(Δ[KOH])/(Δt) CH_3CO_2H | 1 | -1 | -(Δ[CH3CO2H])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) CH_3COOK | 1 | 1 | (Δ[CH3COOK])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -(Δ[KOH])/(Δt) = -(Δ[CH3CO2H])/(Δt) = (Δ[H2O])/(Δt) = (Δ[CH3COOK])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| potassium hydroxide | acetic acid | water | potassium acetate formula | KOH | CH_3CO_2H | H_2O | CH_3COOK Hill formula | HKO | C_2H_4O_2 | H_2O | C_2H_3KO_2 name | potassium hydroxide | acetic acid | water | potassium acetate