H2SO4 + KOH = H2O + KHSO4

H_2SO_4 sulfuric acid + KOH potassium hydroxide ⟶ H_2O water + KHSO_4 potassium bisulfate

Balance the chemical equation algebraically: H_2SO_4 + KOH ⟶ H_2O + KHSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 KOH ⟶ c_3 H_2O + c_4 KHSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S and K: H: | 2 c_1 + c_2 = 2 c_3 + c_4 O: | 4 c_1 + c_2 = c_3 + 4 c_4 S: | c_1 = c_4 K: | c_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: | | H_2SO_4 + KOH ⟶ H_2O + KHSO_4

+ ⟶ +

sulfuric acid + potassium hydroxide ⟶ water + potassium bisulfate

| sulfuric acid | potassium hydroxide | water | potassium bisulfate molecular enthalpy | -814 kJ/mol | -424.6 kJ/mol | -285.8 kJ/mol | -1161 kJ/mol total enthalpy | -814 kJ/mol | -424.6 kJ/mol | -285.8 kJ/mol | -1161 kJ/mol | H_initial = -1239 kJ/mol | | H_final = -1446 kJ/mol | ΔH_rxn^0 | -1446 kJ/mol - -1239 kJ/mol = -207.8 kJ/mol (exothermic) | | |

| sulfuric acid | potassium hydroxide | water | potassium bisulfate molecular free energy | -690 kJ/mol | -379.4 kJ/mol | -237.1 kJ/mol | -1031 kJ/mol total free energy | -690 kJ/mol | -379.4 kJ/mol | -237.1 kJ/mol | -1031 kJ/mol | G_initial = -1069 kJ/mol | | G_final = -1268 kJ/mol | ΔG_rxn^0 | -1268 kJ/mol - -1069 kJ/mol = -199 kJ/mol (exergonic) | | |

Construct the equilibrium constant, K, expression for: H_2SO_4 + KOH ⟶ H_2O + KHSO_4 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: H_2SO_4 + KOH ⟶ H_2O + KHSO_4 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 H_2SO_4 | 1 | -1 KOH | 1 | -1 H_2O | 1 | 1 KHSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) KOH | 1 | -1 | ([KOH])^(-1) H_2O | 1 | 1 | [H2O] KHSO_4 | 1 | 1 | [KHSO4] 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 = ([H2SO4])^(-1) ([KOH])^(-1) [H2O] [KHSO4] = ([H2O] [KHSO4])/([H2SO4] [KOH])

Construct the rate of reaction expression for: H_2SO_4 + KOH ⟶ H_2O + KHSO_4 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: H_2SO_4 + KOH ⟶ H_2O + KHSO_4 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 H_2SO_4 | 1 | -1 KOH | 1 | -1 H_2O | 1 | 1 KHSO_4 | 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 H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) KOH | 1 | -1 | -(Δ[KOH])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) KHSO_4 | 1 | 1 | (Δ[KHSO4])/(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[H2SO4])/(Δt) = -(Δ[KOH])/(Δt) = (Δ[H2O])/(Δt) = (Δ[KHSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sulfuric acid | potassium hydroxide | water | potassium bisulfate formula | H_2SO_4 | KOH | H_2O | KHSO_4 Hill formula | H_2O_4S | HKO | H_2O | HKO_4S name | sulfuric acid | potassium hydroxide | water | potassium bisulfate IUPAC name | sulfuric acid | potassium hydroxide | water | potassium hydrogen sulfate

| sulfuric acid | potassium hydroxide | water | potassium bisulfate molar mass | 98.07 g/mol | 56.105 g/mol | 18.015 g/mol | 136.16 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | 10.371 °C | 406 °C | 0 °C | 214 °C boiling point | 279.6 °C | 1327 °C | 99.9839 °C | density | 1.8305 g/cm^3 | 2.044 g/cm^3 | 1 g/cm^3 | 2.32 g/cm^3 solubility in water | very soluble | soluble | | surface tension | 0.0735 N/m | | 0.0728 N/m | dynamic viscosity | 0.021 Pa s (at 25 °C) | 0.001 Pa s (at 550 °C) | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless |