HCl + Al(OH)3 = H2O + AlOHCl2

HCl hydrogen chloride + Al(OH)_3 aluminum hydroxide ⟶ H_2O water + AlOHCl2

Balance the chemical equation algebraically: HCl + Al(OH)_3 ⟶ H_2O + AlOHCl2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Al(OH)_3 ⟶ c_3 H_2O + c_4 AlOHCl2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Al and O: Cl: | c_1 = 2 c_4 H: | c_1 + 3 c_2 = 2 c_3 + c_4 Al: | c_2 = c_4 O: | 3 c_2 = c_3 + 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + Al(OH)_3 ⟶ 2 H_2O + AlOHCl2

+ ⟶ + AlOHCl2

hydrogen chloride + aluminum hydroxide ⟶ water + AlOHCl2

Construct the equilibrium constant, K, expression for: HCl + Al(OH)_3 ⟶ H_2O + AlOHCl2 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: 2 HCl + Al(OH)_3 ⟶ 2 H_2O + AlOHCl2 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 HCl | 2 | -2 Al(OH)_3 | 1 | -1 H_2O | 2 | 2 AlOHCl2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) Al(OH)_3 | 1 | -1 | ([Al(OH)3])^(-1) H_2O | 2 | 2 | ([H2O])^2 AlOHCl2 | 1 | 1 | [AlOHCl2] 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 = ([HCl])^(-2) ([Al(OH)3])^(-1) ([H2O])^2 [AlOHCl2] = (([H2O])^2 [AlOHCl2])/(([HCl])^2 [Al(OH)3])

Construct the rate of reaction expression for: HCl + Al(OH)_3 ⟶ H_2O + AlOHCl2 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: 2 HCl + Al(OH)_3 ⟶ 2 H_2O + AlOHCl2 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 HCl | 2 | -2 Al(OH)_3 | 1 | -1 H_2O | 2 | 2 AlOHCl2 | 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 HCl | 2 | -2 | -1/2 (Δ[HCl])/(Δt) Al(OH)_3 | 1 | -1 | -(Δ[Al(OH)3])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) AlOHCl2 | 1 | 1 | (Δ[AlOHCl2])/(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 = -1/2 (Δ[HCl])/(Δt) = -(Δ[Al(OH)3])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[AlOHCl2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen chloride | aluminum hydroxide | water | AlOHCl2 formula | HCl | Al(OH)_3 | H_2O | AlOHCl2 Hill formula | ClH | AlH_3O_3 | H_2O | HAlCl2O name | hydrogen chloride | aluminum hydroxide | water |

| hydrogen chloride | aluminum hydroxide | water | AlOHCl2 molar mass | 36.46 g/mol | 78.003 g/mol | 18.015 g/mol | 114.9 g/mol phase | gas (at STP) | | liquid (at STP) | melting point | -114.17 °C | | 0 °C | boiling point | -85 °C | | 99.9839 °C | density | 0.00149 g/cm^3 (at 25 °C) | | 1 g/cm^3 | solubility in water | miscible | | | surface tension | | | 0.0728 N/m | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | odor | | | odorless |