HCl + Mg(OH)2 = H2O + MgOHCl

HCl hydrogen chloride + Mg(OH)_2 magnesium hydroxide ⟶ H_2O water + MgOHCl

Balance the chemical equation algebraically: HCl + Mg(OH)_2 ⟶ H_2O + MgOHCl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Mg(OH)_2 ⟶ c_3 H_2O + c_4 MgOHCl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Mg and O: Cl: | c_1 = c_4 H: | c_1 + 2 c_2 = 2 c_3 + c_4 Mg: | c_2 = c_4 O: | 2 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_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: | | HCl + Mg(OH)_2 ⟶ H_2O + MgOHCl

+ ⟶ + MgOHCl

hydrogen chloride + magnesium hydroxide ⟶ water + MgOHCl

Construct the equilibrium constant, K, expression for: HCl + Mg(OH)_2 ⟶ H_2O + MgOHCl 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: HCl + Mg(OH)_2 ⟶ H_2O + MgOHCl 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 | 1 | -1 Mg(OH)_2 | 1 | -1 H_2O | 1 | 1 MgOHCl | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 1 | -1 | ([HCl])^(-1) Mg(OH)_2 | 1 | -1 | ([Mg(OH)2])^(-1) H_2O | 1 | 1 | [H2O] MgOHCl | 1 | 1 | [MgOHCl] 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])^(-1) ([Mg(OH)2])^(-1) [H2O] [MgOHCl] = ([H2O] [MgOHCl])/([HCl] [Mg(OH)2])

Construct the rate of reaction expression for: HCl + Mg(OH)_2 ⟶ H_2O + MgOHCl 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: HCl + Mg(OH)_2 ⟶ H_2O + MgOHCl 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 | 1 | -1 Mg(OH)_2 | 1 | -1 H_2O | 1 | 1 MgOHCl | 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 | 1 | -1 | -(Δ[HCl])/(Δt) Mg(OH)_2 | 1 | -1 | -(Δ[Mg(OH)2])/(Δt) H_2O | 1 | 1 | (Δ[H2O])/(Δt) MgOHCl | 1 | 1 | (Δ[MgOHCl])/(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[HCl])/(Δt) = -(Δ[Mg(OH)2])/(Δt) = (Δ[H2O])/(Δt) = (Δ[MgOHCl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen chloride | magnesium hydroxide | water | MgOHCl formula | HCl | Mg(OH)_2 | H_2O | MgOHCl Hill formula | ClH | H_2MgO_2 | H_2O | HClMgO name | hydrogen chloride | magnesium hydroxide | water | IUPAC name | hydrogen chloride | magnesium dihydroxide | water |

| hydrogen chloride | magnesium hydroxide | water | MgOHCl molar mass | 36.46 g/mol | 58.319 g/mol | 18.015 g/mol | 76.76 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | melting point | -114.17 °C | 350 °C | 0 °C | boiling point | -85 °C | | 99.9839 °C | density | 0.00149 g/cm^3 (at 25 °C) | 2.3446 g/cm^3 | 1 g/cm^3 | solubility in water | miscible | insoluble | | surface tension | | | 0.0728 N/m | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | odor | | | odorless |