HCl + NaOH = NaClH2O

HCl hydrogen chloride + NaOH sodium hydroxide ⟶ NaClH2O

Balance the chemical equation algebraically: HCl + NaOH ⟶ NaClH2O Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 NaOH ⟶ c_3 NaClH2O Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Na and O: Cl: | c_1 = c_3 H: | c_1 + c_2 = 2 c_3 Na: | c_2 = c_3 O: | c_2 = c_3 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 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | HCl + NaOH ⟶ NaClH2O

+ ⟶ NaClH2O

hydrogen chloride + sodium hydroxide ⟶ NaClH2O

Construct the equilibrium constant, K, expression for: HCl + NaOH ⟶ NaClH2O 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 + NaOH ⟶ NaClH2O 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 NaOH | 1 | -1 NaClH2O | 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) NaOH | 1 | -1 | ([NaOH])^(-1) NaClH2O | 1 | 1 | [NaClH2O] 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) ([NaOH])^(-1) [NaClH2O] = ([NaClH2O])/([HCl] [NaOH])

Construct the rate of reaction expression for: HCl + NaOH ⟶ NaClH2O 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 + NaOH ⟶ NaClH2O 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 NaOH | 1 | -1 NaClH2O | 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) NaOH | 1 | -1 | -(Δ[NaOH])/(Δt) NaClH2O | 1 | 1 | (Δ[NaClH2O])/(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[NaOH])/(Δt) = (Δ[NaClH2O])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen chloride | sodium hydroxide | NaClH2O formula | HCl | NaOH | NaClH2O Hill formula | ClH | HNaO | H2ClNaO name | hydrogen chloride | sodium hydroxide |

| hydrogen chloride | sodium hydroxide | NaClH2O molar mass | 36.46 g/mol | 39.997 g/mol | 76.45 g/mol phase | gas (at STP) | solid (at STP) | melting point | -114.17 °C | 323 °C | boiling point | -85 °C | 1390 °C | density | 0.00149 g/cm^3 (at 25 °C) | 2.13 g/cm^3 | solubility in water | miscible | soluble | surface tension | | 0.07435 N/m | dynamic viscosity | | 0.004 Pa s (at 350 °C) |