NaClO = NaCl + NaClO2

NaOCl sodium hypochlorite ⟶ NaCl sodium chloride + NaClO_2 sodium chlorite

Balance the chemical equation algebraically: NaOCl ⟶ NaCl + NaClO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOCl ⟶ c_2 NaCl + c_3 NaClO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, Na and O: Cl: | c_1 = c_2 + c_3 Na: | c_1 = c_2 + c_3 O: | c_1 = 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NaOCl ⟶ NaCl + NaClO_2

⟶ +

sodium hypochlorite ⟶ sodium chloride + sodium chlorite

Construct the equilibrium constant, K, expression for: NaOCl ⟶ NaCl + NaClO_2 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 NaOCl ⟶ NaCl + NaClO_2 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 NaOCl | 2 | -2 NaCl | 1 | 1 NaClO_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOCl | 2 | -2 | ([NaOCl])^(-2) NaCl | 1 | 1 | [NaCl] NaClO_2 | 1 | 1 | [NaClO2] 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 = ([NaOCl])^(-2) [NaCl] [NaClO2] = ([NaCl] [NaClO2])/([NaOCl])^2

Construct the rate of reaction expression for: NaOCl ⟶ NaCl + NaClO_2 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 NaOCl ⟶ NaCl + NaClO_2 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 NaOCl | 2 | -2 NaCl | 1 | 1 NaClO_2 | 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 NaOCl | 2 | -2 | -1/2 (Δ[NaOCl])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(Δt) NaClO_2 | 1 | 1 | (Δ[NaClO2])/(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[NaOCl])/(Δt) = (Δ[NaCl])/(Δt) = (Δ[NaClO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sodium hypochlorite | sodium chloride | sodium chlorite formula | NaOCl | NaCl | NaClO_2 Hill formula | ClNaO | ClNa | ClNaO_2 name | sodium hypochlorite | sodium chloride | sodium chlorite

| sodium hypochlorite | sodium chloride | sodium chlorite molar mass | 74.44 g/mol | 58.44 g/mol | 90.44 g/mol phase | liquid (at STP) | solid (at STP) | melting point | -6 °C | 801 °C | boiling point | | 1413 °C | density | 1.11 g/cm^3 | 2.16 g/cm^3 | solubility in water | miscible | soluble | odor | | odorless |