KOH + H5IO6 = H2O + K5IO6

KOH potassium hydroxide + H_5IO_6 periodic acid ⟶ H_2O water + K5IO6

Balance the chemical equation algebraically: KOH + H_5IO_6 ⟶ H_2O + K5IO6 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 H_5IO_6 ⟶ c_3 H_2O + c_4 K5IO6 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O and I: H: | c_1 + 5 c_2 = 2 c_3 K: | c_1 = 5 c_4 O: | c_1 + 6 c_2 = c_3 + 6 c_4 I: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 5 c_2 = 1 c_3 = 5 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 5 KOH + H_5IO_6 ⟶ 5 H_2O + K5IO6

+ ⟶ + K5IO6

potassium hydroxide + periodic acid ⟶ water + K5IO6

Construct the equilibrium constant, K, expression for: KOH + H_5IO_6 ⟶ H_2O + K5IO6 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: 5 KOH + H_5IO_6 ⟶ 5 H_2O + K5IO6 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 KOH | 5 | -5 H_5IO_6 | 1 | -1 H_2O | 5 | 5 K5IO6 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 5 | -5 | ([KOH])^(-5) H_5IO_6 | 1 | -1 | ([H5IO6])^(-1) H_2O | 5 | 5 | ([H2O])^5 K5IO6 | 1 | 1 | [K5IO6] 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 = ([KOH])^(-5) ([H5IO6])^(-1) ([H2O])^5 [K5IO6] = (([H2O])^5 [K5IO6])/(([KOH])^5 [H5IO6])

Construct the rate of reaction expression for: KOH + H_5IO_6 ⟶ H_2O + K5IO6 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: 5 KOH + H_5IO_6 ⟶ 5 H_2O + K5IO6 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 KOH | 5 | -5 H_5IO_6 | 1 | -1 H_2O | 5 | 5 K5IO6 | 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 KOH | 5 | -5 | -1/5 (Δ[KOH])/(Δt) H_5IO_6 | 1 | -1 | -(Δ[H5IO6])/(Δt) H_2O | 5 | 5 | 1/5 (Δ[H2O])/(Δt) K5IO6 | 1 | 1 | (Δ[K5IO6])/(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 = -1/5 (Δ[KOH])/(Δt) = -(Δ[H5IO6])/(Δt) = 1/5 (Δ[H2O])/(Δt) = (Δ[K5IO6])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| potassium hydroxide | periodic acid | water | K5IO6 formula | KOH | H_5IO_6 | H_2O | K5IO6 Hill formula | HKO | H_5IO_6 | H_2O | IK5O6 name | potassium hydroxide | periodic acid | water |

| potassium hydroxide | periodic acid | water | K5IO6 molar mass | 56.105 g/mol | 227.94 g/mol | 18.015 g/mol | 418.39 g/mol phase | solid (at STP) | solid (at STP) | liquid (at STP) | melting point | 406 °C | 122 °C | 0 °C | boiling point | 1327 °C | | 99.9839 °C | density | 2.044 g/cm^3 | 1.3875 g/cm^3 | 1 g/cm^3 | solubility in water | soluble | soluble | | surface tension | | | 0.0728 N/m | dynamic viscosity | 0.001 Pa s (at 550 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | | odorless | odorless |