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HCl + KBrO3 + Na2HAsO3 = NaCl + KBr + H3AsO4

Input interpretation

HCl hydrogen chloride + KBrO_3 potassium bromate + Na2HAsO3 ⟶ NaCl sodium chloride + KBr potassium bromide + H_3AsO_4 arsenic acid, solid
HCl hydrogen chloride + KBrO_3 potassium bromate + Na2HAsO3 ⟶ NaCl sodium chloride + KBr potassium bromide + H_3AsO_4 arsenic acid, solid

Balanced equation

Balance the chemical equation algebraically: HCl + KBrO_3 + Na2HAsO3 ⟶ NaCl + KBr + H_3AsO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 KBrO_3 + c_3 Na2HAsO3 ⟶ c_4 NaCl + c_5 KBr + c_6 H_3AsO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Br, K, O, Na and As: Cl: | c_1 = c_4 H: | c_1 + c_3 = 3 c_6 Br: | c_2 = c_5 K: | c_2 = c_5 O: | 3 c_2 + 3 c_3 = 4 c_6 Na: | 2 c_3 = c_4 As: | c_3 = c_6 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 = 6 c_2 = 1 c_3 = 3 c_4 = 6 c_5 = 1 c_6 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 HCl + KBrO_3 + 3 Na2HAsO3 ⟶ 6 NaCl + KBr + 3 H_3AsO_4
Balance the chemical equation algebraically: HCl + KBrO_3 + Na2HAsO3 ⟶ NaCl + KBr + H_3AsO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 KBrO_3 + c_3 Na2HAsO3 ⟶ c_4 NaCl + c_5 KBr + c_6 H_3AsO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Br, K, O, Na and As: Cl: | c_1 = c_4 H: | c_1 + c_3 = 3 c_6 Br: | c_2 = c_5 K: | c_2 = c_5 O: | 3 c_2 + 3 c_3 = 4 c_6 Na: | 2 c_3 = c_4 As: | c_3 = c_6 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 = 6 c_2 = 1 c_3 = 3 c_4 = 6 c_5 = 1 c_6 = 3 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 6 HCl + KBrO_3 + 3 Na2HAsO3 ⟶ 6 NaCl + KBr + 3 H_3AsO_4

Structures

+ + Na2HAsO3 ⟶ + +
+ + Na2HAsO3 ⟶ + +

Names

hydrogen chloride + potassium bromate + Na2HAsO3 ⟶ sodium chloride + potassium bromide + arsenic acid, solid
hydrogen chloride + potassium bromate + Na2HAsO3 ⟶ sodium chloride + potassium bromide + arsenic acid, solid

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + KBrO_3 + Na2HAsO3 ⟶ NaCl + KBr + H_3AsO_4 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: 6 HCl + KBrO_3 + 3 Na2HAsO3 ⟶ 6 NaCl + KBr + 3 H_3AsO_4 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 | 6 | -6 KBrO_3 | 1 | -1 Na2HAsO3 | 3 | -3 NaCl | 6 | 6 KBr | 1 | 1 H_3AsO_4 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 6 | -6 | ([HCl])^(-6) KBrO_3 | 1 | -1 | ([KBrO3])^(-1) Na2HAsO3 | 3 | -3 | ([Na2HAsO3])^(-3) NaCl | 6 | 6 | ([NaCl])^6 KBr | 1 | 1 | [KBr] H_3AsO_4 | 3 | 3 | ([H3AsO4])^3 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])^(-6) ([KBrO3])^(-1) ([Na2HAsO3])^(-3) ([NaCl])^6 [KBr] ([H3AsO4])^3 = (([NaCl])^6 [KBr] ([H3AsO4])^3)/(([HCl])^6 [KBrO3] ([Na2HAsO3])^3)
Construct the equilibrium constant, K, expression for: HCl + KBrO_3 + Na2HAsO3 ⟶ NaCl + KBr + H_3AsO_4 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: 6 HCl + KBrO_3 + 3 Na2HAsO3 ⟶ 6 NaCl + KBr + 3 H_3AsO_4 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 | 6 | -6 KBrO_3 | 1 | -1 Na2HAsO3 | 3 | -3 NaCl | 6 | 6 KBr | 1 | 1 H_3AsO_4 | 3 | 3 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 6 | -6 | ([HCl])^(-6) KBrO_3 | 1 | -1 | ([KBrO3])^(-1) Na2HAsO3 | 3 | -3 | ([Na2HAsO3])^(-3) NaCl | 6 | 6 | ([NaCl])^6 KBr | 1 | 1 | [KBr] H_3AsO_4 | 3 | 3 | ([H3AsO4])^3 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])^(-6) ([KBrO3])^(-1) ([Na2HAsO3])^(-3) ([NaCl])^6 [KBr] ([H3AsO4])^3 = (([NaCl])^6 [KBr] ([H3AsO4])^3)/(([HCl])^6 [KBrO3] ([Na2HAsO3])^3)

Rate of reaction

Construct the rate of reaction expression for: HCl + KBrO_3 + Na2HAsO3 ⟶ NaCl + KBr + H_3AsO_4 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: 6 HCl + KBrO_3 + 3 Na2HAsO3 ⟶ 6 NaCl + KBr + 3 H_3AsO_4 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 | 6 | -6 KBrO_3 | 1 | -1 Na2HAsO3 | 3 | -3 NaCl | 6 | 6 KBr | 1 | 1 H_3AsO_4 | 3 | 3 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 | 6 | -6 | -1/6 (Δ[HCl])/(Δt) KBrO_3 | 1 | -1 | -(Δ[KBrO3])/(Δt) Na2HAsO3 | 3 | -3 | -1/3 (Δ[Na2HAsO3])/(Δt) NaCl | 6 | 6 | 1/6 (Δ[NaCl])/(Δt) KBr | 1 | 1 | (Δ[KBr])/(Δt) H_3AsO_4 | 3 | 3 | 1/3 (Δ[H3AsO4])/(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 = -1/6 (Δ[HCl])/(Δt) = -(Δ[KBrO3])/(Δt) = -1/3 (Δ[Na2HAsO3])/(Δt) = 1/6 (Δ[NaCl])/(Δt) = (Δ[KBr])/(Δt) = 1/3 (Δ[H3AsO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + KBrO_3 + Na2HAsO3 ⟶ NaCl + KBr + H_3AsO_4 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: 6 HCl + KBrO_3 + 3 Na2HAsO3 ⟶ 6 NaCl + KBr + 3 H_3AsO_4 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 | 6 | -6 KBrO_3 | 1 | -1 Na2HAsO3 | 3 | -3 NaCl | 6 | 6 KBr | 1 | 1 H_3AsO_4 | 3 | 3 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 | 6 | -6 | -1/6 (Δ[HCl])/(Δt) KBrO_3 | 1 | -1 | -(Δ[KBrO3])/(Δt) Na2HAsO3 | 3 | -3 | -1/3 (Δ[Na2HAsO3])/(Δt) NaCl | 6 | 6 | 1/6 (Δ[NaCl])/(Δt) KBr | 1 | 1 | (Δ[KBr])/(Δt) H_3AsO_4 | 3 | 3 | 1/3 (Δ[H3AsO4])/(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 = -1/6 (Δ[HCl])/(Δt) = -(Δ[KBrO3])/(Δt) = -1/3 (Δ[Na2HAsO3])/(Δt) = 1/6 (Δ[NaCl])/(Δt) = (Δ[KBr])/(Δt) = 1/3 (Δ[H3AsO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | potassium bromate | Na2HAsO3 | sodium chloride | potassium bromide | arsenic acid, solid formula | HCl | KBrO_3 | Na2HAsO3 | NaCl | KBr | H_3AsO_4 Hill formula | ClH | BrKO_3 | HAsNa2O3 | ClNa | BrK | AsH_3O_4 name | hydrogen chloride | potassium bromate | | sodium chloride | potassium bromide | arsenic acid, solid IUPAC name | hydrogen chloride | potassium bromate | | sodium chloride | potassium bromide | arsoric acid
| hydrogen chloride | potassium bromate | Na2HAsO3 | sodium chloride | potassium bromide | arsenic acid, solid formula | HCl | KBrO_3 | Na2HAsO3 | NaCl | KBr | H_3AsO_4 Hill formula | ClH | BrKO_3 | HAsNa2O3 | ClNa | BrK | AsH_3O_4 name | hydrogen chloride | potassium bromate | | sodium chloride | potassium bromide | arsenic acid, solid IUPAC name | hydrogen chloride | potassium bromate | | sodium chloride | potassium bromide | arsoric acid

Substance properties

| hydrogen chloride | potassium bromate | Na2HAsO3 | sodium chloride | potassium bromide | arsenic acid, solid molar mass | 36.46 g/mol | 167 g/mol | 169.91 g/mol | 58.44 g/mol | 119 g/mol | 141.94 g/mol phase | gas (at STP) | solid (at STP) | | solid (at STP) | solid (at STP) | solid (at STP) melting point | -114.17 °C | 350 °C | | 801 °C | 734 °C | 35.5 °C boiling point | -85 °C | | | 1413 °C | 1435 °C | 160 °C density | 0.00149 g/cm^3 (at 25 °C) | 3.218 g/cm^3 | | 2.16 g/cm^3 | 2.75 g/cm^3 | 2.2 g/cm^3 solubility in water | miscible | | | soluble | soluble | odor | | | | odorless | |
| hydrogen chloride | potassium bromate | Na2HAsO3 | sodium chloride | potassium bromide | arsenic acid, solid molar mass | 36.46 g/mol | 167 g/mol | 169.91 g/mol | 58.44 g/mol | 119 g/mol | 141.94 g/mol phase | gas (at STP) | solid (at STP) | | solid (at STP) | solid (at STP) | solid (at STP) melting point | -114.17 °C | 350 °C | | 801 °C | 734 °C | 35.5 °C boiling point | -85 °C | | | 1413 °C | 1435 °C | 160 °C density | 0.00149 g/cm^3 (at 25 °C) | 3.218 g/cm^3 | | 2.16 g/cm^3 | 2.75 g/cm^3 | 2.2 g/cm^3 solubility in water | miscible | | | soluble | soluble | odor | | | | odorless | |

Units

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