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HClO4 + Ba(OH)2 = H2O + Ba(ClO4)2

Input interpretation

HClO_4 perchloric acid + Ba(OH)_2 barium hydroxide ⟶ H_2O water + Ba(ClO_4)_2 barium perchlorate
HClO_4 perchloric acid + Ba(OH)_2 barium hydroxide ⟶ H_2O water + Ba(ClO_4)_2 barium perchlorate

Balanced equation

Balance the chemical equation algebraically: HClO_4 + Ba(OH)_2 ⟶ H_2O + Ba(ClO_4)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HClO_4 + c_2 Ba(OH)_2 ⟶ c_3 H_2O + c_4 Ba(ClO_4)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, O and Ba: Cl: | c_1 = 2 c_4 H: | c_1 + 2 c_2 = 2 c_3 O: | 4 c_1 + 2 c_2 = c_3 + 8 c_4 Ba: | 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 = 2 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HClO_4 + Ba(OH)_2 ⟶ 2 H_2O + Ba(ClO_4)_2
Balance the chemical equation algebraically: HClO_4 + Ba(OH)_2 ⟶ H_2O + Ba(ClO_4)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HClO_4 + c_2 Ba(OH)_2 ⟶ c_3 H_2O + c_4 Ba(ClO_4)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, O and Ba: Cl: | c_1 = 2 c_4 H: | c_1 + 2 c_2 = 2 c_3 O: | 4 c_1 + 2 c_2 = c_3 + 8 c_4 Ba: | 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 = 2 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HClO_4 + Ba(OH)_2 ⟶ 2 H_2O + Ba(ClO_4)_2

Structures

+ ⟶ +
+ ⟶ +

Names

perchloric acid + barium hydroxide ⟶ water + barium perchlorate
perchloric acid + barium hydroxide ⟶ water + barium perchlorate

Equilibrium constant

Construct the equilibrium constant, K, expression for: HClO_4 + Ba(OH)_2 ⟶ H_2O + Ba(ClO_4)_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 HClO_4 + Ba(OH)_2 ⟶ 2 H_2O + Ba(ClO_4)_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 HClO_4 | 2 | -2 Ba(OH)_2 | 1 | -1 H_2O | 2 | 2 Ba(ClO_4)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HClO_4 | 2 | -2 | ([HClO4])^(-2) Ba(OH)_2 | 1 | -1 | ([Ba(OH)2])^(-1) H_2O | 2 | 2 | ([H2O])^2 Ba(ClO_4)_2 | 1 | 1 | [Ba(ClO4)2] 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 = ([HClO4])^(-2) ([Ba(OH)2])^(-1) ([H2O])^2 [Ba(ClO4)2] = (([H2O])^2 [Ba(ClO4)2])/(([HClO4])^2 [Ba(OH)2])
Construct the equilibrium constant, K, expression for: HClO_4 + Ba(OH)_2 ⟶ H_2O + Ba(ClO_4)_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 HClO_4 + Ba(OH)_2 ⟶ 2 H_2O + Ba(ClO_4)_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 HClO_4 | 2 | -2 Ba(OH)_2 | 1 | -1 H_2O | 2 | 2 Ba(ClO_4)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HClO_4 | 2 | -2 | ([HClO4])^(-2) Ba(OH)_2 | 1 | -1 | ([Ba(OH)2])^(-1) H_2O | 2 | 2 | ([H2O])^2 Ba(ClO_4)_2 | 1 | 1 | [Ba(ClO4)2] 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 = ([HClO4])^(-2) ([Ba(OH)2])^(-1) ([H2O])^2 [Ba(ClO4)2] = (([H2O])^2 [Ba(ClO4)2])/(([HClO4])^2 [Ba(OH)2])

Rate of reaction

Construct the rate of reaction expression for: HClO_4 + Ba(OH)_2 ⟶ H_2O + Ba(ClO_4)_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 HClO_4 + Ba(OH)_2 ⟶ 2 H_2O + Ba(ClO_4)_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 HClO_4 | 2 | -2 Ba(OH)_2 | 1 | -1 H_2O | 2 | 2 Ba(ClO_4)_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 HClO_4 | 2 | -2 | -1/2 (Δ[HClO4])/(Δt) Ba(OH)_2 | 1 | -1 | -(Δ[Ba(OH)2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) Ba(ClO_4)_2 | 1 | 1 | (Δ[Ba(ClO4)2])/(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[HClO4])/(Δt) = -(Δ[Ba(OH)2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[Ba(ClO4)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HClO_4 + Ba(OH)_2 ⟶ H_2O + Ba(ClO_4)_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 HClO_4 + Ba(OH)_2 ⟶ 2 H_2O + Ba(ClO_4)_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 HClO_4 | 2 | -2 Ba(OH)_2 | 1 | -1 H_2O | 2 | 2 Ba(ClO_4)_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 HClO_4 | 2 | -2 | -1/2 (Δ[HClO4])/(Δt) Ba(OH)_2 | 1 | -1 | -(Δ[Ba(OH)2])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) Ba(ClO_4)_2 | 1 | 1 | (Δ[Ba(ClO4)2])/(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[HClO4])/(Δt) = -(Δ[Ba(OH)2])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[Ba(ClO4)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| perchloric acid | barium hydroxide | water | barium perchlorate formula | HClO_4 | Ba(OH)_2 | H_2O | Ba(ClO_4)_2 Hill formula | ClHO_4 | BaH_2O_2 | H_2O | BaCl_2O_8 name | perchloric acid | barium hydroxide | water | barium perchlorate IUPAC name | perchloric acid | barium(+2) cation dihydroxide | water | barium(+2) cation diperchlorate
| perchloric acid | barium hydroxide | water | barium perchlorate formula | HClO_4 | Ba(OH)_2 | H_2O | Ba(ClO_4)_2 Hill formula | ClHO_4 | BaH_2O_2 | H_2O | BaCl_2O_8 name | perchloric acid | barium hydroxide | water | barium perchlorate IUPAC name | perchloric acid | barium(+2) cation dihydroxide | water | barium(+2) cation diperchlorate

Substance properties

| perchloric acid | barium hydroxide | water | barium perchlorate molar mass | 100.5 g/mol | 171.34 g/mol | 18.015 g/mol | 336.22 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | -112 °C | 300 °C | 0 °C | 505 °C boiling point | 90 °C | | 99.9839 °C | density | 1.77 g/cm^3 | 2.2 g/cm^3 | 1 g/cm^3 | 3.2 g/cm^3 solubility in water | very soluble | | | soluble surface tension | | | 0.0728 N/m | dynamic viscosity | 8×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless |
| perchloric acid | barium hydroxide | water | barium perchlorate molar mass | 100.5 g/mol | 171.34 g/mol | 18.015 g/mol | 336.22 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | -112 °C | 300 °C | 0 °C | 505 °C boiling point | 90 °C | | 99.9839 °C | density | 1.77 g/cm^3 | 2.2 g/cm^3 | 1 g/cm^3 | 3.2 g/cm^3 solubility in water | very soluble | | | soluble surface tension | | | 0.0728 N/m | dynamic viscosity | 8×10^-4 Pa s (at 25 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | odorless | | odorless |

Units

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