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KOH + H2CrO4 = H2O + K2CrO4

Input interpretation

KOH potassium hydroxide + H_2CrO_4 chromic acid ⟶ H_2O water + K_2CrO_4 potassium chromate
KOH potassium hydroxide + H_2CrO_4 chromic acid ⟶ H_2O water + K_2CrO_4 potassium chromate

Balanced equation

Balance the chemical equation algebraically: KOH + H_2CrO_4 ⟶ H_2O + K_2CrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 H_2CrO_4 ⟶ c_3 H_2O + c_4 K_2CrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O and Cr: H: | c_1 + 2 c_2 = 2 c_3 K: | c_1 = 2 c_4 O: | c_1 + 4 c_2 = c_3 + 4 c_4 Cr: | 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 KOH + H_2CrO_4 ⟶ 2 H_2O + K_2CrO_4
Balance the chemical equation algebraically: KOH + H_2CrO_4 ⟶ H_2O + K_2CrO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 H_2CrO_4 ⟶ c_3 H_2O + c_4 K_2CrO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O and Cr: H: | c_1 + 2 c_2 = 2 c_3 K: | c_1 = 2 c_4 O: | c_1 + 4 c_2 = c_3 + 4 c_4 Cr: | 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 KOH + H_2CrO_4 ⟶ 2 H_2O + K_2CrO_4

Structures

+ ⟶ +
+ ⟶ +

Names

potassium hydroxide + chromic acid ⟶ water + potassium chromate
potassium hydroxide + chromic acid ⟶ water + potassium chromate

Equilibrium constant

Construct the equilibrium constant, K, expression for: KOH + H_2CrO_4 ⟶ H_2O + K_2CrO_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: 2 KOH + H_2CrO_4 ⟶ 2 H_2O + K_2CrO_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 KOH | 2 | -2 H_2CrO_4 | 1 | -1 H_2O | 2 | 2 K_2CrO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 2 | -2 | ([KOH])^(-2) H_2CrO_4 | 1 | -1 | ([H2CrO4])^(-1) H_2O | 2 | 2 | ([H2O])^2 K_2CrO_4 | 1 | 1 | [K2CrO4] 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])^(-2) ([H2CrO4])^(-1) ([H2O])^2 [K2CrO4] = (([H2O])^2 [K2CrO4])/(([KOH])^2 [H2CrO4])
Construct the equilibrium constant, K, expression for: KOH + H_2CrO_4 ⟶ H_2O + K_2CrO_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: 2 KOH + H_2CrO_4 ⟶ 2 H_2O + K_2CrO_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 KOH | 2 | -2 H_2CrO_4 | 1 | -1 H_2O | 2 | 2 K_2CrO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression KOH | 2 | -2 | ([KOH])^(-2) H_2CrO_4 | 1 | -1 | ([H2CrO4])^(-1) H_2O | 2 | 2 | ([H2O])^2 K_2CrO_4 | 1 | 1 | [K2CrO4] 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])^(-2) ([H2CrO4])^(-1) ([H2O])^2 [K2CrO4] = (([H2O])^2 [K2CrO4])/(([KOH])^2 [H2CrO4])

Rate of reaction

Construct the rate of reaction expression for: KOH + H_2CrO_4 ⟶ H_2O + K_2CrO_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: 2 KOH + H_2CrO_4 ⟶ 2 H_2O + K_2CrO_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 KOH | 2 | -2 H_2CrO_4 | 1 | -1 H_2O | 2 | 2 K_2CrO_4 | 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 | 2 | -2 | -1/2 (Δ[KOH])/(Δt) H_2CrO_4 | 1 | -1 | -(Δ[H2CrO4])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) K_2CrO_4 | 1 | 1 | (Δ[K2CrO4])/(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[KOH])/(Δt) = -(Δ[H2CrO4])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[K2CrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KOH + H_2CrO_4 ⟶ H_2O + K_2CrO_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: 2 KOH + H_2CrO_4 ⟶ 2 H_2O + K_2CrO_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 KOH | 2 | -2 H_2CrO_4 | 1 | -1 H_2O | 2 | 2 K_2CrO_4 | 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 | 2 | -2 | -1/2 (Δ[KOH])/(Δt) H_2CrO_4 | 1 | -1 | -(Δ[H2CrO4])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) K_2CrO_4 | 1 | 1 | (Δ[K2CrO4])/(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[KOH])/(Δt) = -(Δ[H2CrO4])/(Δt) = 1/2 (Δ[H2O])/(Δt) = (Δ[K2CrO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium hydroxide | chromic acid | water | potassium chromate formula | KOH | H_2CrO_4 | H_2O | K_2CrO_4 Hill formula | HKO | CrH_2O_4 | H_2O | CrK_2O_4 name | potassium hydroxide | chromic acid | water | potassium chromate IUPAC name | potassium hydroxide | dihydroxy-dioxo-chromium | water | dipotassium dioxido-dioxochromium
| potassium hydroxide | chromic acid | water | potassium chromate formula | KOH | H_2CrO_4 | H_2O | K_2CrO_4 Hill formula | HKO | CrH_2O_4 | H_2O | CrK_2O_4 name | potassium hydroxide | chromic acid | water | potassium chromate IUPAC name | potassium hydroxide | dihydroxy-dioxo-chromium | water | dipotassium dioxido-dioxochromium

Substance properties

| potassium hydroxide | chromic acid | water | potassium chromate molar mass | 56.105 g/mol | 118.01 g/mol | 18.015 g/mol | 194.19 g/mol phase | solid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | 406 °C | 196 °C | 0 °C | 971 °C boiling point | 1327 °C | | 99.9839 °C | density | 2.044 g/cm^3 | 2.7 g/cm^3 | 1 g/cm^3 | 2.73 g/cm^3 solubility in water | soluble | very 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
| potassium hydroxide | chromic acid | water | potassium chromate molar mass | 56.105 g/mol | 118.01 g/mol | 18.015 g/mol | 194.19 g/mol phase | solid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | 406 °C | 196 °C | 0 °C | 971 °C boiling point | 1327 °C | | 99.9839 °C | density | 2.044 g/cm^3 | 2.7 g/cm^3 | 1 g/cm^3 | 2.73 g/cm^3 solubility in water | soluble | very 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

Units

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