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KOH + ZnSO4 = K2SO4 + Zn(OH)2

Input interpretation

KOH potassium hydroxide + ZnSO_4 zinc sulfate ⟶ K_2SO_4 potassium sulfate + Zn(OH)_2 zinc hydroxide
KOH potassium hydroxide + ZnSO_4 zinc sulfate ⟶ K_2SO_4 potassium sulfate + Zn(OH)_2 zinc hydroxide

Balanced equation

Balance the chemical equation algebraically: KOH + ZnSO_4 ⟶ K_2SO_4 + Zn(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 ZnSO_4 ⟶ c_3 K_2SO_4 + c_4 Zn(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, S and Zn: H: | c_1 = 2 c_4 K: | c_1 = 2 c_3 O: | c_1 + 4 c_2 = 4 c_3 + 2 c_4 S: | c_2 = c_3 Zn: | 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 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KOH + ZnSO_4 ⟶ K_2SO_4 + Zn(OH)_2
Balance the chemical equation algebraically: KOH + ZnSO_4 ⟶ K_2SO_4 + Zn(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 ZnSO_4 ⟶ c_3 K_2SO_4 + c_4 Zn(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, S and Zn: H: | c_1 = 2 c_4 K: | c_1 = 2 c_3 O: | c_1 + 4 c_2 = 4 c_3 + 2 c_4 S: | c_2 = c_3 Zn: | 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 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 KOH + ZnSO_4 ⟶ K_2SO_4 + Zn(OH)_2

Structures

+ ⟶ +
+ ⟶ +

Names

potassium hydroxide + zinc sulfate ⟶ potassium sulfate + zinc hydroxide
potassium hydroxide + zinc sulfate ⟶ potassium sulfate + zinc hydroxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: KOH + ZnSO_4 ⟶ K_2SO_4 + Zn(OH)_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 KOH + ZnSO_4 ⟶ K_2SO_4 + Zn(OH)_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 KOH | 2 | -2 ZnSO_4 | 1 | -1 K_2SO_4 | 1 | 1 Zn(OH)_2 | 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) ZnSO_4 | 1 | -1 | ([ZnSO4])^(-1) K_2SO_4 | 1 | 1 | [K2SO4] Zn(OH)_2 | 1 | 1 | [Zn(OH)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 = ([KOH])^(-2) ([ZnSO4])^(-1) [K2SO4] [Zn(OH)2] = ([K2SO4] [Zn(OH)2])/(([KOH])^2 [ZnSO4])
Construct the equilibrium constant, K, expression for: KOH + ZnSO_4 ⟶ K_2SO_4 + Zn(OH)_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 KOH + ZnSO_4 ⟶ K_2SO_4 + Zn(OH)_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 KOH | 2 | -2 ZnSO_4 | 1 | -1 K_2SO_4 | 1 | 1 Zn(OH)_2 | 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) ZnSO_4 | 1 | -1 | ([ZnSO4])^(-1) K_2SO_4 | 1 | 1 | [K2SO4] Zn(OH)_2 | 1 | 1 | [Zn(OH)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 = ([KOH])^(-2) ([ZnSO4])^(-1) [K2SO4] [Zn(OH)2] = ([K2SO4] [Zn(OH)2])/(([KOH])^2 [ZnSO4])

Rate of reaction

Construct the rate of reaction expression for: KOH + ZnSO_4 ⟶ K_2SO_4 + Zn(OH)_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 KOH + ZnSO_4 ⟶ K_2SO_4 + Zn(OH)_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 KOH | 2 | -2 ZnSO_4 | 1 | -1 K_2SO_4 | 1 | 1 Zn(OH)_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 KOH | 2 | -2 | -1/2 (Δ[KOH])/(Δt) ZnSO_4 | 1 | -1 | -(Δ[ZnSO4])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) Zn(OH)_2 | 1 | 1 | (Δ[Zn(OH)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[KOH])/(Δt) = -(Δ[ZnSO4])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[Zn(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: KOH + ZnSO_4 ⟶ K_2SO_4 + Zn(OH)_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 KOH + ZnSO_4 ⟶ K_2SO_4 + Zn(OH)_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 KOH | 2 | -2 ZnSO_4 | 1 | -1 K_2SO_4 | 1 | 1 Zn(OH)_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 KOH | 2 | -2 | -1/2 (Δ[KOH])/(Δt) ZnSO_4 | 1 | -1 | -(Δ[ZnSO4])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) Zn(OH)_2 | 1 | 1 | (Δ[Zn(OH)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[KOH])/(Δt) = -(Δ[ZnSO4])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[Zn(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium hydroxide | zinc sulfate | potassium sulfate | zinc hydroxide formula | KOH | ZnSO_4 | K_2SO_4 | Zn(OH)_2 Hill formula | HKO | O_4SZn | K_2O_4S | H_2O_2Zn name | potassium hydroxide | zinc sulfate | potassium sulfate | zinc hydroxide IUPAC name | potassium hydroxide | zinc sulfate | dipotassium sulfate | zinc dihydroxide
| potassium hydroxide | zinc sulfate | potassium sulfate | zinc hydroxide formula | KOH | ZnSO_4 | K_2SO_4 | Zn(OH)_2 Hill formula | HKO | O_4SZn | K_2O_4S | H_2O_2Zn name | potassium hydroxide | zinc sulfate | potassium sulfate | zinc hydroxide IUPAC name | potassium hydroxide | zinc sulfate | dipotassium sulfate | zinc dihydroxide

Substance properties

| potassium hydroxide | zinc sulfate | potassium sulfate | zinc hydroxide molar mass | 56.105 g/mol | 161.4 g/mol | 174.25 g/mol | 99.39 g/mol phase | solid (at STP) | | | melting point | 406 °C | | | boiling point | 1327 °C | | | density | 2.044 g/cm^3 | 1.005 g/cm^3 | | solubility in water | soluble | soluble | soluble | dynamic viscosity | 0.001 Pa s (at 550 °C) | | | odor | | odorless | |
| potassium hydroxide | zinc sulfate | potassium sulfate | zinc hydroxide molar mass | 56.105 g/mol | 161.4 g/mol | 174.25 g/mol | 99.39 g/mol phase | solid (at STP) | | | melting point | 406 °C | | | boiling point | 1327 °C | | | density | 2.044 g/cm^3 | 1.005 g/cm^3 | | solubility in water | soluble | soluble | soluble | dynamic viscosity | 0.001 Pa s (at 550 °C) | | | odor | | odorless | |

Units

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