Input interpretation
![KOH potassium hydroxide + MgSO_4 magnesium sulfate ⟶ K_2SO_4 potassium sulfate + Mg(OH)_2 magnesium hydroxide](../image_source/087ef4d2ee8d20288721402af2d8bad9.png)
KOH potassium hydroxide + MgSO_4 magnesium sulfate ⟶ K_2SO_4 potassium sulfate + Mg(OH)_2 magnesium hydroxide
Balanced equation
![Balance the chemical equation algebraically: KOH + MgSO_4 ⟶ K_2SO_4 + Mg(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 MgSO_4 ⟶ c_3 K_2SO_4 + c_4 Mg(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, Mg and S: H: | c_1 = 2 c_4 K: | c_1 = 2 c_3 O: | c_1 + 4 c_2 = 4 c_3 + 2 c_4 Mg: | c_2 = c_4 S: | c_2 = c_3 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 + MgSO_4 ⟶ K_2SO_4 + Mg(OH)_2](../image_source/421d660c4b797f325bc5ecedfb38a6c3.png)
Balance the chemical equation algebraically: KOH + MgSO_4 ⟶ K_2SO_4 + Mg(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 KOH + c_2 MgSO_4 ⟶ c_3 K_2SO_4 + c_4 Mg(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, K, O, Mg and S: H: | c_1 = 2 c_4 K: | c_1 = 2 c_3 O: | c_1 + 4 c_2 = 4 c_3 + 2 c_4 Mg: | c_2 = c_4 S: | c_2 = c_3 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 + MgSO_4 ⟶ K_2SO_4 + Mg(OH)_2
Structures
![+ ⟶ +](../image_source/f54b5796832e4b04bfacade6c389ea48.png)
+ ⟶ +
Names
![potassium hydroxide + magnesium sulfate ⟶ potassium sulfate + magnesium hydroxide](../image_source/e27697b543dacd82884787388ed084a8.png)
potassium hydroxide + magnesium sulfate ⟶ potassium sulfate + magnesium hydroxide
Equilibrium constant
![Construct the equilibrium constant, K, expression for: KOH + MgSO_4 ⟶ K_2SO_4 + Mg(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 + MgSO_4 ⟶ K_2SO_4 + Mg(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 MgSO_4 | 1 | -1 K_2SO_4 | 1 | 1 Mg(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) MgSO_4 | 1 | -1 | ([MgSO4])^(-1) K_2SO_4 | 1 | 1 | [K2SO4] Mg(OH)_2 | 1 | 1 | [Mg(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) ([MgSO4])^(-1) [K2SO4] [Mg(OH)2] = ([K2SO4] [Mg(OH)2])/(([KOH])^2 [MgSO4])](../image_source/6508c10e68444117dc2aaa1e5bc5e35f.png)
Construct the equilibrium constant, K, expression for: KOH + MgSO_4 ⟶ K_2SO_4 + Mg(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 + MgSO_4 ⟶ K_2SO_4 + Mg(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 MgSO_4 | 1 | -1 K_2SO_4 | 1 | 1 Mg(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) MgSO_4 | 1 | -1 | ([MgSO4])^(-1) K_2SO_4 | 1 | 1 | [K2SO4] Mg(OH)_2 | 1 | 1 | [Mg(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) ([MgSO4])^(-1) [K2SO4] [Mg(OH)2] = ([K2SO4] [Mg(OH)2])/(([KOH])^2 [MgSO4])
Rate of reaction
![Construct the rate of reaction expression for: KOH + MgSO_4 ⟶ K_2SO_4 + Mg(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 + MgSO_4 ⟶ K_2SO_4 + Mg(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 MgSO_4 | 1 | -1 K_2SO_4 | 1 | 1 Mg(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) MgSO_4 | 1 | -1 | -(Δ[MgSO4])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) Mg(OH)_2 | 1 | 1 | (Δ[Mg(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[MgSO4])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[Mg(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/290b814db820f339a73de225209bf8be.png)
Construct the rate of reaction expression for: KOH + MgSO_4 ⟶ K_2SO_4 + Mg(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 + MgSO_4 ⟶ K_2SO_4 + Mg(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 MgSO_4 | 1 | -1 K_2SO_4 | 1 | 1 Mg(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) MgSO_4 | 1 | -1 | -(Δ[MgSO4])/(Δt) K_2SO_4 | 1 | 1 | (Δ[K2SO4])/(Δt) Mg(OH)_2 | 1 | 1 | (Δ[Mg(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[MgSO4])/(Δt) = (Δ[K2SO4])/(Δt) = (Δ[Mg(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| potassium hydroxide | magnesium sulfate | potassium sulfate | magnesium hydroxide formula | KOH | MgSO_4 | K_2SO_4 | Mg(OH)_2 Hill formula | HKO | MgO_4S | K_2O_4S | H_2MgO_2 name | potassium hydroxide | magnesium sulfate | potassium sulfate | magnesium hydroxide IUPAC name | potassium hydroxide | magnesium sulfate | dipotassium sulfate | magnesium dihydroxide](../image_source/f463301076fb15203c63eabfe40be01a.png)
| potassium hydroxide | magnesium sulfate | potassium sulfate | magnesium hydroxide formula | KOH | MgSO_4 | K_2SO_4 | Mg(OH)_2 Hill formula | HKO | MgO_4S | K_2O_4S | H_2MgO_2 name | potassium hydroxide | magnesium sulfate | potassium sulfate | magnesium hydroxide IUPAC name | potassium hydroxide | magnesium sulfate | dipotassium sulfate | magnesium dihydroxide
Substance properties
![| potassium hydroxide | magnesium sulfate | potassium sulfate | magnesium hydroxide molar mass | 56.105 g/mol | 120.4 g/mol | 174.25 g/mol | 58.319 g/mol phase | solid (at STP) | solid (at STP) | | solid (at STP) melting point | 406 °C | | | 350 °C boiling point | 1327 °C | | | density | 2.044 g/cm^3 | | | 2.3446 g/cm^3 solubility in water | soluble | soluble | soluble | insoluble dynamic viscosity | 0.001 Pa s (at 550 °C) | | |](../image_source/9066066f5b8e0693c4a377126e0c9d20.png)
| potassium hydroxide | magnesium sulfate | potassium sulfate | magnesium hydroxide molar mass | 56.105 g/mol | 120.4 g/mol | 174.25 g/mol | 58.319 g/mol phase | solid (at STP) | solid (at STP) | | solid (at STP) melting point | 406 °C | | | 350 °C boiling point | 1327 °C | | | density | 2.044 g/cm^3 | | | 2.3446 g/cm^3 solubility in water | soluble | soluble | soluble | insoluble dynamic viscosity | 0.001 Pa s (at 550 °C) | | |
Units