Search

K2SO4 + Ba(OH)2 = KOH + BaSO4

Input interpretation

K_2SO_4 potassium sulfate + Ba(OH)_2 barium hydroxide ⟶ KOH potassium hydroxide + BaSO_4 barium sulfate
K_2SO_4 potassium sulfate + Ba(OH)_2 barium hydroxide ⟶ KOH potassium hydroxide + BaSO_4 barium sulfate

Balanced equation

Balance the chemical equation algebraically: K_2SO_4 + Ba(OH)_2 ⟶ KOH + BaSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 K_2SO_4 + c_2 Ba(OH)_2 ⟶ c_3 KOH + c_4 BaSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for K, O, S, Ba and H: K: | 2 c_1 = c_3 O: | 4 c_1 + 2 c_2 = c_3 + 4 c_4 S: | c_1 = c_4 Ba: | c_2 = c_4 H: | 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | K_2SO_4 + Ba(OH)_2 ⟶ 2 KOH + BaSO_4
Balance the chemical equation algebraically: K_2SO_4 + Ba(OH)_2 ⟶ KOH + BaSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 K_2SO_4 + c_2 Ba(OH)_2 ⟶ c_3 KOH + c_4 BaSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for K, O, S, Ba and H: K: | 2 c_1 = c_3 O: | 4 c_1 + 2 c_2 = c_3 + 4 c_4 S: | c_1 = c_4 Ba: | c_2 = c_4 H: | 2 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | K_2SO_4 + Ba(OH)_2 ⟶ 2 KOH + BaSO_4

Structures

+ ⟶ +
+ ⟶ +

Names

potassium sulfate + barium hydroxide ⟶ potassium hydroxide + barium sulfate
potassium sulfate + barium hydroxide ⟶ potassium hydroxide + barium sulfate

Equilibrium constant

Construct the equilibrium constant, K, expression for: K_2SO_4 + Ba(OH)_2 ⟶ KOH + BaSO_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: K_2SO_4 + Ba(OH)_2 ⟶ 2 KOH + BaSO_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 K_2SO_4 | 1 | -1 Ba(OH)_2 | 1 | -1 KOH | 2 | 2 BaSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression K_2SO_4 | 1 | -1 | ([K2SO4])^(-1) Ba(OH)_2 | 1 | -1 | ([Ba(OH)2])^(-1) KOH | 2 | 2 | ([KOH])^2 BaSO_4 | 1 | 1 | [BaSO4] 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 = ([K2SO4])^(-1) ([Ba(OH)2])^(-1) ([KOH])^2 [BaSO4] = (([KOH])^2 [BaSO4])/([K2SO4] [Ba(OH)2])
Construct the equilibrium constant, K, expression for: K_2SO_4 + Ba(OH)_2 ⟶ KOH + BaSO_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: K_2SO_4 + Ba(OH)_2 ⟶ 2 KOH + BaSO_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 K_2SO_4 | 1 | -1 Ba(OH)_2 | 1 | -1 KOH | 2 | 2 BaSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression K_2SO_4 | 1 | -1 | ([K2SO4])^(-1) Ba(OH)_2 | 1 | -1 | ([Ba(OH)2])^(-1) KOH | 2 | 2 | ([KOH])^2 BaSO_4 | 1 | 1 | [BaSO4] 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 = ([K2SO4])^(-1) ([Ba(OH)2])^(-1) ([KOH])^2 [BaSO4] = (([KOH])^2 [BaSO4])/([K2SO4] [Ba(OH)2])

Rate of reaction

Construct the rate of reaction expression for: K_2SO_4 + Ba(OH)_2 ⟶ KOH + BaSO_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: K_2SO_4 + Ba(OH)_2 ⟶ 2 KOH + BaSO_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 K_2SO_4 | 1 | -1 Ba(OH)_2 | 1 | -1 KOH | 2 | 2 BaSO_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 K_2SO_4 | 1 | -1 | -(Δ[K2SO4])/(Δt) Ba(OH)_2 | 1 | -1 | -(Δ[Ba(OH)2])/(Δt) KOH | 2 | 2 | 1/2 (Δ[KOH])/(Δt) BaSO_4 | 1 | 1 | (Δ[BaSO4])/(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 = -(Δ[K2SO4])/(Δt) = -(Δ[Ba(OH)2])/(Δt) = 1/2 (Δ[KOH])/(Δt) = (Δ[BaSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: K_2SO_4 + Ba(OH)_2 ⟶ KOH + BaSO_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: K_2SO_4 + Ba(OH)_2 ⟶ 2 KOH + BaSO_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 K_2SO_4 | 1 | -1 Ba(OH)_2 | 1 | -1 KOH | 2 | 2 BaSO_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 K_2SO_4 | 1 | -1 | -(Δ[K2SO4])/(Δt) Ba(OH)_2 | 1 | -1 | -(Δ[Ba(OH)2])/(Δt) KOH | 2 | 2 | 1/2 (Δ[KOH])/(Δt) BaSO_4 | 1 | 1 | (Δ[BaSO4])/(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 = -(Δ[K2SO4])/(Δt) = -(Δ[Ba(OH)2])/(Δt) = 1/2 (Δ[KOH])/(Δt) = (Δ[BaSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| potassium sulfate | barium hydroxide | potassium hydroxide | barium sulfate formula | K_2SO_4 | Ba(OH)_2 | KOH | BaSO_4 Hill formula | K_2O_4S | BaH_2O_2 | HKO | BaO_4S name | potassium sulfate | barium hydroxide | potassium hydroxide | barium sulfate IUPAC name | dipotassium sulfate | barium(+2) cation dihydroxide | potassium hydroxide | barium(+2) cation sulfate
| potassium sulfate | barium hydroxide | potassium hydroxide | barium sulfate formula | K_2SO_4 | Ba(OH)_2 | KOH | BaSO_4 Hill formula | K_2O_4S | BaH_2O_2 | HKO | BaO_4S name | potassium sulfate | barium hydroxide | potassium hydroxide | barium sulfate IUPAC name | dipotassium sulfate | barium(+2) cation dihydroxide | potassium hydroxide | barium(+2) cation sulfate

Substance properties

| potassium sulfate | barium hydroxide | potassium hydroxide | barium sulfate molar mass | 174.25 g/mol | 171.34 g/mol | 56.105 g/mol | 233.38 g/mol phase | | solid (at STP) | solid (at STP) | solid (at STP) melting point | | 300 °C | 406 °C | 1345 °C boiling point | | | 1327 °C | density | | 2.2 g/cm^3 | 2.044 g/cm^3 | 4.5 g/cm^3 solubility in water | soluble | | soluble | insoluble dynamic viscosity | | | 0.001 Pa s (at 550 °C) |
| potassium sulfate | barium hydroxide | potassium hydroxide | barium sulfate molar mass | 174.25 g/mol | 171.34 g/mol | 56.105 g/mol | 233.38 g/mol phase | | solid (at STP) | solid (at STP) | solid (at STP) melting point | | 300 °C | 406 °C | 1345 °C boiling point | | | 1327 °C | density | | 2.2 g/cm^3 | 2.044 g/cm^3 | 4.5 g/cm^3 solubility in water | soluble | | soluble | insoluble dynamic viscosity | | | 0.001 Pa s (at 550 °C) |

Units

Random Queries

electronic configuration of actinides
alternate names of nitride anion vs oxide anion
specific heat at STP of alkaline earth metals
alternate names of tin(IV) bromide
DOT numbers of calcium nitrate vs hydrogen chloride
edge types of stannic chloride
bonding characteristics of protactinium
CAS number of platinum(II) bromide vs 2-bromo-3-methyl-2-butene
handwritten style uranium(VI) cation
NaOH + SnCl2 = NaCl + Sn(OH)2