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NH4OH + NiSO4 = (NH4)2SO4 + Ni(OH)2

Input interpretation

NH_4OH ammonium hydroxide + NiSO_4 nickel(II) sulfate ⟶ (NH_4)_2SO_4 ammonium sulfate + Ni(OH)_2 nickel(II) hydroxide
NH_4OH ammonium hydroxide + NiSO_4 nickel(II) sulfate ⟶ (NH_4)_2SO_4 ammonium sulfate + Ni(OH)_2 nickel(II) hydroxide

Balanced equation

Balance the chemical equation algebraically: NH_4OH + NiSO_4 ⟶ (NH_4)_2SO_4 + Ni(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NH_4OH + c_2 NiSO_4 ⟶ c_3 (NH_4)_2SO_4 + c_4 Ni(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, Ni and S: H: | 5 c_1 = 8 c_3 + 2 c_4 N: | c_1 = 2 c_3 O: | c_1 + 4 c_2 = 4 c_3 + 2 c_4 Ni: | 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 NH_4OH + NiSO_4 ⟶ (NH_4)_2SO_4 + Ni(OH)_2
Balance the chemical equation algebraically: NH_4OH + NiSO_4 ⟶ (NH_4)_2SO_4 + Ni(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NH_4OH + c_2 NiSO_4 ⟶ c_3 (NH_4)_2SO_4 + c_4 Ni(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, N, O, Ni and S: H: | 5 c_1 = 8 c_3 + 2 c_4 N: | c_1 = 2 c_3 O: | c_1 + 4 c_2 = 4 c_3 + 2 c_4 Ni: | 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 NH_4OH + NiSO_4 ⟶ (NH_4)_2SO_4 + Ni(OH)_2

Structures

+ ⟶ +
+ ⟶ +

Names

ammonium hydroxide + nickel(II) sulfate ⟶ ammonium sulfate + nickel(II) hydroxide
ammonium hydroxide + nickel(II) sulfate ⟶ ammonium sulfate + nickel(II) hydroxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: NH_4OH + NiSO_4 ⟶ (NH_4)_2SO_4 + Ni(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 NH_4OH + NiSO_4 ⟶ (NH_4)_2SO_4 + Ni(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 NH_4OH | 2 | -2 NiSO_4 | 1 | -1 (NH_4)_2SO_4 | 1 | 1 Ni(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 NH_4OH | 2 | -2 | ([NH4OH])^(-2) NiSO_4 | 1 | -1 | ([NiSO4])^(-1) (NH_4)_2SO_4 | 1 | 1 | [(NH4)2SO4] Ni(OH)_2 | 1 | 1 | [Ni(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 = ([NH4OH])^(-2) ([NiSO4])^(-1) [(NH4)2SO4] [Ni(OH)2] = ([(NH4)2SO4] [Ni(OH)2])/(([NH4OH])^2 [NiSO4])
Construct the equilibrium constant, K, expression for: NH_4OH + NiSO_4 ⟶ (NH_4)_2SO_4 + Ni(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 NH_4OH + NiSO_4 ⟶ (NH_4)_2SO_4 + Ni(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 NH_4OH | 2 | -2 NiSO_4 | 1 | -1 (NH_4)_2SO_4 | 1 | 1 Ni(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 NH_4OH | 2 | -2 | ([NH4OH])^(-2) NiSO_4 | 1 | -1 | ([NiSO4])^(-1) (NH_4)_2SO_4 | 1 | 1 | [(NH4)2SO4] Ni(OH)_2 | 1 | 1 | [Ni(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 = ([NH4OH])^(-2) ([NiSO4])^(-1) [(NH4)2SO4] [Ni(OH)2] = ([(NH4)2SO4] [Ni(OH)2])/(([NH4OH])^2 [NiSO4])

Rate of reaction

Construct the rate of reaction expression for: NH_4OH + NiSO_4 ⟶ (NH_4)_2SO_4 + Ni(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 NH_4OH + NiSO_4 ⟶ (NH_4)_2SO_4 + Ni(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 NH_4OH | 2 | -2 NiSO_4 | 1 | -1 (NH_4)_2SO_4 | 1 | 1 Ni(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 NH_4OH | 2 | -2 | -1/2 (Δ[NH4OH])/(Δt) NiSO_4 | 1 | -1 | -(Δ[NiSO4])/(Δt) (NH_4)_2SO_4 | 1 | 1 | (Δ[(NH4)2SO4])/(Δt) Ni(OH)_2 | 1 | 1 | (Δ[Ni(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[NH4OH])/(Δt) = -(Δ[NiSO4])/(Δt) = (Δ[(NH4)2SO4])/(Δt) = (Δ[Ni(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NH_4OH + NiSO_4 ⟶ (NH_4)_2SO_4 + Ni(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 NH_4OH + NiSO_4 ⟶ (NH_4)_2SO_4 + Ni(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 NH_4OH | 2 | -2 NiSO_4 | 1 | -1 (NH_4)_2SO_4 | 1 | 1 Ni(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 NH_4OH | 2 | -2 | -1/2 (Δ[NH4OH])/(Δt) NiSO_4 | 1 | -1 | -(Δ[NiSO4])/(Δt) (NH_4)_2SO_4 | 1 | 1 | (Δ[(NH4)2SO4])/(Δt) Ni(OH)_2 | 1 | 1 | (Δ[Ni(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[NH4OH])/(Δt) = -(Δ[NiSO4])/(Δt) = (Δ[(NH4)2SO4])/(Δt) = (Δ[Ni(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| ammonium hydroxide | nickel(II) sulfate | ammonium sulfate | nickel(II) hydroxide formula | NH_4OH | NiSO_4 | (NH_4)_2SO_4 | Ni(OH)_2 Hill formula | H_5NO | NiO_4S | H_8N_2O_4S | H_2NiO_2 name | ammonium hydroxide | nickel(II) sulfate | ammonium sulfate | nickel(II) hydroxide IUPAC name | ammonium hydroxide | nickelous sulfate | |
| ammonium hydroxide | nickel(II) sulfate | ammonium sulfate | nickel(II) hydroxide formula | NH_4OH | NiSO_4 | (NH_4)_2SO_4 | Ni(OH)_2 Hill formula | H_5NO | NiO_4S | H_8N_2O_4S | H_2NiO_2 name | ammonium hydroxide | nickel(II) sulfate | ammonium sulfate | nickel(II) hydroxide IUPAC name | ammonium hydroxide | nickelous sulfate | |

Substance properties

| ammonium hydroxide | nickel(II) sulfate | ammonium sulfate | nickel(II) hydroxide molar mass | 35.046 g/mol | 154.75 g/mol | 132.1 g/mol | 92.707 g/mol phase | aqueous (at STP) | solid (at STP) | solid (at STP) | melting point | -57.5 °C | | 280 °C | boiling point | 36 °C | | | density | 0.9 g/cm^3 | 4.01 g/cm^3 | 1.77 g/cm^3 | solubility in water | very soluble | | | odor | | | odorless |
| ammonium hydroxide | nickel(II) sulfate | ammonium sulfate | nickel(II) hydroxide molar mass | 35.046 g/mol | 154.75 g/mol | 132.1 g/mol | 92.707 g/mol phase | aqueous (at STP) | solid (at STP) | solid (at STP) | melting point | -57.5 °C | | 280 °C | boiling point | 36 °C | | | density | 0.9 g/cm^3 | 4.01 g/cm^3 | 1.77 g/cm^3 | solubility in water | very soluble | | | odor | | | odorless |

Units

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