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NaOH + NiCl2 = NaCl + Ni(OH)2

Input interpretation

NaOH sodium hydroxide + NiCl_2 nickel(II) chloride ⟶ NaCl sodium chloride + Ni(OH)_2 nickel(II) hydroxide
NaOH sodium hydroxide + NiCl_2 nickel(II) chloride ⟶ NaCl sodium chloride + Ni(OH)_2 nickel(II) hydroxide

Balanced equation

Balance the chemical equation algebraically: NaOH + NiCl_2 ⟶ NaCl + Ni(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 NiCl_2 ⟶ c_3 NaCl + c_4 Ni(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Cl and Ni: H: | c_1 = 2 c_4 Na: | c_1 = c_3 O: | c_1 = 2 c_4 Cl: | 2 c_2 = c_3 Ni: | 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 NaOH + NiCl_2 ⟶ 2 NaCl + Ni(OH)_2
Balance the chemical equation algebraically: NaOH + NiCl_2 ⟶ NaCl + Ni(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 NiCl_2 ⟶ c_3 NaCl + c_4 Ni(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Cl and Ni: H: | c_1 = 2 c_4 Na: | c_1 = c_3 O: | c_1 = 2 c_4 Cl: | 2 c_2 = c_3 Ni: | 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 NaOH + NiCl_2 ⟶ 2 NaCl + Ni(OH)_2

Structures

+ ⟶ +
+ ⟶ +

Names

sodium hydroxide + nickel(II) chloride ⟶ sodium chloride + nickel(II) hydroxide
sodium hydroxide + nickel(II) chloride ⟶ sodium chloride + nickel(II) hydroxide

Equilibrium constant

Construct the equilibrium constant, K, expression for: NaOH + NiCl_2 ⟶ NaCl + 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 NaOH + NiCl_2 ⟶ 2 NaCl + 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 NaOH | 2 | -2 NiCl_2 | 1 | -1 NaCl | 2 | 2 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 NaOH | 2 | -2 | ([NaOH])^(-2) NiCl_2 | 1 | -1 | ([NiCl2])^(-1) NaCl | 2 | 2 | ([NaCl])^2 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 = ([NaOH])^(-2) ([NiCl2])^(-1) ([NaCl])^2 [Ni(OH)2] = (([NaCl])^2 [Ni(OH)2])/(([NaOH])^2 [NiCl2])
Construct the equilibrium constant, K, expression for: NaOH + NiCl_2 ⟶ NaCl + 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 NaOH + NiCl_2 ⟶ 2 NaCl + 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 NaOH | 2 | -2 NiCl_2 | 1 | -1 NaCl | 2 | 2 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 NaOH | 2 | -2 | ([NaOH])^(-2) NiCl_2 | 1 | -1 | ([NiCl2])^(-1) NaCl | 2 | 2 | ([NaCl])^2 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 = ([NaOH])^(-2) ([NiCl2])^(-1) ([NaCl])^2 [Ni(OH)2] = (([NaCl])^2 [Ni(OH)2])/(([NaOH])^2 [NiCl2])

Rate of reaction

Construct the rate of reaction expression for: NaOH + NiCl_2 ⟶ NaCl + 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 NaOH + NiCl_2 ⟶ 2 NaCl + 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 NaOH | 2 | -2 NiCl_2 | 1 | -1 NaCl | 2 | 2 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 NaOH | 2 | -2 | -1/2 (Δ[NaOH])/(Δt) NiCl_2 | 1 | -1 | -(Δ[NiCl2])/(Δt) NaCl | 2 | 2 | 1/2 (Δ[NaCl])/(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[NaOH])/(Δt) = -(Δ[NiCl2])/(Δt) = 1/2 (Δ[NaCl])/(Δt) = (Δ[Ni(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NaOH + NiCl_2 ⟶ NaCl + 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 NaOH + NiCl_2 ⟶ 2 NaCl + 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 NaOH | 2 | -2 NiCl_2 | 1 | -1 NaCl | 2 | 2 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 NaOH | 2 | -2 | -1/2 (Δ[NaOH])/(Δt) NiCl_2 | 1 | -1 | -(Δ[NiCl2])/(Δt) NaCl | 2 | 2 | 1/2 (Δ[NaCl])/(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[NaOH])/(Δt) = -(Δ[NiCl2])/(Δt) = 1/2 (Δ[NaCl])/(Δt) = (Δ[Ni(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sodium hydroxide | nickel(II) chloride | sodium chloride | nickel(II) hydroxide formula | NaOH | NiCl_2 | NaCl | Ni(OH)_2 Hill formula | HNaO | Cl_2Ni | ClNa | H_2NiO_2 name | sodium hydroxide | nickel(II) chloride | sodium chloride | nickel(II) hydroxide IUPAC name | sodium hydroxide | dichloronickel | sodium chloride |
| sodium hydroxide | nickel(II) chloride | sodium chloride | nickel(II) hydroxide formula | NaOH | NiCl_2 | NaCl | Ni(OH)_2 Hill formula | HNaO | Cl_2Ni | ClNa | H_2NiO_2 name | sodium hydroxide | nickel(II) chloride | sodium chloride | nickel(II) hydroxide IUPAC name | sodium hydroxide | dichloronickel | sodium chloride |

Substance properties

| sodium hydroxide | nickel(II) chloride | sodium chloride | nickel(II) hydroxide molar mass | 39.997 g/mol | 129.6 g/mol | 58.44 g/mol | 92.707 g/mol phase | solid (at STP) | | solid (at STP) | melting point | 323 °C | | 801 °C | boiling point | 1390 °C | | 1413 °C | density | 2.13 g/cm^3 | 3.55 g/cm^3 | 2.16 g/cm^3 | solubility in water | soluble | | soluble | surface tension | 0.07435 N/m | | | dynamic viscosity | 0.004 Pa s (at 350 °C) | | | odor | | | odorless |
| sodium hydroxide | nickel(II) chloride | sodium chloride | nickel(II) hydroxide molar mass | 39.997 g/mol | 129.6 g/mol | 58.44 g/mol | 92.707 g/mol phase | solid (at STP) | | solid (at STP) | melting point | 323 °C | | 801 °C | boiling point | 1390 °C | | 1413 °C | density | 2.13 g/cm^3 | 3.55 g/cm^3 | 2.16 g/cm^3 | solubility in water | soluble | | soluble | surface tension | 0.07435 N/m | | | dynamic viscosity | 0.004 Pa s (at 350 °C) | | | odor | | | odorless |

Units

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