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NaOH + AlCl3 = H2O + NaCl + NaAlO2

Input interpretation

NaOH sodium hydroxide + AlCl_3 aluminum chloride ⟶ H_2O water + NaCl sodium chloride + AlNaO_2 sodium aluminate
NaOH sodium hydroxide + AlCl_3 aluminum chloride ⟶ H_2O water + NaCl sodium chloride + AlNaO_2 sodium aluminate

Balanced equation

Balance the chemical equation algebraically: NaOH + AlCl_3 ⟶ H_2O + NaCl + AlNaO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 AlCl_3 ⟶ c_3 H_2O + c_4 NaCl + c_5 AlNaO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Al and Cl: H: | c_1 = 2 c_3 Na: | c_1 = c_4 + c_5 O: | c_1 = c_3 + 2 c_5 Al: | c_2 = c_5 Cl: | 3 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 = 4 c_2 = 1 c_3 = 2 c_4 = 3 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 NaOH + AlCl_3 ⟶ 2 H_2O + 3 NaCl + AlNaO_2
Balance the chemical equation algebraically: NaOH + AlCl_3 ⟶ H_2O + NaCl + AlNaO_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 AlCl_3 ⟶ c_3 H_2O + c_4 NaCl + c_5 AlNaO_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Al and Cl: H: | c_1 = 2 c_3 Na: | c_1 = c_4 + c_5 O: | c_1 = c_3 + 2 c_5 Al: | c_2 = c_5 Cl: | 3 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 = 4 c_2 = 1 c_3 = 2 c_4 = 3 c_5 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 NaOH + AlCl_3 ⟶ 2 H_2O + 3 NaCl + AlNaO_2

Structures

+ ⟶ + +
+ ⟶ + +

Names

sodium hydroxide + aluminum chloride ⟶ water + sodium chloride + sodium aluminate
sodium hydroxide + aluminum chloride ⟶ water + sodium chloride + sodium aluminate

Equilibrium constant

Construct the equilibrium constant, K, expression for: NaOH + AlCl_3 ⟶ H_2O + NaCl + AlNaO_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: 4 NaOH + AlCl_3 ⟶ 2 H_2O + 3 NaCl + AlNaO_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 | 4 | -4 AlCl_3 | 1 | -1 H_2O | 2 | 2 NaCl | 3 | 3 AlNaO_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 | 4 | -4 | ([NaOH])^(-4) AlCl_3 | 1 | -1 | ([AlCl3])^(-1) H_2O | 2 | 2 | ([H2O])^2 NaCl | 3 | 3 | ([NaCl])^3 AlNaO_2 | 1 | 1 | [AlNaO2] 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])^(-4) ([AlCl3])^(-1) ([H2O])^2 ([NaCl])^3 [AlNaO2] = (([H2O])^2 ([NaCl])^3 [AlNaO2])/(([NaOH])^4 [AlCl3])
Construct the equilibrium constant, K, expression for: NaOH + AlCl_3 ⟶ H_2O + NaCl + AlNaO_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: 4 NaOH + AlCl_3 ⟶ 2 H_2O + 3 NaCl + AlNaO_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 | 4 | -4 AlCl_3 | 1 | -1 H_2O | 2 | 2 NaCl | 3 | 3 AlNaO_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 | 4 | -4 | ([NaOH])^(-4) AlCl_3 | 1 | -1 | ([AlCl3])^(-1) H_2O | 2 | 2 | ([H2O])^2 NaCl | 3 | 3 | ([NaCl])^3 AlNaO_2 | 1 | 1 | [AlNaO2] 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])^(-4) ([AlCl3])^(-1) ([H2O])^2 ([NaCl])^3 [AlNaO2] = (([H2O])^2 ([NaCl])^3 [AlNaO2])/(([NaOH])^4 [AlCl3])

Rate of reaction

Construct the rate of reaction expression for: NaOH + AlCl_3 ⟶ H_2O + NaCl + AlNaO_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: 4 NaOH + AlCl_3 ⟶ 2 H_2O + 3 NaCl + AlNaO_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 | 4 | -4 AlCl_3 | 1 | -1 H_2O | 2 | 2 NaCl | 3 | 3 AlNaO_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 | 4 | -4 | -1/4 (Δ[NaOH])/(Δt) AlCl_3 | 1 | -1 | -(Δ[AlCl3])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NaCl | 3 | 3 | 1/3 (Δ[NaCl])/(Δt) AlNaO_2 | 1 | 1 | (Δ[AlNaO2])/(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 = -1/4 (Δ[NaOH])/(Δt) = -(Δ[AlCl3])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/3 (Δ[NaCl])/(Δt) = (Δ[AlNaO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NaOH + AlCl_3 ⟶ H_2O + NaCl + AlNaO_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: 4 NaOH + AlCl_3 ⟶ 2 H_2O + 3 NaCl + AlNaO_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 | 4 | -4 AlCl_3 | 1 | -1 H_2O | 2 | 2 NaCl | 3 | 3 AlNaO_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 | 4 | -4 | -1/4 (Δ[NaOH])/(Δt) AlCl_3 | 1 | -1 | -(Δ[AlCl3])/(Δt) H_2O | 2 | 2 | 1/2 (Δ[H2O])/(Δt) NaCl | 3 | 3 | 1/3 (Δ[NaCl])/(Δt) AlNaO_2 | 1 | 1 | (Δ[AlNaO2])/(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 = -1/4 (Δ[NaOH])/(Δt) = -(Δ[AlCl3])/(Δt) = 1/2 (Δ[H2O])/(Δt) = 1/3 (Δ[NaCl])/(Δt) = (Δ[AlNaO2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sodium hydroxide | aluminum chloride | water | sodium chloride | sodium aluminate formula | NaOH | AlCl_3 | H_2O | NaCl | AlNaO_2 Hill formula | HNaO | AlCl_3 | H_2O | ClNa | AlNaO_2 name | sodium hydroxide | aluminum chloride | water | sodium chloride | sodium aluminate IUPAC name | sodium hydroxide | trichloroalumane | water | sodium chloride | sodium oxido-oxo-alumane
| sodium hydroxide | aluminum chloride | water | sodium chloride | sodium aluminate formula | NaOH | AlCl_3 | H_2O | NaCl | AlNaO_2 Hill formula | HNaO | AlCl_3 | H_2O | ClNa | AlNaO_2 name | sodium hydroxide | aluminum chloride | water | sodium chloride | sodium aluminate IUPAC name | sodium hydroxide | trichloroalumane | water | sodium chloride | sodium oxido-oxo-alumane

Substance properties

| sodium hydroxide | aluminum chloride | water | sodium chloride | sodium aluminate molar mass | 39.997 g/mol | 133.3 g/mol | 18.015 g/mol | 58.44 g/mol | 81.969 g/mol phase | solid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 323 °C | 190 °C | 0 °C | 801 °C | 1800 °C boiling point | 1390 °C | | 99.9839 °C | 1413 °C | density | 2.13 g/cm^3 | | 1 g/cm^3 | 2.16 g/cm^3 | 1.5 g/cm^3 solubility in water | soluble | | | soluble | soluble surface tension | 0.07435 N/m | | 0.0728 N/m | | dynamic viscosity | 0.004 Pa s (at 350 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | odorless |
| sodium hydroxide | aluminum chloride | water | sodium chloride | sodium aluminate molar mass | 39.997 g/mol | 133.3 g/mol | 18.015 g/mol | 58.44 g/mol | 81.969 g/mol phase | solid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) | solid (at STP) melting point | 323 °C | 190 °C | 0 °C | 801 °C | 1800 °C boiling point | 1390 °C | | 99.9839 °C | 1413 °C | density | 2.13 g/cm^3 | | 1 g/cm^3 | 2.16 g/cm^3 | 1.5 g/cm^3 solubility in water | soluble | | | soluble | soluble surface tension | 0.07435 N/m | | 0.0728 N/m | | dynamic viscosity | 0.004 Pa s (at 350 °C) | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | odorless |

Units

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