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HCl + Na[Al(OH)4] = H2O + NaCl + AlCl3

Input interpretation

HCl hydrogen chloride + NaAl(OH)4 ⟶ H_2O water + NaCl sodium chloride + AlCl_3 aluminum chloride
HCl hydrogen chloride + NaAl(OH)4 ⟶ H_2O water + NaCl sodium chloride + AlCl_3 aluminum chloride

Balanced equation

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

Structures

+ NaAl(OH)4 ⟶ + +
+ NaAl(OH)4 ⟶ + +

Names

hydrogen chloride + NaAl(OH)4 ⟶ water + sodium chloride + aluminum chloride
hydrogen chloride + NaAl(OH)4 ⟶ water + sodium chloride + aluminum chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + NaAl(OH)4 ⟶ H_2O + NaCl + AlCl_3 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 HCl + NaAl(OH)4 ⟶ 4 H_2O + NaCl + AlCl_3 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 HCl | 4 | -4 NaAl(OH)4 | 1 | -1 H_2O | 4 | 4 NaCl | 1 | 1 AlCl_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 4 | -4 | ([HCl])^(-4) NaAl(OH)4 | 1 | -1 | ([NaAl(OH)4])^(-1) H_2O | 4 | 4 | ([H2O])^4 NaCl | 1 | 1 | [NaCl] AlCl_3 | 1 | 1 | [AlCl3] 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 = ([HCl])^(-4) ([NaAl(OH)4])^(-1) ([H2O])^4 [NaCl] [AlCl3] = (([H2O])^4 [NaCl] [AlCl3])/(([HCl])^4 [NaAl(OH)4])
Construct the equilibrium constant, K, expression for: HCl + NaAl(OH)4 ⟶ H_2O + NaCl + AlCl_3 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 HCl + NaAl(OH)4 ⟶ 4 H_2O + NaCl + AlCl_3 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 HCl | 4 | -4 NaAl(OH)4 | 1 | -1 H_2O | 4 | 4 NaCl | 1 | 1 AlCl_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 4 | -4 | ([HCl])^(-4) NaAl(OH)4 | 1 | -1 | ([NaAl(OH)4])^(-1) H_2O | 4 | 4 | ([H2O])^4 NaCl | 1 | 1 | [NaCl] AlCl_3 | 1 | 1 | [AlCl3] 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 = ([HCl])^(-4) ([NaAl(OH)4])^(-1) ([H2O])^4 [NaCl] [AlCl3] = (([H2O])^4 [NaCl] [AlCl3])/(([HCl])^4 [NaAl(OH)4])

Rate of reaction

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

Chemical names and formulas

| hydrogen chloride | NaAl(OH)4 | water | sodium chloride | aluminum chloride formula | HCl | NaAl(OH)4 | H_2O | NaCl | AlCl_3 Hill formula | ClH | H4AlNaO4 | H_2O | ClNa | AlCl_3 name | hydrogen chloride | | water | sodium chloride | aluminum chloride IUPAC name | hydrogen chloride | | water | sodium chloride | trichloroalumane
| hydrogen chloride | NaAl(OH)4 | water | sodium chloride | aluminum chloride formula | HCl | NaAl(OH)4 | H_2O | NaCl | AlCl_3 Hill formula | ClH | H4AlNaO4 | H_2O | ClNa | AlCl_3 name | hydrogen chloride | | water | sodium chloride | aluminum chloride IUPAC name | hydrogen chloride | | water | sodium chloride | trichloroalumane

Substance properties

| hydrogen chloride | NaAl(OH)4 | water | sodium chloride | aluminum chloride molar mass | 36.46 g/mol | 118 g/mol | 18.015 g/mol | 58.44 g/mol | 133.3 g/mol phase | gas (at STP) | | liquid (at STP) | solid (at STP) | solid (at STP) melting point | -114.17 °C | | 0 °C | 801 °C | 190 °C boiling point | -85 °C | | 99.9839 °C | 1413 °C | density | 0.00149 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 2.16 g/cm^3 | solubility in water | miscible | | | soluble | surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | odorless |
| hydrogen chloride | NaAl(OH)4 | water | sodium chloride | aluminum chloride molar mass | 36.46 g/mol | 118 g/mol | 18.015 g/mol | 58.44 g/mol | 133.3 g/mol phase | gas (at STP) | | liquid (at STP) | solid (at STP) | solid (at STP) melting point | -114.17 °C | | 0 °C | 801 °C | 190 °C boiling point | -85 °C | | 99.9839 °C | 1413 °C | density | 0.00149 g/cm^3 (at 25 °C) | | 1 g/cm^3 | 2.16 g/cm^3 | solubility in water | miscible | | | soluble | surface tension | | | 0.0728 N/m | | dynamic viscosity | | | 8.9×10^-4 Pa s (at 25 °C) | | odor | | | odorless | odorless |

Units

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