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HCl + NaAlO2 = NaCl + [Al(H2O)2]Cl3

Input interpretation

HCl hydrogen chloride + AlNaO_2 sodium aluminate ⟶ NaCl sodium chloride + Al(H2O)2Cl3
HCl hydrogen chloride + AlNaO_2 sodium aluminate ⟶ NaCl sodium chloride + Al(H2O)2Cl3

Balanced equation

Balance the chemical equation algebraically: HCl + AlNaO_2 ⟶ NaCl + Al(H2O)2Cl3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 AlNaO_2 ⟶ c_3 NaCl + c_4 Al(H2O)2Cl3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Al, Na and O: Cl: | c_1 = c_3 + 3 c_4 H: | c_1 = 4 c_4 Al: | c_2 = c_4 Na: | c_2 = c_3 O: | 2 c_2 = 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 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 HCl + AlNaO_2 ⟶ NaCl + Al(H2O)2Cl3
Balance the chemical equation algebraically: HCl + AlNaO_2 ⟶ NaCl + Al(H2O)2Cl3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 AlNaO_2 ⟶ c_3 NaCl + c_4 Al(H2O)2Cl3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Al, Na and O: Cl: | c_1 = c_3 + 3 c_4 H: | c_1 = 4 c_4 Al: | c_2 = c_4 Na: | c_2 = c_3 O: | 2 c_2 = 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 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 4 HCl + AlNaO_2 ⟶ NaCl + Al(H2O)2Cl3

Structures

+ ⟶ + Al(H2O)2Cl3
+ ⟶ + Al(H2O)2Cl3

Names

hydrogen chloride + sodium aluminate ⟶ sodium chloride + Al(H2O)2Cl3
hydrogen chloride + sodium aluminate ⟶ sodium chloride + Al(H2O)2Cl3

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + AlNaO_2 ⟶ NaCl + Al(H2O)2Cl3 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 + AlNaO_2 ⟶ NaCl + Al(H2O)2Cl3 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 AlNaO_2 | 1 | -1 NaCl | 1 | 1 Al(H2O)2Cl3 | 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) AlNaO_2 | 1 | -1 | ([AlNaO2])^(-1) NaCl | 1 | 1 | [NaCl] Al(H2O)2Cl3 | 1 | 1 | [Al(H2O)2Cl3] 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) ([AlNaO2])^(-1) [NaCl] [Al(H2O)2Cl3] = ([NaCl] [Al(H2O)2Cl3])/(([HCl])^4 [AlNaO2])
Construct the equilibrium constant, K, expression for: HCl + AlNaO_2 ⟶ NaCl + Al(H2O)2Cl3 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 + AlNaO_2 ⟶ NaCl + Al(H2O)2Cl3 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 AlNaO_2 | 1 | -1 NaCl | 1 | 1 Al(H2O)2Cl3 | 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) AlNaO_2 | 1 | -1 | ([AlNaO2])^(-1) NaCl | 1 | 1 | [NaCl] Al(H2O)2Cl3 | 1 | 1 | [Al(H2O)2Cl3] 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) ([AlNaO2])^(-1) [NaCl] [Al(H2O)2Cl3] = ([NaCl] [Al(H2O)2Cl3])/(([HCl])^4 [AlNaO2])

Rate of reaction

Construct the rate of reaction expression for: HCl + AlNaO_2 ⟶ NaCl + Al(H2O)2Cl3 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 + AlNaO_2 ⟶ NaCl + Al(H2O)2Cl3 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 AlNaO_2 | 1 | -1 NaCl | 1 | 1 Al(H2O)2Cl3 | 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) AlNaO_2 | 1 | -1 | -(Δ[AlNaO2])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(Δt) Al(H2O)2Cl3 | 1 | 1 | (Δ[Al(H2O)2Cl3])/(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[AlNaO2])/(Δt) = (Δ[NaCl])/(Δt) = (Δ[Al(H2O)2Cl3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + AlNaO_2 ⟶ NaCl + Al(H2O)2Cl3 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 + AlNaO_2 ⟶ NaCl + Al(H2O)2Cl3 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 AlNaO_2 | 1 | -1 NaCl | 1 | 1 Al(H2O)2Cl3 | 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) AlNaO_2 | 1 | -1 | -(Δ[AlNaO2])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(Δt) Al(H2O)2Cl3 | 1 | 1 | (Δ[Al(H2O)2Cl3])/(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[AlNaO2])/(Δt) = (Δ[NaCl])/(Δt) = (Δ[Al(H2O)2Cl3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | sodium aluminate | sodium chloride | Al(H2O)2Cl3 formula | HCl | AlNaO_2 | NaCl | Al(H2O)2Cl3 Hill formula | ClH | AlNaO_2 | ClNa | H4AlCl3O2 name | hydrogen chloride | sodium aluminate | sodium chloride | IUPAC name | hydrogen chloride | sodium oxido-oxo-alumane | sodium chloride |
| hydrogen chloride | sodium aluminate | sodium chloride | Al(H2O)2Cl3 formula | HCl | AlNaO_2 | NaCl | Al(H2O)2Cl3 Hill formula | ClH | AlNaO_2 | ClNa | H4AlCl3O2 name | hydrogen chloride | sodium aluminate | sodium chloride | IUPAC name | hydrogen chloride | sodium oxido-oxo-alumane | sodium chloride |

Substance properties

| hydrogen chloride | sodium aluminate | sodium chloride | Al(H2O)2Cl3 molar mass | 36.46 g/mol | 81.969 g/mol | 58.44 g/mol | 169.4 g/mol phase | gas (at STP) | solid (at STP) | solid (at STP) | melting point | -114.17 °C | 1800 °C | 801 °C | boiling point | -85 °C | | 1413 °C | density | 0.00149 g/cm^3 (at 25 °C) | 1.5 g/cm^3 | 2.16 g/cm^3 | solubility in water | miscible | soluble | soluble | odor | | | odorless |
| hydrogen chloride | sodium aluminate | sodium chloride | Al(H2O)2Cl3 molar mass | 36.46 g/mol | 81.969 g/mol | 58.44 g/mol | 169.4 g/mol phase | gas (at STP) | solid (at STP) | solid (at STP) | melting point | -114.17 °C | 1800 °C | 801 °C | boiling point | -85 °C | | 1413 °C | density | 0.00149 g/cm^3 (at 25 °C) | 1.5 g/cm^3 | 2.16 g/cm^3 | solubility in water | miscible | soluble | soluble | odor | | | odorless |

Units

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