Input interpretation
![Al(OH)_3 aluminum hydroxide + CH_3CO_2H acetic acid ⟶ H_2O water + (CH3COO)3Al](../image_source/23a90daa2639f0059cfaca03efb5b107.png)
Al(OH)_3 aluminum hydroxide + CH_3CO_2H acetic acid ⟶ H_2O water + (CH3COO)3Al
Balanced equation
![Balance the chemical equation algebraically: Al(OH)_3 + CH_3CO_2H ⟶ H_2O + (CH3COO)3Al Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Al(OH)_3 + c_2 CH_3CO_2H ⟶ c_3 H_2O + c_4 (CH3COO)3Al Set the number of atoms in the reactants equal to the number of atoms in the products for Al, H, O and C: Al: | c_1 = c_4 H: | 3 c_1 + 4 c_2 = 2 c_3 + 9 c_4 O: | 3 c_1 + 2 c_2 = c_3 + 6 c_4 C: | 2 c_2 = 6 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 3 c_3 = 3 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Al(OH)_3 + 3 CH_3CO_2H ⟶ 3 H_2O + (CH3COO)3Al](../image_source/39b210144294719f4950c08e96dfab3f.png)
Balance the chemical equation algebraically: Al(OH)_3 + CH_3CO_2H ⟶ H_2O + (CH3COO)3Al Add stoichiometric coefficients, c_i, to the reactants and products: c_1 Al(OH)_3 + c_2 CH_3CO_2H ⟶ c_3 H_2O + c_4 (CH3COO)3Al Set the number of atoms in the reactants equal to the number of atoms in the products for Al, H, O and C: Al: | c_1 = c_4 H: | 3 c_1 + 4 c_2 = 2 c_3 + 9 c_4 O: | 3 c_1 + 2 c_2 = c_3 + 6 c_4 C: | 2 c_2 = 6 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 3 c_3 = 3 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | Al(OH)_3 + 3 CH_3CO_2H ⟶ 3 H_2O + (CH3COO)3Al
Structures
![+ ⟶ + (CH3COO)3Al](../image_source/db1fb6db2f562073349a698bf221e2b1.png)
+ ⟶ + (CH3COO)3Al
Names
![aluminum hydroxide + acetic acid ⟶ water + (CH3COO)3Al](../image_source/8b2a9716039df88d7b77eecb7ded9421.png)
aluminum hydroxide + acetic acid ⟶ water + (CH3COO)3Al
Equilibrium constant
![Construct the equilibrium constant, K, expression for: Al(OH)_3 + CH_3CO_2H ⟶ H_2O + (CH3COO)3Al 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: Al(OH)_3 + 3 CH_3CO_2H ⟶ 3 H_2O + (CH3COO)3Al 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 Al(OH)_3 | 1 | -1 CH_3CO_2H | 3 | -3 H_2O | 3 | 3 (CH3COO)3Al | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Al(OH)_3 | 1 | -1 | ([Al(OH)3])^(-1) CH_3CO_2H | 3 | -3 | ([CH3CO2H])^(-3) H_2O | 3 | 3 | ([H2O])^3 (CH3COO)3Al | 1 | 1 | [(CH3COO)3Al] 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 = ([Al(OH)3])^(-1) ([CH3CO2H])^(-3) ([H2O])^3 [(CH3COO)3Al] = (([H2O])^3 [(CH3COO)3Al])/([Al(OH)3] ([CH3CO2H])^3)](../image_source/9dc7da6945a0199bbf27706598a2d8f7.png)
Construct the equilibrium constant, K, expression for: Al(OH)_3 + CH_3CO_2H ⟶ H_2O + (CH3COO)3Al 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: Al(OH)_3 + 3 CH_3CO_2H ⟶ 3 H_2O + (CH3COO)3Al 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 Al(OH)_3 | 1 | -1 CH_3CO_2H | 3 | -3 H_2O | 3 | 3 (CH3COO)3Al | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression Al(OH)_3 | 1 | -1 | ([Al(OH)3])^(-1) CH_3CO_2H | 3 | -3 | ([CH3CO2H])^(-3) H_2O | 3 | 3 | ([H2O])^3 (CH3COO)3Al | 1 | 1 | [(CH3COO)3Al] 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 = ([Al(OH)3])^(-1) ([CH3CO2H])^(-3) ([H2O])^3 [(CH3COO)3Al] = (([H2O])^3 [(CH3COO)3Al])/([Al(OH)3] ([CH3CO2H])^3)
Rate of reaction
![Construct the rate of reaction expression for: Al(OH)_3 + CH_3CO_2H ⟶ H_2O + (CH3COO)3Al 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: Al(OH)_3 + 3 CH_3CO_2H ⟶ 3 H_2O + (CH3COO)3Al 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 Al(OH)_3 | 1 | -1 CH_3CO_2H | 3 | -3 H_2O | 3 | 3 (CH3COO)3Al | 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 Al(OH)_3 | 1 | -1 | -(Δ[Al(OH)3])/(Δt) CH_3CO_2H | 3 | -3 | -1/3 (Δ[CH3CO2H])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) (CH3COO)3Al | 1 | 1 | (Δ[(CH3COO)3Al])/(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 = -(Δ[Al(OH)3])/(Δt) = -1/3 (Δ[CH3CO2H])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[(CH3COO)3Al])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/38802c211b1ee8e79bdff0cfe009d9c2.png)
Construct the rate of reaction expression for: Al(OH)_3 + CH_3CO_2H ⟶ H_2O + (CH3COO)3Al 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: Al(OH)_3 + 3 CH_3CO_2H ⟶ 3 H_2O + (CH3COO)3Al 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 Al(OH)_3 | 1 | -1 CH_3CO_2H | 3 | -3 H_2O | 3 | 3 (CH3COO)3Al | 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 Al(OH)_3 | 1 | -1 | -(Δ[Al(OH)3])/(Δt) CH_3CO_2H | 3 | -3 | -1/3 (Δ[CH3CO2H])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) (CH3COO)3Al | 1 | 1 | (Δ[(CH3COO)3Al])/(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 = -(Δ[Al(OH)3])/(Δt) = -1/3 (Δ[CH3CO2H])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[(CH3COO)3Al])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| aluminum hydroxide | acetic acid | water | (CH3COO)3Al formula | Al(OH)_3 | CH_3CO_2H | H_2O | (CH3COO)3Al Hill formula | AlH_3O_3 | C_2H_4O_2 | H_2O | C6H9AlO6 name | aluminum hydroxide | acetic acid | water |](../image_source/2998af109a34d3c5ddb273cf2855f721.png)
| aluminum hydroxide | acetic acid | water | (CH3COO)3Al formula | Al(OH)_3 | CH_3CO_2H | H_2O | (CH3COO)3Al Hill formula | AlH_3O_3 | C_2H_4O_2 | H_2O | C6H9AlO6 name | aluminum hydroxide | acetic acid | water |
Substance properties
![| aluminum hydroxide | acetic acid | water | (CH3COO)3Al molar mass | 78.003 g/mol | 60.052 g/mol | 18.015 g/mol | 204.11 g/mol phase | | liquid (at STP) | liquid (at STP) | melting point | | 16.2 °C | 0 °C | boiling point | | 117.5 °C | 99.9839 °C | density | | 1.049 g/cm^3 | 1 g/cm^3 | solubility in water | | miscible | | surface tension | | 0.0288 N/m | 0.0728 N/m | dynamic viscosity | | 0.001056 Pa s (at 25 °C) | 8.9×10^-4 Pa s (at 25 °C) | odor | | vinegar-like | odorless |](../image_source/a444ddc555f8471fa911a68e77bfea03.png)
| aluminum hydroxide | acetic acid | water | (CH3COO)3Al molar mass | 78.003 g/mol | 60.052 g/mol | 18.015 g/mol | 204.11 g/mol phase | | liquid (at STP) | liquid (at STP) | melting point | | 16.2 °C | 0 °C | boiling point | | 117.5 °C | 99.9839 °C | density | | 1.049 g/cm^3 | 1 g/cm^3 | solubility in water | | miscible | | surface tension | | 0.0288 N/m | 0.0728 N/m | dynamic viscosity | | 0.001056 Pa s (at 25 °C) | 8.9×10^-4 Pa s (at 25 °C) | odor | | vinegar-like | odorless |
Units