Search

Al(OH)3 + CH3COOH = H2O + Al(C2H3O2)3

Input interpretation

Al(OH)_3 (aluminum hydroxide) + CH_3CO_2H (acetic acid) ⟶ H_2O (water) + Al(C2H3O2)3
Al(OH)_3 (aluminum hydroxide) + CH_3CO_2H (acetic acid) ⟶ H_2O (water) + Al(C2H3O2)3

Balanced equation

Balance the chemical equation algebraically: Al(OH)_3 + CH_3CO_2H ⟶ H_2O + Al(C2H3O2)3 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 Al(C2H3O2)3 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 + Al(C2H3O2)3
Balance the chemical equation algebraically: Al(OH)_3 + CH_3CO_2H ⟶ H_2O + Al(C2H3O2)3 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 Al(C2H3O2)3 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 + Al(C2H3O2)3

Structures

+ ⟶ + Al(C2H3O2)3
+ ⟶ + Al(C2H3O2)3

Names

aluminum hydroxide + acetic acid ⟶ water + Al(C2H3O2)3
aluminum hydroxide + acetic acid ⟶ water + Al(C2H3O2)3

Equilibrium constant

Construct the equilibrium constant, K, expression for: Al(OH)_3 + CH_3CO_2H ⟶ H_2O + Al(C2H3O2)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: Al(OH)_3 + 3 CH_3CO_2H ⟶ 3 H_2O + Al(C2H3O2)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 Al(OH)_3 | 1 | -1 CH_3CO_2H | 3 | -3 H_2O | 3 | 3 Al(C2H3O2)3 | 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 Al(C2H3O2)3 | 1 | 1 | [Al(C2H3O2)3] 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 [Al(C2H3O2)3] = (([H2O])^3 [Al(C2H3O2)3])/([Al(OH)3] ([CH3CO2H])^3)
Construct the equilibrium constant, K, expression for: Al(OH)_3 + CH_3CO_2H ⟶ H_2O + Al(C2H3O2)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: Al(OH)_3 + 3 CH_3CO_2H ⟶ 3 H_2O + Al(C2H3O2)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 Al(OH)_3 | 1 | -1 CH_3CO_2H | 3 | -3 H_2O | 3 | 3 Al(C2H3O2)3 | 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 Al(C2H3O2)3 | 1 | 1 | [Al(C2H3O2)3] 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 [Al(C2H3O2)3] = (([H2O])^3 [Al(C2H3O2)3])/([Al(OH)3] ([CH3CO2H])^3)

Rate of reaction

Construct the rate of reaction expression for: Al(OH)_3 + CH_3CO_2H ⟶ H_2O + Al(C2H3O2)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: Al(OH)_3 + 3 CH_3CO_2H ⟶ 3 H_2O + Al(C2H3O2)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 Al(OH)_3 | 1 | -1 CH_3CO_2H | 3 | -3 H_2O | 3 | 3 Al(C2H3O2)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 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) Al(C2H3O2)3 | 1 | 1 | (Δ[Al(C2H3O2)3])/(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[Al(C2H3O2)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: Al(OH)_3 + CH_3CO_2H ⟶ H_2O + Al(C2H3O2)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: Al(OH)_3 + 3 CH_3CO_2H ⟶ 3 H_2O + Al(C2H3O2)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 Al(OH)_3 | 1 | -1 CH_3CO_2H | 3 | -3 H_2O | 3 | 3 Al(C2H3O2)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 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) Al(C2H3O2)3 | 1 | 1 | (Δ[Al(C2H3O2)3])/(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[Al(C2H3O2)3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| aluminum hydroxide | acetic acid | water | Al(C2H3O2)3 formula | Al(OH)_3 | CH_3CO_2H | H_2O | Al(C2H3O2)3 Hill formula | AlH_3O_3 | C_2H_4O_2 | H_2O | C6H9AlO6 name | aluminum hydroxide | acetic acid | water |
| aluminum hydroxide | acetic acid | water | Al(C2H3O2)3 formula | Al(OH)_3 | CH_3CO_2H | H_2O | Al(C2H3O2)3 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 | Al(C2H3O2)3 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 |
| aluminum hydroxide | acetic acid | water | Al(C2H3O2)3 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

Random Queries

thermal conductivity of indium vs thallium
boiling point of aniline
formula of thallium(III) nitrate
hexaammineruthenium(III) chloride
H2O + KOH + Zn = H2 + K
name of thorium(IV) cation
HCl + KI + KBrO3 = H2O + I2 + KCl + KBr
color of loveringite
MDL number of indium(III) fluoride
alternate names of terbium(III) sulfate octahydrate