Input interpretation
![H_2SO_4 sulfuric acid + CH_3COONa sodium acetate ⟶ CH_3CO_2H acetic acid + NaHSO_4 sodium bisulfate](../image_source/24465ca3e5c5c91fb5a634b37929625b.png)
H_2SO_4 sulfuric acid + CH_3COONa sodium acetate ⟶ CH_3CO_2H acetic acid + NaHSO_4 sodium bisulfate
Balanced equation
![Balance the chemical equation algebraically: H_2SO_4 + CH_3COONa ⟶ CH_3CO_2H + NaHSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 CH_3COONa ⟶ c_3 CH_3CO_2H + c_4 NaHSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, C and Na: H: | 2 c_1 + 3 c_2 = 4 c_3 + c_4 O: | 4 c_1 + 2 c_2 = 2 c_3 + 4 c_4 S: | c_1 = c_4 C: | 2 c_2 = 2 c_3 Na: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + CH_3COONa ⟶ CH_3CO_2H + NaHSO_4](../image_source/27c687a8778730fc3c0696a69d4531a6.png)
Balance the chemical equation algebraically: H_2SO_4 + CH_3COONa ⟶ CH_3CO_2H + NaHSO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2SO_4 + c_2 CH_3COONa ⟶ c_3 CH_3CO_2H + c_4 NaHSO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, S, C and Na: H: | 2 c_1 + 3 c_2 = 4 c_3 + c_4 O: | 4 c_1 + 2 c_2 = 2 c_3 + 4 c_4 S: | c_1 = c_4 C: | 2 c_2 = 2 c_3 Na: | 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_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2SO_4 + CH_3COONa ⟶ CH_3CO_2H + NaHSO_4
Structures
![+ ⟶ +](../image_source/fa8c994c0f711bf135031743c5ac9438.png)
+ ⟶ +
Names
![sulfuric acid + sodium acetate ⟶ acetic acid + sodium bisulfate](../image_source/dcf95bde1900248632b007a35ea89b84.png)
sulfuric acid + sodium acetate ⟶ acetic acid + sodium bisulfate
Reaction thermodynamics
Gibbs free energy
![| sulfuric acid | sodium acetate | acetic acid | sodium bisulfate molecular free energy | -690 kJ/mol | -607.2 kJ/mol | -389.9 kJ/mol | -992.8 kJ/mol total free energy | -690 kJ/mol | -607.2 kJ/mol | -389.9 kJ/mol | -992.8 kJ/mol | G_initial = -1297 kJ/mol | | G_final = -1383 kJ/mol | ΔG_rxn^0 | -1383 kJ/mol - -1297 kJ/mol = -85.5 kJ/mol (exergonic) | | |](../image_source/ccfc4825e4ea909080e8e7132dc638ac.png)
| sulfuric acid | sodium acetate | acetic acid | sodium bisulfate molecular free energy | -690 kJ/mol | -607.2 kJ/mol | -389.9 kJ/mol | -992.8 kJ/mol total free energy | -690 kJ/mol | -607.2 kJ/mol | -389.9 kJ/mol | -992.8 kJ/mol | G_initial = -1297 kJ/mol | | G_final = -1383 kJ/mol | ΔG_rxn^0 | -1383 kJ/mol - -1297 kJ/mol = -85.5 kJ/mol (exergonic) | | |
Equilibrium constant
![Construct the equilibrium constant, K, expression for: H_2SO_4 + CH_3COONa ⟶ CH_3CO_2H + NaHSO_4 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: H_2SO_4 + CH_3COONa ⟶ CH_3CO_2H + NaHSO_4 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 H_2SO_4 | 1 | -1 CH_3COONa | 1 | -1 CH_3CO_2H | 1 | 1 NaHSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) CH_3COONa | 1 | -1 | ([CH3COONa])^(-1) CH_3CO_2H | 1 | 1 | [CH3CO2H] NaHSO_4 | 1 | 1 | [NaHSO4] 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 = ([H2SO4])^(-1) ([CH3COONa])^(-1) [CH3CO2H] [NaHSO4] = ([CH3CO2H] [NaHSO4])/([H2SO4] [CH3COONa])](../image_source/e547d9e1c41a5ca0099c09fb09c33451.png)
Construct the equilibrium constant, K, expression for: H_2SO_4 + CH_3COONa ⟶ CH_3CO_2H + NaHSO_4 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: H_2SO_4 + CH_3COONa ⟶ CH_3CO_2H + NaHSO_4 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 H_2SO_4 | 1 | -1 CH_3COONa | 1 | -1 CH_3CO_2H | 1 | 1 NaHSO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2SO_4 | 1 | -1 | ([H2SO4])^(-1) CH_3COONa | 1 | -1 | ([CH3COONa])^(-1) CH_3CO_2H | 1 | 1 | [CH3CO2H] NaHSO_4 | 1 | 1 | [NaHSO4] 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 = ([H2SO4])^(-1) ([CH3COONa])^(-1) [CH3CO2H] [NaHSO4] = ([CH3CO2H] [NaHSO4])/([H2SO4] [CH3COONa])
Rate of reaction
![Construct the rate of reaction expression for: H_2SO_4 + CH_3COONa ⟶ CH_3CO_2H + NaHSO_4 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: H_2SO_4 + CH_3COONa ⟶ CH_3CO_2H + NaHSO_4 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 H_2SO_4 | 1 | -1 CH_3COONa | 1 | -1 CH_3CO_2H | 1 | 1 NaHSO_4 | 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 H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) CH_3COONa | 1 | -1 | -(Δ[CH3COONa])/(Δt) CH_3CO_2H | 1 | 1 | (Δ[CH3CO2H])/(Δt) NaHSO_4 | 1 | 1 | (Δ[NaHSO4])/(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[H2SO4])/(Δt) = -(Δ[CH3COONa])/(Δt) = (Δ[CH3CO2H])/(Δt) = (Δ[NaHSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/e46298ef2f679ee5bd0c53eb1dd7cda4.png)
Construct the rate of reaction expression for: H_2SO_4 + CH_3COONa ⟶ CH_3CO_2H + NaHSO_4 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: H_2SO_4 + CH_3COONa ⟶ CH_3CO_2H + NaHSO_4 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 H_2SO_4 | 1 | -1 CH_3COONa | 1 | -1 CH_3CO_2H | 1 | 1 NaHSO_4 | 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 H_2SO_4 | 1 | -1 | -(Δ[H2SO4])/(Δt) CH_3COONa | 1 | -1 | -(Δ[CH3COONa])/(Δt) CH_3CO_2H | 1 | 1 | (Δ[CH3CO2H])/(Δt) NaHSO_4 | 1 | 1 | (Δ[NaHSO4])/(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[H2SO4])/(Δt) = -(Δ[CH3COONa])/(Δt) = (Δ[CH3CO2H])/(Δt) = (Δ[NaHSO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| sulfuric acid | sodium acetate | acetic acid | sodium bisulfate formula | H_2SO_4 | CH_3COONa | CH_3CO_2H | NaHSO_4 Hill formula | H_2O_4S | C_2H_3NaO_2 | C_2H_4O_2 | HNaO_4S name | sulfuric acid | sodium acetate | acetic acid | sodium bisulfate](../image_source/ff992b5b5c1f718be058d1e3cf488251.png)
| sulfuric acid | sodium acetate | acetic acid | sodium bisulfate formula | H_2SO_4 | CH_3COONa | CH_3CO_2H | NaHSO_4 Hill formula | H_2O_4S | C_2H_3NaO_2 | C_2H_4O_2 | HNaO_4S name | sulfuric acid | sodium acetate | acetic acid | sodium bisulfate
Substance properties
![| sulfuric acid | sodium acetate | acetic acid | sodium bisulfate molar mass | 98.07 g/mol | 82.034 g/mol | 60.052 g/mol | 120.1 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | 10.371 °C | 300 °C | 16.2 °C | 181.85 °C boiling point | 279.6 °C | 881.4 °C | 117.5 °C | density | 1.8305 g/cm^3 | 1.528 g/cm^3 | 1.049 g/cm^3 | 1.8 g/cm^3 solubility in water | very soluble | soluble | miscible | surface tension | 0.0735 N/m | | 0.0288 N/m | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 0.001056 Pa s (at 25 °C) | odor | odorless | odorless | vinegar-like |](../image_source/0e1853e17f73f368969258085a2e9113.png)
| sulfuric acid | sodium acetate | acetic acid | sodium bisulfate molar mass | 98.07 g/mol | 82.034 g/mol | 60.052 g/mol | 120.1 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | 10.371 °C | 300 °C | 16.2 °C | 181.85 °C boiling point | 279.6 °C | 881.4 °C | 117.5 °C | density | 1.8305 g/cm^3 | 1.528 g/cm^3 | 1.049 g/cm^3 | 1.8 g/cm^3 solubility in water | very soluble | soluble | miscible | surface tension | 0.0735 N/m | | 0.0288 N/m | dynamic viscosity | 0.021 Pa s (at 25 °C) | | 0.001056 Pa s (at 25 °C) | odor | odorless | odorless | vinegar-like |
Units