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NaOH + H3PO4 = H2O + Na3PO4

Input interpretation

NaOH (sodium hydroxide) + H_3PO_4 (phosphoric acid) ⟶ H_2O (water) + Na_3PO_4 (trisodium phosphate)
NaOH (sodium hydroxide) + H_3PO_4 (phosphoric acid) ⟶ H_2O (water) + Na_3PO_4 (trisodium phosphate)

Balanced equation

Balance the chemical equation algebraically: NaOH + H_3PO_4 ⟶ H_2O + Na_3PO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 H_3PO_4 ⟶ c_3 H_2O + c_4 Na_3PO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O and P: H: | c_1 + 3 c_2 = 2 c_3 Na: | c_1 = 3 c_4 O: | c_1 + 4 c_2 = c_3 + 4 c_4 P: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 1 c_3 = 3 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 NaOH + H_3PO_4 ⟶ 3 H_2O + Na_3PO_4
Balance the chemical equation algebraically: NaOH + H_3PO_4 ⟶ H_2O + Na_3PO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 H_3PO_4 ⟶ c_3 H_2O + c_4 Na_3PO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O and P: H: | c_1 + 3 c_2 = 2 c_3 Na: | c_1 = 3 c_4 O: | c_1 + 4 c_2 = c_3 + 4 c_4 P: | 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 3 c_2 = 1 c_3 = 3 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 3 NaOH + H_3PO_4 ⟶ 3 H_2O + Na_3PO_4

Structures

+ ⟶ +
+ ⟶ +

Names

sodium hydroxide + phosphoric acid ⟶ water + trisodium phosphate
sodium hydroxide + phosphoric acid ⟶ water + trisodium phosphate

Equilibrium constant

Construct the equilibrium constant, K, expression for: NaOH + H_3PO_4 ⟶ H_2O + Na_3PO_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: 3 NaOH + H_3PO_4 ⟶ 3 H_2O + Na_3PO_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 NaOH | 3 | -3 H_3PO_4 | 1 | -1 H_2O | 3 | 3 Na_3PO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 3 | -3 | ([NaOH])^(-3) H_3PO_4 | 1 | -1 | ([H3PO4])^(-1) H_2O | 3 | 3 | ([H2O])^3 Na_3PO_4 | 1 | 1 | [Na3PO4] 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 = ([NaOH])^(-3) ([H3PO4])^(-1) ([H2O])^3 [Na3PO4] = (([H2O])^3 [Na3PO4])/(([NaOH])^3 [H3PO4])
Construct the equilibrium constant, K, expression for: NaOH + H_3PO_4 ⟶ H_2O + Na_3PO_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: 3 NaOH + H_3PO_4 ⟶ 3 H_2O + Na_3PO_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 NaOH | 3 | -3 H_3PO_4 | 1 | -1 H_2O | 3 | 3 Na_3PO_4 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 3 | -3 | ([NaOH])^(-3) H_3PO_4 | 1 | -1 | ([H3PO4])^(-1) H_2O | 3 | 3 | ([H2O])^3 Na_3PO_4 | 1 | 1 | [Na3PO4] 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 = ([NaOH])^(-3) ([H3PO4])^(-1) ([H2O])^3 [Na3PO4] = (([H2O])^3 [Na3PO4])/(([NaOH])^3 [H3PO4])

Rate of reaction

Construct the rate of reaction expression for: NaOH + H_3PO_4 ⟶ H_2O + Na_3PO_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: 3 NaOH + H_3PO_4 ⟶ 3 H_2O + Na_3PO_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 NaOH | 3 | -3 H_3PO_4 | 1 | -1 H_2O | 3 | 3 Na_3PO_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 NaOH | 3 | -3 | -1/3 (Δ[NaOH])/(Δt) H_3PO_4 | 1 | -1 | -(Δ[H3PO4])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) Na_3PO_4 | 1 | 1 | (Δ[Na3PO4])/(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 = -1/3 (Δ[NaOH])/(Δt) = -(Δ[H3PO4])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[Na3PO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: NaOH + H_3PO_4 ⟶ H_2O + Na_3PO_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: 3 NaOH + H_3PO_4 ⟶ 3 H_2O + Na_3PO_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 NaOH | 3 | -3 H_3PO_4 | 1 | -1 H_2O | 3 | 3 Na_3PO_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 NaOH | 3 | -3 | -1/3 (Δ[NaOH])/(Δt) H_3PO_4 | 1 | -1 | -(Δ[H3PO4])/(Δt) H_2O | 3 | 3 | 1/3 (Δ[H2O])/(Δt) Na_3PO_4 | 1 | 1 | (Δ[Na3PO4])/(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 = -1/3 (Δ[NaOH])/(Δt) = -(Δ[H3PO4])/(Δt) = 1/3 (Δ[H2O])/(Δt) = (Δ[Na3PO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| sodium hydroxide | phosphoric acid | water | trisodium phosphate formula | NaOH | H_3PO_4 | H_2O | Na_3PO_4 Hill formula | HNaO | H_3O_4P | H_2O | Na_3O_4P name | sodium hydroxide | phosphoric acid | water | trisodium phosphate
| sodium hydroxide | phosphoric acid | water | trisodium phosphate formula | NaOH | H_3PO_4 | H_2O | Na_3PO_4 Hill formula | HNaO | H_3O_4P | H_2O | Na_3O_4P name | sodium hydroxide | phosphoric acid | water | trisodium phosphate

Substance properties

| sodium hydroxide | phosphoric acid | water | trisodium phosphate molar mass | 39.997 g/mol | 97.994 g/mol | 18.015 g/mol | 163.94 g/mol phase | solid (at STP) | liquid (at STP) | liquid (at STP) | solid (at STP) melting point | 323 °C | 42.4 °C | 0 °C | 75 °C boiling point | 1390 °C | 158 °C | 99.9839 °C | density | 2.13 g/cm^3 | 1.685 g/cm^3 | 1 g/cm^3 | 2.536 g/cm^3 solubility in water | soluble | very soluble | | soluble surface tension | 0.07435 N/m | | 0.0728 N/m | dynamic viscosity | 0.004 Pa s (at 350 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | | odorless | odorless | odorless
| sodium hydroxide | phosphoric acid | water | trisodium phosphate molar mass | 39.997 g/mol | 97.994 g/mol | 18.015 g/mol | 163.94 g/mol phase | solid (at STP) | liquid (at STP) | liquid (at STP) | solid (at STP) melting point | 323 °C | 42.4 °C | 0 °C | 75 °C boiling point | 1390 °C | 158 °C | 99.9839 °C | density | 2.13 g/cm^3 | 1.685 g/cm^3 | 1 g/cm^3 | 2.536 g/cm^3 solubility in water | soluble | very soluble | | soluble surface tension | 0.07435 N/m | | 0.0728 N/m | dynamic viscosity | 0.004 Pa s (at 350 °C) | | 8.9×10^-4 Pa s (at 25 °C) | odor | | odorless | odorless | odorless

Units

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