Input interpretation
![HCl hydrogen chloride + Na_3PO_4 trisodium phosphate ⟶ NaCl sodium chloride + H_3PO_4 phosphoric acid](../image_source/831d2a03d900f2e07dce9c3be5973035.png)
HCl hydrogen chloride + Na_3PO_4 trisodium phosphate ⟶ NaCl sodium chloride + H_3PO_4 phosphoric acid
Balanced equation
![Balance the chemical equation algebraically: HCl + Na_3PO_4 ⟶ NaCl + H_3PO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Na_3PO_4 ⟶ c_3 NaCl + c_4 H_3PO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Na, O and P: Cl: | c_1 = c_3 H: | c_1 = 3 c_4 Na: | 3 c_2 = c_3 O: | 4 c_2 = 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 HCl + Na_3PO_4 ⟶ 3 NaCl + H_3PO_4](../image_source/4aff50580b10315ebe65fb96283fdd74.png)
Balance the chemical equation algebraically: HCl + Na_3PO_4 ⟶ NaCl + H_3PO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 Na_3PO_4 ⟶ c_3 NaCl + c_4 H_3PO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, Na, O and P: Cl: | c_1 = c_3 H: | c_1 = 3 c_4 Na: | 3 c_2 = c_3 O: | 4 c_2 = 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 HCl + Na_3PO_4 ⟶ 3 NaCl + H_3PO_4
Structures
![+ ⟶ +](../image_source/173c076b7c045a7d8278663d2eb9842a.png)
+ ⟶ +
Names
![hydrogen chloride + trisodium phosphate ⟶ sodium chloride + phosphoric acid](../image_source/cede94f4b9608784cdc80d6a8da74bc9.png)
hydrogen chloride + trisodium phosphate ⟶ sodium chloride + phosphoric acid
Equilibrium constant
![Construct the equilibrium constant, K, expression for: HCl + Na_3PO_4 ⟶ NaCl + H_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 HCl + Na_3PO_4 ⟶ 3 NaCl + H_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 HCl | 3 | -3 Na_3PO_4 | 1 | -1 NaCl | 3 | 3 H_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 HCl | 3 | -3 | ([HCl])^(-3) Na_3PO_4 | 1 | -1 | ([Na3PO4])^(-1) NaCl | 3 | 3 | ([NaCl])^3 H_3PO_4 | 1 | 1 | [H3PO4] 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])^(-3) ([Na3PO4])^(-1) ([NaCl])^3 [H3PO4] = (([NaCl])^3 [H3PO4])/(([HCl])^3 [Na3PO4])](../image_source/0b1dc8d5e3e09a17f7147a1ed3ebf053.png)
Construct the equilibrium constant, K, expression for: HCl + Na_3PO_4 ⟶ NaCl + H_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 HCl + Na_3PO_4 ⟶ 3 NaCl + H_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 HCl | 3 | -3 Na_3PO_4 | 1 | -1 NaCl | 3 | 3 H_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 HCl | 3 | -3 | ([HCl])^(-3) Na_3PO_4 | 1 | -1 | ([Na3PO4])^(-1) NaCl | 3 | 3 | ([NaCl])^3 H_3PO_4 | 1 | 1 | [H3PO4] 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])^(-3) ([Na3PO4])^(-1) ([NaCl])^3 [H3PO4] = (([NaCl])^3 [H3PO4])/(([HCl])^3 [Na3PO4])
Rate of reaction
![Construct the rate of reaction expression for: HCl + Na_3PO_4 ⟶ NaCl + H_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 HCl + Na_3PO_4 ⟶ 3 NaCl + H_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 HCl | 3 | -3 Na_3PO_4 | 1 | -1 NaCl | 3 | 3 H_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 HCl | 3 | -3 | -1/3 (Δ[HCl])/(Δt) Na_3PO_4 | 1 | -1 | -(Δ[Na3PO4])/(Δt) NaCl | 3 | 3 | 1/3 (Δ[NaCl])/(Δt) H_3PO_4 | 1 | 1 | (Δ[H3PO4])/(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[HCl])/(Δt) = -(Δ[Na3PO4])/(Δt) = 1/3 (Δ[NaCl])/(Δt) = (Δ[H3PO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/66a0f77d4739dea971c3839e1f457058.png)
Construct the rate of reaction expression for: HCl + Na_3PO_4 ⟶ NaCl + H_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 HCl + Na_3PO_4 ⟶ 3 NaCl + H_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 HCl | 3 | -3 Na_3PO_4 | 1 | -1 NaCl | 3 | 3 H_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 HCl | 3 | -3 | -1/3 (Δ[HCl])/(Δt) Na_3PO_4 | 1 | -1 | -(Δ[Na3PO4])/(Δt) NaCl | 3 | 3 | 1/3 (Δ[NaCl])/(Δt) H_3PO_4 | 1 | 1 | (Δ[H3PO4])/(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[HCl])/(Δt) = -(Δ[Na3PO4])/(Δt) = 1/3 (Δ[NaCl])/(Δt) = (Δ[H3PO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| hydrogen chloride | trisodium phosphate | sodium chloride | phosphoric acid formula | HCl | Na_3PO_4 | NaCl | H_3PO_4 Hill formula | ClH | Na_3O_4P | ClNa | H_3O_4P name | hydrogen chloride | trisodium phosphate | sodium chloride | phosphoric acid](../image_source/9187a1a86510270dbb14d022cfbe023c.png)
| hydrogen chloride | trisodium phosphate | sodium chloride | phosphoric acid formula | HCl | Na_3PO_4 | NaCl | H_3PO_4 Hill formula | ClH | Na_3O_4P | ClNa | H_3O_4P name | hydrogen chloride | trisodium phosphate | sodium chloride | phosphoric acid
Substance properties
![| hydrogen chloride | trisodium phosphate | sodium chloride | phosphoric acid molar mass | 36.46 g/mol | 163.94 g/mol | 58.44 g/mol | 97.994 g/mol phase | gas (at STP) | solid (at STP) | solid (at STP) | liquid (at STP) melting point | -114.17 °C | 75 °C | 801 °C | 42.4 °C boiling point | -85 °C | | 1413 °C | 158 °C density | 0.00149 g/cm^3 (at 25 °C) | 2.536 g/cm^3 | 2.16 g/cm^3 | 1.685 g/cm^3 solubility in water | miscible | soluble | soluble | very soluble odor | | odorless | odorless | odorless](../image_source/ccf00610d7cf132d02910c5ee6fcbcc9.png)
| hydrogen chloride | trisodium phosphate | sodium chloride | phosphoric acid molar mass | 36.46 g/mol | 163.94 g/mol | 58.44 g/mol | 97.994 g/mol phase | gas (at STP) | solid (at STP) | solid (at STP) | liquid (at STP) melting point | -114.17 °C | 75 °C | 801 °C | 42.4 °C boiling point | -85 °C | | 1413 °C | 158 °C density | 0.00149 g/cm^3 (at 25 °C) | 2.536 g/cm^3 | 2.16 g/cm^3 | 1.685 g/cm^3 solubility in water | miscible | soluble | soluble | very soluble odor | | odorless | odorless | odorless
Units