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H3PO4 + AgNO3 = HNO3 + Ag3PO4

Input interpretation

H_3PO_4 (phosphoric acid) + AgNO_3 (silver nitrate) ⟶ HNO_3 (nitric acid) + Ag_3PO_4 (silver phosphate)
H_3PO_4 (phosphoric acid) + AgNO_3 (silver nitrate) ⟶ HNO_3 (nitric acid) + Ag_3PO_4 (silver phosphate)

Balanced equation

Balance the chemical equation algebraically: H_3PO_4 + AgNO_3 ⟶ HNO_3 + Ag_3PO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_3PO_4 + c_2 AgNO_3 ⟶ c_3 HNO_3 + c_4 Ag_3PO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, P, Ag and N: H: | 3 c_1 = c_3 O: | 4 c_1 + 3 c_2 = 3 c_3 + 4 c_4 P: | c_1 = c_4 Ag: | c_2 = 3 c_4 N: | c_2 = c_3 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: | | H_3PO_4 + 3 AgNO_3 ⟶ 3 HNO_3 + Ag_3PO_4
Balance the chemical equation algebraically: H_3PO_4 + AgNO_3 ⟶ HNO_3 + Ag_3PO_4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_3PO_4 + c_2 AgNO_3 ⟶ c_3 HNO_3 + c_4 Ag_3PO_4 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, P, Ag and N: H: | 3 c_1 = c_3 O: | 4 c_1 + 3 c_2 = 3 c_3 + 4 c_4 P: | c_1 = c_4 Ag: | c_2 = 3 c_4 N: | c_2 = c_3 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: | | H_3PO_4 + 3 AgNO_3 ⟶ 3 HNO_3 + Ag_3PO_4

Structures

+ ⟶ +
+ ⟶ +

Names

phosphoric acid + silver nitrate ⟶ nitric acid + silver phosphate
phosphoric acid + silver nitrate ⟶ nitric acid + silver phosphate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_3PO_4 + AgNO_3 ⟶ HNO_3 + Ag_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: H_3PO_4 + 3 AgNO_3 ⟶ 3 HNO_3 + Ag_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 H_3PO_4 | 1 | -1 AgNO_3 | 3 | -3 HNO_3 | 3 | 3 Ag_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 H_3PO_4 | 1 | -1 | ([H3PO4])^(-1) AgNO_3 | 3 | -3 | ([AgNO3])^(-3) HNO_3 | 3 | 3 | ([HNO3])^3 Ag_3PO_4 | 1 | 1 | [Ag3PO4] 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 = ([H3PO4])^(-1) ([AgNO3])^(-3) ([HNO3])^3 [Ag3PO4] = (([HNO3])^3 [Ag3PO4])/([H3PO4] ([AgNO3])^3)
Construct the equilibrium constant, K, expression for: H_3PO_4 + AgNO_3 ⟶ HNO_3 + Ag_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: H_3PO_4 + 3 AgNO_3 ⟶ 3 HNO_3 + Ag_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 H_3PO_4 | 1 | -1 AgNO_3 | 3 | -3 HNO_3 | 3 | 3 Ag_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 H_3PO_4 | 1 | -1 | ([H3PO4])^(-1) AgNO_3 | 3 | -3 | ([AgNO3])^(-3) HNO_3 | 3 | 3 | ([HNO3])^3 Ag_3PO_4 | 1 | 1 | [Ag3PO4] 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 = ([H3PO4])^(-1) ([AgNO3])^(-3) ([HNO3])^3 [Ag3PO4] = (([HNO3])^3 [Ag3PO4])/([H3PO4] ([AgNO3])^3)

Rate of reaction

Construct the rate of reaction expression for: H_3PO_4 + AgNO_3 ⟶ HNO_3 + Ag_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: H_3PO_4 + 3 AgNO_3 ⟶ 3 HNO_3 + Ag_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 H_3PO_4 | 1 | -1 AgNO_3 | 3 | -3 HNO_3 | 3 | 3 Ag_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 H_3PO_4 | 1 | -1 | -(Δ[H3PO4])/(Δt) AgNO_3 | 3 | -3 | -1/3 (Δ[AgNO3])/(Δt) HNO_3 | 3 | 3 | 1/3 (Δ[HNO3])/(Δt) Ag_3PO_4 | 1 | 1 | (Δ[Ag3PO4])/(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[H3PO4])/(Δt) = -1/3 (Δ[AgNO3])/(Δt) = 1/3 (Δ[HNO3])/(Δt) = (Δ[Ag3PO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_3PO_4 + AgNO_3 ⟶ HNO_3 + Ag_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: H_3PO_4 + 3 AgNO_3 ⟶ 3 HNO_3 + Ag_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 H_3PO_4 | 1 | -1 AgNO_3 | 3 | -3 HNO_3 | 3 | 3 Ag_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 H_3PO_4 | 1 | -1 | -(Δ[H3PO4])/(Δt) AgNO_3 | 3 | -3 | -1/3 (Δ[AgNO3])/(Δt) HNO_3 | 3 | 3 | 1/3 (Δ[HNO3])/(Δt) Ag_3PO_4 | 1 | 1 | (Δ[Ag3PO4])/(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[H3PO4])/(Δt) = -1/3 (Δ[AgNO3])/(Δt) = 1/3 (Δ[HNO3])/(Δt) = (Δ[Ag3PO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| phosphoric acid | silver nitrate | nitric acid | silver phosphate formula | H_3PO_4 | AgNO_3 | HNO_3 | Ag_3PO_4 Hill formula | H_3O_4P | AgNO_3 | HNO_3 | Ag_3O_4P name | phosphoric acid | silver nitrate | nitric acid | silver phosphate IUPAC name | phosphoric acid | silver nitrate | nitric acid | trisilver phosphate
| phosphoric acid | silver nitrate | nitric acid | silver phosphate formula | H_3PO_4 | AgNO_3 | HNO_3 | Ag_3PO_4 Hill formula | H_3O_4P | AgNO_3 | HNO_3 | Ag_3O_4P name | phosphoric acid | silver nitrate | nitric acid | silver phosphate IUPAC name | phosphoric acid | silver nitrate | nitric acid | trisilver phosphate

Substance properties

| phosphoric acid | silver nitrate | nitric acid | silver phosphate molar mass | 97.994 g/mol | 169.87 g/mol | 63.012 g/mol | 418.574 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | 42.4 °C | 212 °C | -41.6 °C | 485 °C boiling point | 158 °C | | 83 °C | density | 1.685 g/cm^3 | | 1.5129 g/cm^3 | 4.449 g/cm^3 solubility in water | very soluble | soluble | miscible | insoluble dynamic viscosity | | | 7.6×10^-4 Pa s (at 25 °C) | odor | odorless | odorless | |
| phosphoric acid | silver nitrate | nitric acid | silver phosphate molar mass | 97.994 g/mol | 169.87 g/mol | 63.012 g/mol | 418.574 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | 42.4 °C | 212 °C | -41.6 °C | 485 °C boiling point | 158 °C | | 83 °C | density | 1.685 g/cm^3 | | 1.5129 g/cm^3 | 4.449 g/cm^3 solubility in water | very soluble | soluble | miscible | insoluble dynamic viscosity | | | 7.6×10^-4 Pa s (at 25 °C) | odor | odorless | odorless | |

Units

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