AgNO3 + Na3PO4 = AgPO4 + Na3NO3

AgNO_3 silver nitrate + Na_3PO_4 trisodium phosphate ⟶ AgPO4 + Na3NO3

Balance the chemical equation algebraically: AgNO_3 + Na_3PO_4 ⟶ AgPO4 + Na3NO3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgNO_3 + c_2 Na_3PO_4 ⟶ c_3 AgPO4 + c_4 Na3NO3 Set the number of atoms in the reactants equal to the number of atoms in the products for Ag, N, O, Na and P: Ag: | c_1 = c_3 N: | c_1 = c_4 O: | 3 c_1 + 4 c_2 = 4 c_3 + 3 c_4 Na: | 3 c_2 = 3 c_4 P: | 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 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | AgNO_3 + Na_3PO_4 ⟶ AgPO4 + Na3NO3

+ ⟶ AgPO4 + Na3NO3

silver nitrate + trisodium phosphate ⟶ AgPO4 + Na3NO3

Construct the equilibrium constant, K, expression for: AgNO_3 + Na_3PO_4 ⟶ AgPO4 + Na3NO3 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: AgNO_3 + Na_3PO_4 ⟶ AgPO4 + Na3NO3 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 AgNO_3 | 1 | -1 Na_3PO_4 | 1 | -1 AgPO4 | 1 | 1 Na3NO3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression AgNO_3 | 1 | -1 | ([AgNO3])^(-1) Na_3PO_4 | 1 | -1 | ([Na3PO4])^(-1) AgPO4 | 1 | 1 | [AgPO4] Na3NO3 | 1 | 1 | [Na3NO3] 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 = ([AgNO3])^(-1) ([Na3PO4])^(-1) [AgPO4] [Na3NO3] = ([AgPO4] [Na3NO3])/([AgNO3] [Na3PO4])

Construct the rate of reaction expression for: AgNO_3 + Na_3PO_4 ⟶ AgPO4 + Na3NO3 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: AgNO_3 + Na_3PO_4 ⟶ AgPO4 + Na3NO3 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 AgNO_3 | 1 | -1 Na_3PO_4 | 1 | -1 AgPO4 | 1 | 1 Na3NO3 | 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 AgNO_3 | 1 | -1 | -(Δ[AgNO3])/(Δt) Na_3PO_4 | 1 | -1 | -(Δ[Na3PO4])/(Δt) AgPO4 | 1 | 1 | (Δ[AgPO4])/(Δt) Na3NO3 | 1 | 1 | (Δ[Na3NO3])/(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[AgNO3])/(Δt) = -(Δ[Na3PO4])/(Δt) = (Δ[AgPO4])/(Δt) = (Δ[Na3NO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| silver nitrate | trisodium phosphate | AgPO4 | Na3NO3 formula | AgNO_3 | Na_3PO_4 | AgPO4 | Na3NO3 Hill formula | AgNO_3 | Na_3O_4P | AgO4P | NNa3O3 name | silver nitrate | trisodium phosphate | |

| silver nitrate | trisodium phosphate | AgPO4 | Na3NO3 molar mass | 169.87 g/mol | 163.94 g/mol | 202.84 g/mol | 130.97 g/mol phase | solid (at STP) | solid (at STP) | | melting point | 212 °C | 75 °C | | density | | 2.536 g/cm^3 | | solubility in water | soluble | soluble | | odor | odorless | odorless | |