AgNO3 + NaPO4 = NaNO3 + AgPO4

AgNO_3 silver nitrate + NaPO4 ⟶ NaNO_3 sodium nitrate + AgPO4

Balance the chemical equation algebraically: AgNO_3 + NaPO4 ⟶ NaNO_3 + AgPO4 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 AgNO_3 + c_2 NaPO4 ⟶ c_3 NaNO_3 + c_4 AgPO4 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_4 N: | c_1 = c_3 O: | 3 c_1 + 4 c_2 = 3 c_3 + 4 c_4 Na: | c_2 = c_3 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_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 + NaPO4 ⟶ NaNO_3 + AgPO4

+ NaPO4 ⟶ + AgPO4

silver nitrate + NaPO4 ⟶ sodium nitrate + AgPO4

Construct the equilibrium constant, K, expression for: AgNO_3 + NaPO4 ⟶ NaNO_3 + AgPO4 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 + NaPO4 ⟶ NaNO_3 + AgPO4 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 NaPO4 | 1 | -1 NaNO_3 | 1 | 1 AgPO4 | 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) NaPO4 | 1 | -1 | ([NaPO4])^(-1) NaNO_3 | 1 | 1 | [NaNO3] AgPO4 | 1 | 1 | [AgPO4] 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) ([NaPO4])^(-1) [NaNO3] [AgPO4] = ([NaNO3] [AgPO4])/([AgNO3] [NaPO4])

Construct the rate of reaction expression for: AgNO_3 + NaPO4 ⟶ NaNO_3 + AgPO4 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 + NaPO4 ⟶ NaNO_3 + AgPO4 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 NaPO4 | 1 | -1 NaNO_3 | 1 | 1 AgPO4 | 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) NaPO4 | 1 | -1 | -(Δ[NaPO4])/(Δt) NaNO_3 | 1 | 1 | (Δ[NaNO3])/(Δt) AgPO4 | 1 | 1 | (Δ[AgPO4])/(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[NaPO4])/(Δt) = (Δ[NaNO3])/(Δt) = (Δ[AgPO4])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| silver nitrate | NaPO4 | sodium nitrate | AgPO4 formula | AgNO_3 | NaPO4 | NaNO_3 | AgPO4 Hill formula | AgNO_3 | NaO4P | NNaO_3 | AgO4P name | silver nitrate | | sodium nitrate |

| silver nitrate | NaPO4 | sodium nitrate | AgPO4 molar mass | 169.87 g/mol | 117.96 g/mol | 84.994 g/mol | 202.84 g/mol phase | solid (at STP) | | solid (at STP) | melting point | 212 °C | | 306 °C | density | | | 2.26 g/cm^3 | solubility in water | soluble | | soluble | dynamic viscosity | | | 0.003 Pa s (at 250 °C) | odor | odorless | | |