NaOH + AgNO3 = NaNO3 + AgOH

NaOH sodium hydroxide + AgNO_3 silver nitrate ⟶ NaNO_3 sodium nitrate + AgOH

Balance the chemical equation algebraically: NaOH + AgNO_3 ⟶ NaNO_3 + AgOH Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 AgNO_3 ⟶ c_3 NaNO_3 + c_4 AgOH Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Ag and N: H: | c_1 = c_4 Na: | c_1 = c_3 O: | c_1 + 3 c_2 = 3 c_3 + c_4 Ag: | c_2 = 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 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | NaOH + AgNO_3 ⟶ NaNO_3 + AgOH

+ ⟶ + AgOH

sodium hydroxide + silver nitrate ⟶ sodium nitrate + AgOH

Construct the equilibrium constant, K, expression for: NaOH + AgNO_3 ⟶ NaNO_3 + AgOH 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: NaOH + AgNO_3 ⟶ NaNO_3 + AgOH 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 | 1 | -1 AgNO_3 | 1 | -1 NaNO_3 | 1 | 1 AgOH | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 1 | -1 | ([NaOH])^(-1) AgNO_3 | 1 | -1 | ([AgNO3])^(-1) NaNO_3 | 1 | 1 | [NaNO3] AgOH | 1 | 1 | [AgOH] 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])^(-1) ([AgNO3])^(-1) [NaNO3] [AgOH] = ([NaNO3] [AgOH])/([NaOH] [AgNO3])

Construct the rate of reaction expression for: NaOH + AgNO_3 ⟶ NaNO_3 + AgOH 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: NaOH + AgNO_3 ⟶ NaNO_3 + AgOH 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 | 1 | -1 AgNO_3 | 1 | -1 NaNO_3 | 1 | 1 AgOH | 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 | 1 | -1 | -(Δ[NaOH])/(Δt) AgNO_3 | 1 | -1 | -(Δ[AgNO3])/(Δt) NaNO_3 | 1 | 1 | (Δ[NaNO3])/(Δt) AgOH | 1 | 1 | (Δ[AgOH])/(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[NaOH])/(Δt) = -(Δ[AgNO3])/(Δt) = (Δ[NaNO3])/(Δt) = (Δ[AgOH])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sodium hydroxide | silver nitrate | sodium nitrate | AgOH formula | NaOH | AgNO_3 | NaNO_3 | AgOH Hill formula | HNaO | AgNO_3 | NNaO_3 | HAgO name | sodium hydroxide | silver nitrate | sodium nitrate |

| sodium hydroxide | silver nitrate | sodium nitrate | AgOH molar mass | 39.997 g/mol | 169.87 g/mol | 84.994 g/mol | 124.875 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | melting point | 323 °C | 212 °C | 306 °C | boiling point | 1390 °C | | | density | 2.13 g/cm^3 | | 2.26 g/cm^3 | solubility in water | soluble | soluble | soluble | surface tension | 0.07435 N/m | | | dynamic viscosity | 0.004 Pa s (at 350 °C) | | 0.003 Pa s (at 250 °C) | odor | | odorless | |