NaOH + Mg(NO3)2 = NaNO3 + Mg(OH)2

NaOH sodium hydroxide + Mg(NO_3)_2 magnesium nitrate ⟶ NaNO_3 sodium nitrate + Mg(OH)_2 magnesium hydroxide

Balance the chemical equation algebraically: NaOH + Mg(NO_3)_2 ⟶ NaNO_3 + Mg(OH)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 NaOH + c_2 Mg(NO_3)_2 ⟶ c_3 NaNO_3 + c_4 Mg(OH)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, Na, O, Mg and N: H: | c_1 = 2 c_4 Na: | c_1 = c_3 O: | c_1 + 6 c_2 = 3 c_3 + 2 c_4 Mg: | c_2 = c_4 N: | 2 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 2 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 NaOH + Mg(NO_3)_2 ⟶ 2 NaNO_3 + Mg(OH)_2

+ ⟶ +

sodium hydroxide + magnesium nitrate ⟶ sodium nitrate + magnesium hydroxide

| sodium hydroxide | magnesium nitrate | sodium nitrate | magnesium hydroxide molecular enthalpy | -425.8 kJ/mol | -790.7 kJ/mol | -467.9 kJ/mol | -924.5 kJ/mol total enthalpy | -851.6 kJ/mol | -790.7 kJ/mol | -935.8 kJ/mol | -924.5 kJ/mol | H_initial = -1642 kJ/mol | | H_final = -1860 kJ/mol | ΔH_rxn^0 | -1860 kJ/mol - -1642 kJ/mol = -218 kJ/mol (exothermic) | | |

| sodium hydroxide | magnesium nitrate | sodium nitrate | magnesium hydroxide molecular free energy | -379.7 kJ/mol | -589.4 kJ/mol | -366 kJ/mol | -833.5 kJ/mol total free energy | -759.4 kJ/mol | -589.4 kJ/mol | -732 kJ/mol | -833.5 kJ/mol | G_initial = -1349 kJ/mol | | G_final = -1566 kJ/mol | ΔG_rxn^0 | -1566 kJ/mol - -1349 kJ/mol = -216.7 kJ/mol (exergonic) | | |

Construct the equilibrium constant, K, expression for: NaOH + Mg(NO_3)_2 ⟶ NaNO_3 + Mg(OH)_2 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: 2 NaOH + Mg(NO_3)_2 ⟶ 2 NaNO_3 + Mg(OH)_2 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 | 2 | -2 Mg(NO_3)_2 | 1 | -1 NaNO_3 | 2 | 2 Mg(OH)_2 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression NaOH | 2 | -2 | ([NaOH])^(-2) Mg(NO_3)_2 | 1 | -1 | ([Mg(NO3)2])^(-1) NaNO_3 | 2 | 2 | ([NaNO3])^2 Mg(OH)_2 | 1 | 1 | [Mg(OH)2] 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])^(-2) ([Mg(NO3)2])^(-1) ([NaNO3])^2 [Mg(OH)2] = (([NaNO3])^2 [Mg(OH)2])/(([NaOH])^2 [Mg(NO3)2])

Construct the rate of reaction expression for: NaOH + Mg(NO_3)_2 ⟶ NaNO_3 + Mg(OH)_2 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: 2 NaOH + Mg(NO_3)_2 ⟶ 2 NaNO_3 + Mg(OH)_2 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 | 2 | -2 Mg(NO_3)_2 | 1 | -1 NaNO_3 | 2 | 2 Mg(OH)_2 | 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 | 2 | -2 | -1/2 (Δ[NaOH])/(Δt) Mg(NO_3)_2 | 1 | -1 | -(Δ[Mg(NO3)2])/(Δt) NaNO_3 | 2 | 2 | 1/2 (Δ[NaNO3])/(Δt) Mg(OH)_2 | 1 | 1 | (Δ[Mg(OH)2])/(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 = -1/2 (Δ[NaOH])/(Δt) = -(Δ[Mg(NO3)2])/(Δt) = 1/2 (Δ[NaNO3])/(Δt) = (Δ[Mg(OH)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| sodium hydroxide | magnesium nitrate | sodium nitrate | magnesium hydroxide formula | NaOH | Mg(NO_3)_2 | NaNO_3 | Mg(OH)_2 Hill formula | HNaO | MgN_2O_6 | NNaO_3 | H_2MgO_2 name | sodium hydroxide | magnesium nitrate | sodium nitrate | magnesium hydroxide IUPAC name | sodium hydroxide | magnesium dinitrate | sodium nitrate | magnesium dihydroxide

| sodium hydroxide | magnesium nitrate | sodium nitrate | magnesium hydroxide molar mass | 39.997 g/mol | 148.31 g/mol | 84.994 g/mol | 58.319 g/mol phase | solid (at STP) | solid (at STP) | solid (at STP) | solid (at STP) melting point | 323 °C | 88.9 °C | 306 °C | 350 °C boiling point | 1390 °C | 330 °C | | density | 2.13 g/cm^3 | 1.2051 g/cm^3 | 2.26 g/cm^3 | 2.3446 g/cm^3 solubility in water | soluble | | soluble | insoluble surface tension | 0.07435 N/m | | | dynamic viscosity | 0.004 Pa s (at 350 °C) | | 0.003 Pa s (at 250 °C) |