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H3PO4 + Ca(NO3)2 = HNO3 + Ca3(PO4)2

Input interpretation

H_3PO_4 phosphoric acid + Ca(NO_3)_2 calcium nitrate ⟶ HNO_3 nitric acid + Ca_3(PO_4)_2 tricalcium diphosphate
H_3PO_4 phosphoric acid + Ca(NO_3)_2 calcium nitrate ⟶ HNO_3 nitric acid + Ca_3(PO_4)_2 tricalcium diphosphate

Balanced equation

Balance the chemical equation algebraically: H_3PO_4 + Ca(NO_3)_2 ⟶ HNO_3 + Ca_3(PO_4)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_3PO_4 + c_2 Ca(NO_3)_2 ⟶ c_3 HNO_3 + c_4 Ca_3(PO_4)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, P, Ca and N: H: | 3 c_1 = c_3 O: | 4 c_1 + 6 c_2 = 3 c_3 + 8 c_4 P: | c_1 = 2 c_4 Ca: | c_2 = 3 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 3 c_3 = 6 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_3PO_4 + 3 Ca(NO_3)_2 ⟶ 6 HNO_3 + Ca_3(PO_4)_2
Balance the chemical equation algebraically: H_3PO_4 + Ca(NO_3)_2 ⟶ HNO_3 + Ca_3(PO_4)_2 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_3PO_4 + c_2 Ca(NO_3)_2 ⟶ c_3 HNO_3 + c_4 Ca_3(PO_4)_2 Set the number of atoms in the reactants equal to the number of atoms in the products for H, O, P, Ca and N: H: | 3 c_1 = c_3 O: | 4 c_1 + 6 c_2 = 3 c_3 + 8 c_4 P: | c_1 = 2 c_4 Ca: | c_2 = 3 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_4 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 3 c_3 = 6 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 H_3PO_4 + 3 Ca(NO_3)_2 ⟶ 6 HNO_3 + Ca_3(PO_4)_2

Structures

+ ⟶ +
+ ⟶ +

Names

phosphoric acid + calcium nitrate ⟶ nitric acid + tricalcium diphosphate
phosphoric acid + calcium nitrate ⟶ nitric acid + tricalcium diphosphate

Equilibrium constant

Construct the equilibrium constant, K, expression for: H_3PO_4 + Ca(NO_3)_2 ⟶ HNO_3 + Ca_3(PO_4)_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 H_3PO_4 + 3 Ca(NO_3)_2 ⟶ 6 HNO_3 + Ca_3(PO_4)_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 H_3PO_4 | 2 | -2 Ca(NO_3)_2 | 3 | -3 HNO_3 | 6 | 6 Ca_3(PO_4)_2 | 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 | 2 | -2 | ([H3PO4])^(-2) Ca(NO_3)_2 | 3 | -3 | ([Ca(NO3)2])^(-3) HNO_3 | 6 | 6 | ([HNO3])^6 Ca_3(PO_4)_2 | 1 | 1 | [Ca3(PO4)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 = ([H3PO4])^(-2) ([Ca(NO3)2])^(-3) ([HNO3])^6 [Ca3(PO4)2] = (([HNO3])^6 [Ca3(PO4)2])/(([H3PO4])^2 ([Ca(NO3)2])^3)
Construct the equilibrium constant, K, expression for: H_3PO_4 + Ca(NO_3)_2 ⟶ HNO_3 + Ca_3(PO_4)_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 H_3PO_4 + 3 Ca(NO_3)_2 ⟶ 6 HNO_3 + Ca_3(PO_4)_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 H_3PO_4 | 2 | -2 Ca(NO_3)_2 | 3 | -3 HNO_3 | 6 | 6 Ca_3(PO_4)_2 | 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 | 2 | -2 | ([H3PO4])^(-2) Ca(NO_3)_2 | 3 | -3 | ([Ca(NO3)2])^(-3) HNO_3 | 6 | 6 | ([HNO3])^6 Ca_3(PO_4)_2 | 1 | 1 | [Ca3(PO4)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 = ([H3PO4])^(-2) ([Ca(NO3)2])^(-3) ([HNO3])^6 [Ca3(PO4)2] = (([HNO3])^6 [Ca3(PO4)2])/(([H3PO4])^2 ([Ca(NO3)2])^3)

Rate of reaction

Construct the rate of reaction expression for: H_3PO_4 + Ca(NO_3)_2 ⟶ HNO_3 + Ca_3(PO_4)_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 H_3PO_4 + 3 Ca(NO_3)_2 ⟶ 6 HNO_3 + Ca_3(PO_4)_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 H_3PO_4 | 2 | -2 Ca(NO_3)_2 | 3 | -3 HNO_3 | 6 | 6 Ca_3(PO_4)_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 H_3PO_4 | 2 | -2 | -1/2 (Δ[H3PO4])/(Δt) Ca(NO_3)_2 | 3 | -3 | -1/3 (Δ[Ca(NO3)2])/(Δt) HNO_3 | 6 | 6 | 1/6 (Δ[HNO3])/(Δt) Ca_3(PO_4)_2 | 1 | 1 | (Δ[Ca3(PO4)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[H3PO4])/(Δt) = -1/3 (Δ[Ca(NO3)2])/(Δt) = 1/6 (Δ[HNO3])/(Δt) = (Δ[Ca3(PO4)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: H_3PO_4 + Ca(NO_3)_2 ⟶ HNO_3 + Ca_3(PO_4)_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 H_3PO_4 + 3 Ca(NO_3)_2 ⟶ 6 HNO_3 + Ca_3(PO_4)_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 H_3PO_4 | 2 | -2 Ca(NO_3)_2 | 3 | -3 HNO_3 | 6 | 6 Ca_3(PO_4)_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 H_3PO_4 | 2 | -2 | -1/2 (Δ[H3PO4])/(Δt) Ca(NO_3)_2 | 3 | -3 | -1/3 (Δ[Ca(NO3)2])/(Δt) HNO_3 | 6 | 6 | 1/6 (Δ[HNO3])/(Δt) Ca_3(PO_4)_2 | 1 | 1 | (Δ[Ca3(PO4)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[H3PO4])/(Δt) = -1/3 (Δ[Ca(NO3)2])/(Δt) = 1/6 (Δ[HNO3])/(Δt) = (Δ[Ca3(PO4)2])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| phosphoric acid | calcium nitrate | nitric acid | tricalcium diphosphate formula | H_3PO_4 | Ca(NO_3)_2 | HNO_3 | Ca_3(PO_4)_2 Hill formula | H_3O_4P | CaN_2O_6 | HNO_3 | Ca_3O_8P_2 name | phosphoric acid | calcium nitrate | nitric acid | tricalcium diphosphate IUPAC name | phosphoric acid | calcium dinitrate | nitric acid | tricalcium diphosphate
| phosphoric acid | calcium nitrate | nitric acid | tricalcium diphosphate formula | H_3PO_4 | Ca(NO_3)_2 | HNO_3 | Ca_3(PO_4)_2 Hill formula | H_3O_4P | CaN_2O_6 | HNO_3 | Ca_3O_8P_2 name | phosphoric acid | calcium nitrate | nitric acid | tricalcium diphosphate IUPAC name | phosphoric acid | calcium dinitrate | nitric acid | tricalcium diphosphate

Substance properties

| phosphoric acid | calcium nitrate | nitric acid | tricalcium diphosphate molar mass | 97.994 g/mol | 164.09 g/mol | 63.012 g/mol | 310.17 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | melting point | 42.4 °C | 562 °C | -41.6 °C | boiling point | 158 °C | | 83 °C | density | 1.685 g/cm^3 | 2.5 g/cm^3 | 1.5129 g/cm^3 | 3.14 g/cm^3 solubility in water | very soluble | soluble | miscible | dynamic viscosity | | | 7.6×10^-4 Pa s (at 25 °C) | odor | odorless | | |
| phosphoric acid | calcium nitrate | nitric acid | tricalcium diphosphate molar mass | 97.994 g/mol | 164.09 g/mol | 63.012 g/mol | 310.17 g/mol phase | liquid (at STP) | solid (at STP) | liquid (at STP) | melting point | 42.4 °C | 562 °C | -41.6 °C | boiling point | 158 °C | | 83 °C | density | 1.685 g/cm^3 | 2.5 g/cm^3 | 1.5129 g/cm^3 | 3.14 g/cm^3 solubility in water | very soluble | soluble | miscible | dynamic viscosity | | | 7.6×10^-4 Pa s (at 25 °C) | odor | odorless | | |

Units

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