Search

HCl + (NH4)2HPO4 = H3PO4 + NH4Cl

Input interpretation

HCl hydrogen chloride + (NH_4)_2HPO_4 diammonium hydrogen phosphate ⟶ H_3PO_4 phosphoric acid + NH_4Cl ammonium chloride
HCl hydrogen chloride + (NH_4)_2HPO_4 diammonium hydrogen phosphate ⟶ H_3PO_4 phosphoric acid + NH_4Cl ammonium chloride

Balanced equation

Balance the chemical equation algebraically: HCl + (NH_4)_2HPO_4 ⟶ H_3PO_4 + NH_4Cl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 (NH_4)_2HPO_4 ⟶ c_3 H_3PO_4 + c_4 NH_4Cl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N, O and P: Cl: | c_1 = c_4 H: | c_1 + 9 c_2 = 3 c_3 + 4 c_4 N: | 2 c_2 = c_4 O: | 4 c_2 = 4 c_3 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + (NH_4)_2HPO_4 ⟶ H_3PO_4 + 2 NH_4Cl
Balance the chemical equation algebraically: HCl + (NH_4)_2HPO_4 ⟶ H_3PO_4 + NH_4Cl Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 (NH_4)_2HPO_4 ⟶ c_3 H_3PO_4 + c_4 NH_4Cl Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, N, O and P: Cl: | c_1 = c_4 H: | c_1 + 9 c_2 = 3 c_3 + 4 c_4 N: | 2 c_2 = c_4 O: | 4 c_2 = 4 c_3 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_2 = 1 and solve the system of equations for the remaining coefficients: c_1 = 2 c_2 = 1 c_3 = 1 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | 2 HCl + (NH_4)_2HPO_4 ⟶ H_3PO_4 + 2 NH_4Cl

Structures

+ ⟶ +
+ ⟶ +

Names

hydrogen chloride + diammonium hydrogen phosphate ⟶ phosphoric acid + ammonium chloride
hydrogen chloride + diammonium hydrogen phosphate ⟶ phosphoric acid + ammonium chloride

Equilibrium constant

Construct the equilibrium constant, K, expression for: HCl + (NH_4)_2HPO_4 ⟶ H_3PO_4 + NH_4Cl 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 HCl + (NH_4)_2HPO_4 ⟶ H_3PO_4 + 2 NH_4Cl 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 HCl | 2 | -2 (NH_4)_2HPO_4 | 1 | -1 H_3PO_4 | 1 | 1 NH_4Cl | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) (NH_4)_2HPO_4 | 1 | -1 | ([(NH4)2HPO4])^(-1) H_3PO_4 | 1 | 1 | [H3PO4] NH_4Cl | 2 | 2 | ([NH4Cl])^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 = ([HCl])^(-2) ([(NH4)2HPO4])^(-1) [H3PO4] ([NH4Cl])^2 = ([H3PO4] ([NH4Cl])^2)/(([HCl])^2 [(NH4)2HPO4])
Construct the equilibrium constant, K, expression for: HCl + (NH_4)_2HPO_4 ⟶ H_3PO_4 + NH_4Cl 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 HCl + (NH_4)_2HPO_4 ⟶ H_3PO_4 + 2 NH_4Cl 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 HCl | 2 | -2 (NH_4)_2HPO_4 | 1 | -1 H_3PO_4 | 1 | 1 NH_4Cl | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 2 | -2 | ([HCl])^(-2) (NH_4)_2HPO_4 | 1 | -1 | ([(NH4)2HPO4])^(-1) H_3PO_4 | 1 | 1 | [H3PO4] NH_4Cl | 2 | 2 | ([NH4Cl])^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 = ([HCl])^(-2) ([(NH4)2HPO4])^(-1) [H3PO4] ([NH4Cl])^2 = ([H3PO4] ([NH4Cl])^2)/(([HCl])^2 [(NH4)2HPO4])

Rate of reaction

Construct the rate of reaction expression for: HCl + (NH_4)_2HPO_4 ⟶ H_3PO_4 + NH_4Cl 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 HCl + (NH_4)_2HPO_4 ⟶ H_3PO_4 + 2 NH_4Cl 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 HCl | 2 | -2 (NH_4)_2HPO_4 | 1 | -1 H_3PO_4 | 1 | 1 NH_4Cl | 2 | 2 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 HCl | 2 | -2 | -1/2 (Δ[HCl])/(Δt) (NH_4)_2HPO_4 | 1 | -1 | -(Δ[(NH4)2HPO4])/(Δt) H_3PO_4 | 1 | 1 | (Δ[H3PO4])/(Δt) NH_4Cl | 2 | 2 | 1/2 (Δ[NH4Cl])/(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[HCl])/(Δt) = -(Δ[(NH4)2HPO4])/(Δt) = (Δ[H3PO4])/(Δt) = 1/2 (Δ[NH4Cl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Construct the rate of reaction expression for: HCl + (NH_4)_2HPO_4 ⟶ H_3PO_4 + NH_4Cl 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 HCl + (NH_4)_2HPO_4 ⟶ H_3PO_4 + 2 NH_4Cl 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 HCl | 2 | -2 (NH_4)_2HPO_4 | 1 | -1 H_3PO_4 | 1 | 1 NH_4Cl | 2 | 2 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 HCl | 2 | -2 | -1/2 (Δ[HCl])/(Δt) (NH_4)_2HPO_4 | 1 | -1 | -(Δ[(NH4)2HPO4])/(Δt) H_3PO_4 | 1 | 1 | (Δ[H3PO4])/(Δt) NH_4Cl | 2 | 2 | 1/2 (Δ[NH4Cl])/(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[HCl])/(Δt) = -(Δ[(NH4)2HPO4])/(Δt) = (Δ[H3PO4])/(Δt) = 1/2 (Δ[NH4Cl])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

Chemical names and formulas

| hydrogen chloride | diammonium hydrogen phosphate | phosphoric acid | ammonium chloride formula | HCl | (NH_4)_2HPO_4 | H_3PO_4 | NH_4Cl Hill formula | ClH | H_9N_2O_4P | H_3O_4P | ClH_4N name | hydrogen chloride | diammonium hydrogen phosphate | phosphoric acid | ammonium chloride
| hydrogen chloride | diammonium hydrogen phosphate | phosphoric acid | ammonium chloride formula | HCl | (NH_4)_2HPO_4 | H_3PO_4 | NH_4Cl Hill formula | ClH | H_9N_2O_4P | H_3O_4P | ClH_4N name | hydrogen chloride | diammonium hydrogen phosphate | phosphoric acid | ammonium chloride

Substance properties

| hydrogen chloride | diammonium hydrogen phosphate | phosphoric acid | ammonium chloride molar mass | 36.46 g/mol | 132.06 g/mol | 97.994 g/mol | 53.49 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | -114.17 °C | 155 °C | 42.4 °C | 340 °C boiling point | -85 °C | | 158 °C | density | 0.00149 g/cm^3 (at 25 °C) | 1.619 g/cm^3 | 1.685 g/cm^3 | 1.5256 g/cm^3 solubility in water | miscible | | very soluble | soluble odor | | odorless | odorless |
| hydrogen chloride | diammonium hydrogen phosphate | phosphoric acid | ammonium chloride molar mass | 36.46 g/mol | 132.06 g/mol | 97.994 g/mol | 53.49 g/mol phase | gas (at STP) | solid (at STP) | liquid (at STP) | solid (at STP) melting point | -114.17 °C | 155 °C | 42.4 °C | 340 °C boiling point | -85 °C | | 158 °C | density | 0.00149 g/cm^3 (at 25 °C) | 1.619 g/cm^3 | 1.685 g/cm^3 | 1.5256 g/cm^3 solubility in water | miscible | | very soluble | soluble odor | | odorless | odorless |

Units

Random Queries

alternate names of dibutyl phosphate vs hexane anion
alternate names of iron vs zinc
formula of platinum silicide vs californium
labeled hybridization diagram of scopolamine
formula of hexabromoplatinate(IV) anion
silver(I) cation vs acetate anion vs hypobromite anion vs phosphate anion
alternate names of sodium arsenate vs nickel carbonyl
2,2-bis(3-amino-4-hydroxyphenyl)hexafluoropropane
edge types of chlordecone
PubChem SID number of choline ion