15 Facts on HCl + Na2PO4: What, How To Balance & FAQs

Hydrochloric acid is a strong acid. In contrast, sodium phosphate is a salt with a strong base, i.e., sodium hydroxide. Let us study how HCl and Na₂PO₄ react.

HCl + Na₂PO₄ react to give salt metathesis reaction. HCl is an aqueous solution of hydrogen chloride. It dissociates readily to give proton and chloride anions. In contrast, sodium phosphate is a dibasic compound. It is an inexpensive, non-toxic compound commonly used for baked goods.

In this article, we will study the type, product, and balancing of the HCl + Na₂PO₄ reaction.

What is the product of HCl and Na₂PO₄?

HCl and Na₂PO₄ react to form sodium chloride and dihydrogen phosphate.

Na₂PO₄ + 2HCl → 2NaCl + H₂PO₄

What type of Reaction is HCl + Na₂PO₄

The HCl + Na₂PO₄ is a double displacement reaction as the cation and anion of the two ionic compounds exchange bonds to create 2 new compounds with nearby or equivalent bonding affiliations.

How to Balance HCl + Na₂PO₄

The equations is balanced by a hit-and-trial method as follows. 

• To balance HCl + Na₂PO₄ equation, we will balance the number of sodium atoms both in reactant and product side.
• Na₂PO₄ + HCl → 2NaCl + H₂PO₄

• Now, we will balance the number of chlorine atoms.
• Na₂PO₄ + 2HCl → 2NaCl + H₂PO₄

• Next, we will balance the oxygen and hydrogen atoms as we can see that the number of hydrogen and oxygen is already balanced.
• Thus, we can conclude that the above equation is a required balance equation.
• Na₂PO₄ + 2HCl → 2NaCl + H₂PO₄

HCl + Na₂PO₄ Titration

HCl + Na₂PO₄ does not undergo titration as no equivalence point is observed during the reaction.

HCl + Na₂PO₄ Net Ionic Equation

The net ionic equation of HCl + Na₂PO₄ is PO₄^-3 + 2H⁺ → H₂PO₄. We will follow the following steps to calculate the net ionic equation.

• To calculate the net ionic equation of HCl + Na₂PO₄, the balanced equation is written first.
• Na₂PO₄ + 2HCl → 2NaCl + H₂PO₄

• The total ionic equation for the balanced equation is as follows:
• 2Na⁺ + PO₄^-3 + 2H⁺ + 2Cl^– → 2Na⁺ + 2Cl^– + H₂PO₄

• Hence, the net equation is:
• PO₄^-3 + 2H⁺ → H₂PO₄

HCl + Na₂PO₄ Conjugate Pairs

• The conjugate pair of hydrochloric acid is Cl^–.
• There is no conjugate pair of Na₂PO₄ because of the absence of protons in sodium phosphate.

HCl and Na₂PO₄ Intermolecular Forces

• Dipole-dipole intermolecular force is present between the molecule of hydrochloric acid.
• There is an electrostatic force of attraction between molecules of sodium phosphate.

HCl + Na₂PO₄ Reaction Enthalpy

The reaction enthalpy data of HCl + Na₂PO₄ is not available in literature.

Is HCl + Na₂PO₄ a Buffer Solution

HCl + Na₂PO₄ is not a buffer solution as it contains strong hydrochloric acid(HCl) and a weak acid salt, sodium phosphate (Na₂PO₄).

Is HCl + Na₂PO₄ a Complete Reaction

HCl + Na₂PO₄ is a complete reaction as no reactant is left at the end of reaction.

Na₂PO₄ + 2HCl → 2NaCl + H₂PO₄

Is HCl + Na₂PO₄ an Exothermic Reaction

The reaction between HCl and Na₂PO₄ is an exothermic reaction as the value of delta G is negative.

Is HCl + Na₂PO₄ a Redox Reaction

The HCl + Na₂PO₄ is not a redox reaction, as the oxidation state of the substrate remains unchanged.

Is HCl + Na₂PO₄ a Precipitation Reaction

The HCl + Na₂PO₄ is not a precipitation reaction as no insoluble salt is formed during the reaction.

Na₂PO₄ + 2HCl → No precipitate

Is HCl + Na₂PO₄ Irreversible Reaction

The HCl + Na₂PO₄ is an irreversible reaction as it is a unidirectional reaction thus can not extract the reactants from the products.

Is HCl + Na₂PO₄ Displacement Reaction

The HCl + Na₂PO₄ is a displacement reaction because sodium ion displaces the hydrogen ion from hydrochloric acid to form sodium chloride. And the phosphate ion displaces chloride ion from hydrochloric acid to form phosphoric acid.

Na₂PO₄ + 2HCl → 2NaCl + H₂PO₄

Conclusion 

Sodium phosphate (Na₂PO₄), reacts with hydrochloric acid to give a double displacement reaction forming sodium chloride (NaCl) and dihydrogen phosphate (H₂PO₄). It is an irreversible reaction, and the oxidation state of the substrate remains unchanged during the reaction.