15 Facts on H2SO3 + BaCl2: What, How To Balance & FAQs

H₂SO₃ (sulfurous acid) is a weak acid. BaCl₂ is neither acidic nor basic. It is a salt with no charge. Let us examine the reaction between H₂SO₃ and BaCl₂ in this article.

H₂SO₃ is a colorless liquid with a strong, burning sulfur odor. H₂SO₃ is an oxoacid of sulfur. It is a hydrogen sulfite conjugate acid. Barium chloride is an inorganic salt. Barium muriate or barium dichloride is another name for it. It is a white solid that is hygroscopic and soluble in water.

This article discusses how to balance the H₂SO₃ and BaCl₂ reaction, the product of the reaction, the reaction enthalpy, the type of reaction, the buffer solution, and many other aspects of the H₂SO₃ + BaCl₂ reaction.

What is the product of H₂SO₃ and BaCl₂?

When H₂SO₃ and BaCl₂ react, they produce Barium Sulfite (BaSO₃) and Hydrogen chloride (HCl) molecules. The following is the reaction equation,

BaCl₂ + H₂SO₃ → BaSO₃ + 2HCl

What type of reaction is H₂SO₃ + BaCl₂?

The reaction of H₂SO₃ + BaCl₂ is a double displacement reaction.

How to balance H₂SO3 + BaCl₂?

The following are the steps for equating the H₂SO₃ + BaCl₂ reaction scheme:

• Using stoichiometry, multiply HCl by two to balance the reactant side

• BaCl₂ + H₂SO₃ → BaSO₃ + HCl

• Since the reactant side contains two hydrogen atoms, multiply HCl by two.

• H₂SO₃ + BaCl₂→ BaSO₃ + 2HCl

• The reactant and product sides are now equal. On both sides, there are two hydrogens, three oxygens, two chlorines, and one sulfur atom.

• H₂SO₃ + BaCl₂→ BaSO₃ + 2HCl

H₂SO₃ + BaCl₂ titration

H₂SO₃ and BaCl₂ cannot be titrated. Because BaCl₂ was hardly acidic or basic, it is a salt without charge, and H₂SO₃ is a weak acid.

H₂SO₃ + BaCl₂ net ionic equation

For the given reaction of H₂SO₃ and BaCl₂, the net ionic equation is,

H₂SO₃ + BaCl₂→ BaSO₃ + 2HCl

• The molecular equation should be balanced, and each compound’s phase should be included.

• H₂SO_{3 (aq)} + BaCl_{2 (aq)} → BaSO_{3 (s)} + 2HCl _(l)

• In the equation, the aqueous salts or chemicals must be converted into ions.
• Weak electrolytes and solids cannot be split apart. Here, H₂SO₃ is a weak electrolyte, and BaCl₂ is solid.
• H₂SO_{3 (aq)} + Ba²⁺ + 2Cl^–  → BaSO_{3 (s)} + 2H⁺ + 2Cl^–
• Remove the ions that are similar on both sides of the complete ionic equation.
• As a result, the net ionic equation is,
• H₂SO_{3 (aq) )} + Ba²⁺ → BaSO_{3 (s)} + 2H⁺

 H₂SO₃ + BaCl₂ conjugate pairs

The H₂SO₃ + BaCl₂ reaction produces the following conjugate pairs:

• When H₂SO₃ donates its H⁺ ion, the resulting compound is HSO3^–, which acts as a conjugate base.
• BaCl₂ was neither acidic nor basic; it is a salt with no charge. As a result, it will not produce conjugate pairs.

H₂SO₃ and BaCl₂ intermolecular forces

In the case of H₂SO₃ and BaCl_2,

• Ionic bonds keep Ba²⁺ and Cl^– together in BaCl₂. And since ionic bonds are more powerful than dipole interactions, BaCl₂ has a higher boiling point.
• The intermolecular force is caused by the strong electrostatic force between protons and sulfite ions in H₂SO₃, which also has hydrogen bonding.

H₂SO₃ + BaCl₂ reaction enthalpy

The enthalpy data for the H₂SO₃ + BaCl₂ reaction are as follows:

• Reaction enthalpy of H₂SO₃ is 108.5 kJ
• The enthalpy change of BaCl₂.2H₂O solution is 8.8 kJ/mol and -20.6 kJ/mol for BaCl₂.

Is H₂SO₃ + BaCl₂ a buffer solution?

H₂SO₃ + BaCl₂ is not a buffer solution. Because

• H₂SO₃ is a weak acid capable of producing two H⁺ ions.
• Barium chloride is a salt. It has no acidic or basic properties. As a result, it is ineffective as a buffer.
• Buffer solutions are high in a weak acid and its conjugate base (or a weak base and its conjugate acid). Buffers are highly resistant to changes in pH because these components can neutralize added H⁺ or OH^–.

Is H₂SO₃ + BaCl₂ a complete reaction?

H₂SO₃ + BaCl₂ is not a complete reaction. The formation of barium sulfite salt makes the reaction irreversible in nature. However, due to its low acidity, H₂SO₃ cannot be completely dissociated.

Is H₂SO₃ + BaCl₂ an exothermic or endothermic reaction?

The reaction between H₂SO₃ and BaCl₂ is exothermic in nature because heat is produced during the reaction. In order for the reaction to take place, more energy must be absorbed than is released when salt is formed.

Is H₂SO₃ + BaCl₂ a redox reaction?

The reaction H₂SO₃ + BaCl₂ is not a redox reaction. The oxidation state of elements does not change (H, S, Ba, O, and Cl). Throughout the reaction, the oxidation state has been maintained.

Is H₂SO₃ + BaCl₂ a precipitation reaction?

The reaction H₂SO₃ + BaCl₂ results in the formation of a white precipitate of barium sulfite, which is insoluble in water, and even sulfurous acid.

Is H₂SO₃ + BaCl₂ reversible or irreversible reaction?

The reaction H₂SO₃ + BaCl₂ is irreversible. Because the formation of barium sulfite salt results in a white precipitate, the reaction cannot be reversed.

Is H₂SO₃ + BaCl₂ displacement reaction?

H₂SO₃ + BaCl₂ is a double displacement reaction.  When HCl molecules are formed, the barium ion in barium chloride is displaced by the hydrogen ion, resulting in the formation of barium sulfite.

Conclusion

The reaction between H₂SO₃ + BaCl₂ is a double displacement reaction. The anhydrous form of BaCl₂ is crystalline, orthorhombic, and monoclinic. It is used in the papermaking industry as well as steel hardening. H₂SO₃ is used in the production of fertilizers, pigments, dyes, detergents, etc.