13 Facts on H2SO3 + NaHCO3: What, How to Balance & FAQs

NaHCO₃ and H₂SO₃ are known as Sodium bicarbonate and Sulfurous acid respectively. These inorganic compound reactions will be discussed here. Let us know more about their reaction.

H₂SO₃ (Sulfurous acid) is a colourless liquid having a strong smell. While NaHCO₃ ( Sodium bicarbonate/Nahcolite) also known as baking soda is a crystalline white solid used in baking, and even in little extent in chemical fire extinguishers.

Here we will study more about the reaction between NaHCO₃+H₂SO₃, the type of reaction, buffer solution, the product formed, conjugate pair, and much more.

What is the product of H₂SO₃ and NaHCO₃

Sodium sulfite and Carbonic acid are formed as products when sulfurous acid reacts with sodium bicarbonate (Nahcolite). The reaction is presented below:-
2NAHCO₃ + H₂SO₃ —> Na₂SO₃ + 2HHCO₃

What type of reaction is H₂SO₃ + NaHCO₃

The reaction between H₂SO₃ and NaHCO₃ is a double displacement reaction.

How to balance H₂SO₃ + NaHCO₃

The general reaction is H₂SO₃ + 2NaHCO₃ —> Na₂SO₃+2HHCO₃ which is balanced.
Calculate the number of moles of each element involved in both the reactant and product side of the reaction.

Element	Reactant side	Product side
Na	2	2
H	4	4
C	2	2
O	9	9
S	1	1

• It can be balanced by labeling each compound with a variable.
• Solve for the variable.
• Substitution and equating both sides.
• And the thus balanced reaction is obtained.
As the number of each element in the reactant side and product is equal the reaction is balanced.

H₂SO₃ + NaHCO₃ net ionic equation

• The net ionic equation between NaHCO₃+H₂SO₃ is –
• 2NaHCO_3(aq)+H₂SO_3(aq)—> Na₂SO_3(aq) + 2HHCO_3(aq)
• These steps are involved to derive the net ionic equation:
• To write the balanced molecular equation along with the physical state.
• Then the ionic form of each of them existing in an aqueous form and is capable of forming dissociation is mentioned.
• The complete ionic equation is as given-
• 2Na⁺(aq)+ 2HCO₃(aq)+2H⁺(aq)+SO₃^2-(aq)—> 2Na+(aq)+SO₃^2-(aq)+4H⁺(aq)+2CO₃^2-(aq)
• The balanced ionic reaction has only those species which are involved in the reaction. The ions found on both sides are removed and the net ionic equation is derived.
• 2HCO₃^–_(aq)—>2H⁺_(aq)+2CO₃^2-

Is H₂SO₃+NaHCO₃ conjugate pairs

H₂SO₃ and NaHCO₃ are both conjugate acid-base pair.

• The conjugate base of H₂SO₃ is HSO₃^–( bisulfite anion).
• The conjugate base of NaHCO₃ is H₂CO₃(carbonic acid).

H₂SO₃ and NaHCO₃ intermolecular forces

The intermolecular forces in H₂SO₃ are London dispersion forces, Van der Waals forces, and dipole-dipole interactions. NaHCO₃ has an ionic bond between Na⁺ and HCO₃^–.

H₂SO₃ + NaHCO₃ reaction enthalpy

The standard reaction enthalpy of the reaction between H₂SO₃ and NaHCO₃ is negative.

Is H₂SO₃+NaHCO₃ a buffer solution

H₂SO₃+NaHCO₃ is a buffer solution. As the reaction includes a weak acid and weak base which marks it as a buffer.

Is H₂SO₃ + NaHCO₃ a complete reaction

H₂SO₃ + NaHCO₃ is not a complete reaction. Due to H₂SO₃ being a weak acid remains in the reaction.

Is H₂SO₃ + NaHCO₃ an exothermic or endothermic reaction

H₂SO₃ + NaHCO₃ is an exothermic reaction as the energy is the result of combustion in the form of Carbon dioxide and water vapours. As the energy is given out during the reaction it is exothermic in nature.

Is H₂SO₃+NaHCO₃ a redox reaction

The reaction between H₂SO₃+NaHCO₃ is not a redox reaction, as the oxidation state of elements remains unchanged during the reaction.

Is H₂SO₃ +NaHCO₃ a precipitation reaction

H₂SO₃ +NaHCO₃ is a precipitation reaction as the product formed is a white crystalline precipitate of sodium sulphite, which is insoluble in water.

Is H₂SO₃+NaHCO₃ displacement reaction

The reaction between H₂SO₃ + NaHCO₃ is a double displacement reaction, because the anions and cations exchange leading formation of salt.

Conclusion

Nahcolite also known as mineral carbonate of Sodium bicarbonate is used as a buffering agent. It has predominant use in baking. An aqueous solution of SO₂ often called Sulfurous acid is used in many industries such as fertilizer, dyes, and also in the metallurgical and petrol refining process.