15 Facts on H2SO4 + K2O: What, How To Balance & FAQs

Potassium oxide (K₂O) is the simplest oxide of potassium with a pale-yellow colour. Let us discuss how K₂O reacts with H₂SO₄ in this article.

H₂SO₄ and K₂O neutralise each other to generate a salt and release water. Sulphuric acid (H₂SO₄) is a powerful dehydrating agent of organic chemistry. It is a colourless and odourless viscous liquid. Potassium oxide (K₂O) is a highly reactive ionic compound with a basic character.

We will discuss many important facts about the H₂SO₄ + K₂O reaction, like enthalpy of formation, type of reaction and products in this article.

What is the product of H₂SO₄ and K₂O

Potassium sulphate (K₂SO₄) and Water (H₂O) are the products of H₂SO₄ and K₂O reactions. The chemical equation for this reaction is:

K₂O + H₂SO₄ = K₂SO₄ + H₂O

What type of reaction is H₂SO₄ + K₂O

H₂SO₄ + K₂O reaction is an acid-base (neutralisation) reaction. Here H₂SO₄ is acid and K₂O is a base.

How to balance H₂SO₄ + K₂O

The balanced chemical equation for H₂SO₄ + K₂O reaction is,

K₂O + H₂SO₄ = K₂SO₄ + H₂O

• The general chemical equation for the above reaction is,

• K₂O + H₂SO₄ = K₂SO₄ + H₂O

• Check if the number of atoms present on both sides of the chemical equation is equal or not.

• Here the number of atoms is equal. Therefore, the equation is already balanced.

• Thus, the balanced chemical equation is,

• K₂O + H₂SO₄ = K₂SO₄ + H₂O

H₂SO₄ + K₂O titration

H₂SO₄ + K₂O titration is an acid-base titration. Concentration of Sulphuric acid can be determined using the procedure mentioned below:

Apparatus Used:

Burette, conical flask, beaker, burette stand, pipette.

Indicator:

Phenolphthalein is the indicator used for strong acid-strong base titration. 

Procedure:

• Wash and rinse the burette with a standardised solution of K₂O and fit it in a burette stand.

• Pipette out 10mL of H₂SO₄ in the conical flask and add 2-3 drops of phenolphthalein to it.

• Start adding the K₂O solution to the conical flask in a dropwise manner.

• The colour of the solution will change from colourless to light pink when the endpoint is reached.

• Repeat the above steps to get concurrent readings.

• Contraction of sulphuric acid is found using the formula S_H2SO4V_H2SO4 = S_K2OV_K2O.

H₂SO₄ + K₂O net ionic equation

H₂SO₄ + K₂O net ionic equation is,

2H⁺ (aq.) + O^2- (aq.) = H₂O (l)

• Write the general balanced chemical equation of H₂SO₄ + K₂O.

• K₂O + H₂SO₄ = K₂SO₄ + H₂O

• Display the chemical state of every compound involved during the reaction

• K₂O (aq.) + H₂SO₄ (aq.) = K₂SO₄ (aq.) + H₂O (l)

• Split the strong electrolytes into their respective ions having positive and negative charges.

• 2H⁺ (aq.) + SO₄^2- (aq.) + 2K⁺ (aq.) + O^2- (aq.) = 2K⁺ (aq.) + SO₄^2- (aq.) + H₂O (l)

• Eliminate the spectator ions to obtain the net ionic equation.

• 2H⁺ (aq.) + O^2- (aq.) = H₂O (l)

H₂SO₄ + K₂O conjugate pairs

The pair of H₂SO₄ + K₂O itself does not have any conjugate pair.

• H₂SO₄ and HSO₄^– form a conjugate acid-base pair.

• The conjugate pair of H₂O contains its conjugate base OH^–.

H₂SO₄ + K₂O intermolecular forces

H₂SO₄ + K₂O reaction has the following intermolecular forces,

• The intermolecular forces in H₂O molecules are dipole-dipole interaction and intramolecular hydrogen bonding.

• H₂SO₄ contains London dispersion forces, dipole-dipole interaction and hydrogen bonding between their molecules.

• Ionic bonding is present in K₂SO₄ because it is an ionic compound.

H₂SO₄ + K₂O reaction enthalpy

H₂SO₄ + K₂O reaction enthalpy is -427.4 kJ/mol. The standard enthalpy of formation of compounds involved in the reaction is:

Molecules	Reaction enthalpy (in kJ/mol)
H2SO4	-909.27
K2O	-363.17
K2SO4	-1161.65
H2O	-285.83

Reaction Enthalpy ΔH_f = Standard enthalpy of products – Standard enthalpy of reactants

Thus, ΔH_f = (-1161.65 – 285.83) – (-909.27 – 363.17)

ΔH_f = -427.4 kJ/mol.

Is H₂SO₄ + K₂O a buffer solution

H₂SO₄ + K₂O is not a buffer solution because H₂SO₄ is a strong acid and we need a weak acid for a solution to act as a buffer solution.

Is H₂SO₄ + K₂O a complete reaction

H₂SO₄ + K₂O is a complete reaction and no further steps are left to proceed.

Is H₂SO₄ + K₂O an exothermic or endothermic reaction

H₂SO₄ + K₂O is an exothermic reaction because the reaction enthalpy has a negative value for the given chemical equation.

Is H₂SO₄ + K₂O a redox reaction

H₂SO₄ + K₂O is not a redox reaction because the oxidation state of atoms involved in the reaction remains unchanged throughout the chemical process.

Is H₂SO₄ + K₂O a precipitation reaction

H₂SO₄ + K₂O is not a precipitation reaction as no solid product is obtained at the end of the process.

Is H₂SO₄ + K₂O reversible or irreversible reaction

H₂SO₄ + K₂O is an irreversible reaction because the heat released during the process cannot be reverted back to the reaction mixture. 

Is H₂SO₄ + K₂O displacement reaction

H₂SO₄ + K₂O is a double displacement reaction in which H₂ and K₂ displace each other from their respective compounds to form new products.

Conclusion

This article concludes that H₂SO₄ and K₂O neutralise each other completely and form the corresponding salt. H₂SO₄ is acidic and has several laboratory and industrial importance. K₂O is one of the strongest bases known till now.