15 Facts on H2SO4 + K2CO3: What, How To Balance & FAQs

The physicochemical properties of H2SO4 and K2CO3 are researched as environmentally friendly to cure microbial activity in wastewater. Let us explore the reactions between H2SO4 + K2CO3.

The oxidation reaction between H2SO4 and K2CO3 is seen to be a solution to the removal of contaminants from water. The wastewater purifications can be extensively utilized using these chemicals.

The reactivity of H2SO4 and K2CO3 was investigated to evaluate their potential as chemical adsorbents for water purification assays. Here, we discuss a more mechanistic approach to the reactions with a detailed explanation.

1. What is the product of H2SO4 and K2CO3?

Potassium sulphate, water molecules, and bubbles of carbon dioxide gas are formed when sulphuric acid reacts with potassium carbonate.

H2SO4 + K2CO3 = K2SO4 + CO2 + H2O

2. What type of reaction is H2SO4 + K2CO3?

H2SO4 + K2CO3 is an acid-base neutralization reaction where K2CO3 is a base and H2SO4 is an acid.

3. How to balance H2SO4 + K2CO3?

We can balance the reaction K2CO3 + H2SO4 = K2SO4 + CO2 + H2O as per the following algebraic method,

  • Step 1- Each reactant and product in the equation is labeled with a variable (A, B, C, D, and E) to represent unknown coefficients.
  • A K2CO3 + B H2SO4 = C K2SO4 + D CO2 + E H2O
  • Step 2 – Now, the equation is solved by an appropriate number, considered to be the coefficient of reactants and products.
  • K = 2A = 2C, C = A = D, O = 3A + 4B = 4D +2D + E, H = 2B = 2E, S = B = C
  • Step 3- All the variables and coefficients are calculated by the Gauss elimination method, and lastly, we get
  • A = 1, B = 1, C = 1, D = 1, and E = 1
  • So, the overall balanced equation is,
  • K2CO3 + H2SO4 = K2SO4 + CO2 + H2O

4. H2SO4 + K2CO3 titration

The titration system mentioned above is an example of volumetric titration of a strong acid (H2SO4) against a strong base (K2CO3). We hereby discuss the apparatus and chemicals involved, conditions, and experimental procedures required for the titration.

Apparatus used

Burette, burette clamps, pipette, volumetric flask, conical flask, dropper, and beakers.


Methyl orange is the specific indicator used in the titration of K2CO3 and H2SO4.


  • The burette is filled with standard H2SO4 solution and K2CO3 was taken in a conical flask.
  • The titration process is started by adding H2SO4 dropwise to the conical flask and the flask was shaken continuously.
  • Methyl orange is chosen as an indicator that starts to change from yellow to orange when the reaction reaches the equivalence point.
  • The experiment is repeated concordantly for accurate results
  • The strength of H2SO4 is estimated using the formulae
  • S2 = (V1 * S1)/V2 where S2 is the strength of the acid, V1 is the volume of base added, and S1 is the strength of the base and V2 is the volume of the acid used.

5. H2SO4 + K2CO3 net ionic equation

The net ionic equation of K2CO3 + H2SO4 is

CO3-2 (aq)+ 2H+ (aq)= CO2 (g) + H2O (aq)

Following steps are used to derive the net ionic equation:

  • Firstly, write the balanced chemical equation and represent the physical states of reactants and products
  • K2CO3 (s) + H2SO4 (aq) = K2SO4 (s) + CO2 (g) + H2O (aq)
  • Now, strong acids, bases and salts dissociates into ions whereas the pure solid substances and molecules do not dissociate
  • CO3-2 (aq)+ 2H+ (aq)= CO2 (g) + H2O (aq)

6. H2SO4 + K2CO3 conjugate pairs

  • H2SO4 can exist as conjugate pair of HSO4.
  • K2CO3 can not form a conjugate pair due to absence of proton.

7. H2SO4 and K2CO3 intermolecular forces

8. H2SO4 + K2CO3 reaction enthalpy

K2CO3 + H2SO4 show reaction enthalpy of -967.20 kJ/mol.

9. Is H2SO4 + K2CO3 a buffer solution?

K2CO3 + H2SO4 do not form a buffer solution as strong acids do not form a buffer.

10. Is H2SO4 + K2CO3 a complete reaction?

K2CO3 + H2SO4 is a complete reaction as stable products namely potassium sulphate, water, and carbon dioxide are formed as products.

11. Is H2SO4 + K2CO3 an exothermic or endothermic reaction?

K2CO3 + H2SO4 is an exothermic reaction because the enthalpy rate is observed to be negative.

12. Is H2SO4 + K2CO3 a redox reaction?

K2CO3 + H2SO4 do not show a redox reaction as reduction and oxidation of compounds do not occur.

13. Is H2SO4 + K2CO3 a precipitation reaction?

K2CO3 + H2SO4 is not a precipitation reaction as no precipitates are observed at the end of the reactions.

14. Is H2SO4 + K2CO3 reversible or irreversible reaction?

K2CO3 + H2SO4 is irreversible reaction because the formed products cannot be converted back into the original reactants.

15. Is H2SO4 + K2CO3 displacement reaction?

K2CO3 + H2SO4 is a displacement reaction as double displacement of molecules from the reactants were observed.


The reaction of sulphuric acid with potassium carbonate is an example of a carbonate acid reaction or neutralization reaction where an acid and a base react to form salt and water. Also, bubbles of carbon dioxide are produced in the reaction. The reaction is also an important solution for wastewater purifications.

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