Le Chatelier's principle: when a force is applied to a system in equilibrium, it tends to readjust itself in order to reduce the effects of that force.
Changes in acidity and basicity act as external forces on chemical balances. The system then needs to move to mitigate the effects of this force. Let's look at an example of a factor that can change the balance of a system, concentration.
2 CrO2-4(aq) + 2 H+(here) ↔ CrO2-7(here)+ H2O (1)
If we add a few drops of lemon (acid solution) in this balance, it will shift to the right or to the left and favor the formation of one of the products.
This is because through this action we increase the amount of H+ ions in one of the members of the equation. If this occurs in the reactants on the left, the balance shifts to the right to balance itself.
The reaction can be reversed if we add a basic NaOH solution to the system. The presence of OH- ions consumes the H+ ions and the balance shifts to the left.
Conclusion: When the ion concentration (CrO2-7) prevails, the balance shifts to the left. If the ion concentration (CrO
Do not stop now... There's more after the advertising ;)
By Líria Alves
Graduated in Chemistry
Would you like to reference this text in a school or academic work? Look:
FOGAÇA, Jennifer Rocha Vargas. "Principle of Le Chatelier"; Brazil School. Available in: https://brasilescola.uol.com.br/quimica/principio-le-chatelier.htm. Accessed on June 28, 2021.
