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gracy
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Chromate and dichromate ions in equilibrium
- Thread starter gracy
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- Equilibrium Ions
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SUMMARY
The equilibrium between potassium dichromate (K2Cr2O7) and potassium chromate (K2CrO4) involves the presence of water in the dichromate ion equation but not in the chromate ion equation. This discrepancy arises from the stoichiometry of the reaction, where the dichromate ion includes water molecules, while the chromate ion balances with hydrogen cations (H+). Both potassium dichromate and potassium chromate are soluble in water, contradicting initial assumptions about their solubility affecting the equilibrium.
PREREQUISITES- Understanding of chemical equilibrium principles
- Knowledge of solubility rules in aqueous solutions
- Familiarity with stoichiometry in chemical reactions
- Basic concepts of ionization in water
- Research the solubility of potassium dichromate and potassium chromate in detail
- Study the principles of chemical equilibrium and Le Chatelier's principle
- Learn about the stoichiometric calculations in redox reactions
- Explore the role of water in chemical reactions and ion formation
Chemistry students, educators, and professionals interested in chemical equilibria, solubility, and stoichiometric relationships in aqueous solutions.
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No.gracy said:
Both are water soluble. This won't get you anywhere.gracy said:
Ignore the notes in red in the chemical equation and just look at the stoichiometry between the right and left hand sides, counting H, O, and water.
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