The Effect of Dilution on Equilibrium - Le Chatelier’s Principle

🔍 Diluting an equilibrium mixture decreases the concentration of ions and disrupts the equilibrium.

⚖️ Le Chatelier's Principle states that the equilibrium will shift to favor the reaction with more dissolved ions.

▶️ In the given reaction mixture, dilution favors the dissociation of HNO2.

🔑 Dilution does not affect the equilibrium constant value.

📈 Dilution changes the shape of the concentration-time graph.

⬇️ Higher concentration substances are more impacted by dilution.

⇄ When a solution is diluted, the equilibrium of the reaction shifts to the left, favoring the formation of Fe3+ and SCN- ions.

↗️ Although the concentration of Fe3+ and SCN- ions increases slightly after dilution, it is still lower than the original concentration.

↘️ However, the concentration of iron III thiocyanate ion decreases because the reverse reaction is favored.

🔁 By adding more water, the equilibrium shifts to the left, favoring the reverse reaction and increasing the number of dissolved ions to oppose dilution.

⬇️ When the equilibrium mixture is diluted, there is a sudden drop in concentration for both reactants and products due to more dissolved ions on the reactants, indicating a shift to the left.

🔵 At equilibrium, the reaction mixture is blue.

🔵 Diluting the sample of cobalt chloride causes a change in color from blue to paler blue.

⬅️ Adding water decreases the concentration of ions, causing the equilibrium to shift to the left.

🌸 The concentration of cobalt chloride ion decreases, while the concentration of chloride and cobalt water complex increases slightly, resulting in a more pink or paler blue color.