🔍 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.
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