What will happen if the pH of the following equilibrium system is increased?

Question

H+(aq) + 2CrO42-aq) ⇔ Cr2O72-(aq) + OH-(aq)
yellow orange

a) The solution will turn yellow.
b) The solution will turn a darker orange.
c) There will be no effect on the equilibrium system.
d) The concentration of OH-(aq) will decrease.
e) None of the above.

Answer 1

If the pH of the system is increased, it means that the concentration of OH-(aq) is increasing. According to Le Chatelier's principle, when the concentration of OH-(aq) increases, the equilibrium will shift to the left to consume some of the OH-(aq) and maintain equilibrium. As a result, the concentration of H+(aq) will increase and the concentration of Cr2O72-(aq) will decrease.

Therefore, the solution will turn a darker orange because the concentration of Cr2O72-(aq) is decreasing.

The correct answer is b) The solution will turn a darker orange.

Answer 2

are you sure?

Answer 3

I apologize for the incorrect response. Let's reevaluate the equilibrium system based on the change in pH.

When the pH of the system is increased, it means that the concentration of OH-(aq) is increasing. In the given equilibrium, the addition of OH-(aq) will react with H+(aq) to form water, shifting the equilibrium to the right. As a result, the concentration of H+(aq) will decrease and the concentration of OH-(aq) will increase.

Since the equilibrium system is moving to the right, more Cr2O72-(aq) will be formed, resulting in a darker orange color. Therefore, the correct answer is b) The solution will turn a darker orange.