Question

What would happen to a weak base dissociation equilibrium if more products
were added?
A. The equilibrium constant would shift to a new constant
O
B. The concentration of reactants would increase.
O
C. The equilibrium concentrations would stay the same,
D. The concentration of products would increase

Answer 1

Answer:

Both B and D are correct.

Explanation:

B + H₂O ⇌ BH⁺ + OH⁻

If you add more products, the position of equilibrium will shift to the left to decrease their concentrations (Le Châtelier's Principle). The concentration of reactants will increase, but the equilibrium concentrations of products will also be higher than they were initially.

A is wrong. The equilibrium constant is a constant. It does not change when you change concentrations.

C is wrong. Per Le Châtelier's Principle, the concentrations must change when you ad a stress to a system at equilibrium.

(This is a poorly-worded question. "They" are probably expecting answer D.)

Answer 2

The equilibrium constant would shift to a new constant this would happen to a weak base dissociation equilibrium if more products were added.

Hence, Option (A) is correct answer.

What is a weak base dissociation ?

The weak base dissociation is a base that do not completely dissociates in water at equilibrium.

BOH → B⁺(aq) + OH⁻(aq)

B(aq) + H₂O (l) ⇄ BH⁺ (aq) + OH⁻(aq)

weak base

What is Equilibrium ?

The equilibrium is a state of balanced in a reaction in which the concentration of the reactant and the concentration of the product remain unchanged with time.

Thus, from the above conclusion we can say that The equilibrium constant would shift to a new constant this would happen to a weak base dissociation equilibrium if more products were added.

Hence, Option (A) is correct answer.

Learn more about the Equilibrium here: https://brainly.com/question/517289
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