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Chapter 14: Problem 25

Relate Le Chatelier's principle to the common-ion effect.

Short Answer

Expert verified
Le Chatelier's principle and the common-ion effect are related in that when a common ion is introduced into a system in equilibrium (common-ion effect), the system reacts by shifting the position of the equilibrium (Le Chatelier's principle) to counteract the change and minimize the influence of the added ion. This can be observed in solubility equilibria and acid/base reactions.

Step by step solution

01

Understanding Le Chatelier's Principle

Le Chatelier's principle states that if a change is imposed on a system at equilibrium, the system will respond by adjusting in such a way as to counter the change. This means that if a reaction at equilibrium is disturbed by changing the conditions, the position of equilibrium moves to oppose the change.
02

Defining the Common-ion Effect

The common-ion effect refers to the decreasing ionization of an ionic compound by adding more of an ion that is a part of the compound. It can be observed when a weak acid or weak base is in a solution with a strong acid or base that shares one of its ions.
03

Relating the Two Concepts

Le Chatelier's principle can be related to the common-ion effect when an external source introduces a common ion into the system. This induces a change in the system, and according to Le Chatelier's principle, the system will adjust itself to counter that change. In practical terms: When a common ion is added to a solution with a weak acid or base, it provides an excess of a particular ion, causing the equilibrium to shift to compensate.
04

Practical Example

Consider the equilibrium involving acetic acid (CH3COOH), a weak acid, and water: CH3COOH ⇌ CH3COO- + H+. If a common ion such as CH3COO- is added (from sodium acetate, for instance), according to Le Chatelier's principle, the excess CH3COO- will cause the equilibrium to shift to the left, reducing the ionization of acetic acid and therefore decreasing the concentration of H+ ions (making the solution less acidic).

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Most popular questions from this chapter

Distinguish between solubility and solubility product constant. Explain how one may be calculated from the other.

Imagine the following hypothetical reaction, taking place in a sealed, rigid container, to be neither exothermic nor endothermic. $$\mathrm{A}(g)+\mathrm{B}(g) \rightleftarrows \mathrm{C}(g) \quad \Delta H=0$$ Would an increase in temperature favor the forward reaction or the reverse reaction? (Hint: Recall the gas laws.)

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