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Chapter 17: Problem 3

What is the common ion effect?

Short Answer

Expert verified
The common ion effect is the shift in equilibrium caused by the addition of an ion already present in the solution, leading to changes in the solubility of salts.

Step by step solution

01

Define the Common Ion Effect

The common ion effect refers to the phenomenon where the addition of an ion that is already present in a solution can affect the equilibrium of the solution. To understand this effect, one should be familiar with the basic principles of chemical equilibrium and Le Chatelier's principle.
02

Explain with Le Chatelier's Principle

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change. In the context of the common ion effect, adding more of a common ion shifts the equilibrium away from forming more of that ion, often resulting in less soluble salts precipitating or reducing the solubility of an ionic compound.
03

Illustrate with an Example

Consider a saturated solution of calcium fluoride (CaF2), which is in equilibrium with its ions: CaF2(s) ⇋ Ca2+(aq) + 2F−(aq)Adding a soluble fluoride salt, such as sodium fluoride (NaF), which dissociates to provide an additional source of F− ions, will shift the equilibrium to the left, reducing the solubility of calcium fluoride due to the increased concentration of fluoride ions.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Chemical Equilibrium
Imagine a busy market where people come and go, buying and selling goods all day. Chemical equilibrium is not too different; it represents a state where the rate of the forward reaction, where reactants turn into products, matches the rate of the backward reaction, where products revert to reactants. This does not mean the reactants and products stop changing, rather they do so at a constant, unchanging rate, similar to a busy market that stays busy throughout the day.

This balanced state can be illustrated by a simple chemical equation where the reactants and products are represented by letters, such as A and B forming C:

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Most popular questions from this chapter

Methyl red has a pKa of 5.0 and is red in its acid form and yellow in its basic form. If several drops of this indicator are placed in a 25.0-mL sample of 0.100 M HCl, what color does the solution appear? If 0.100 M NaOH is slowly added to the HCl sample, in what pH range will the indicator change color?

Phenolphthalein has a pKa of 9.7. It is colorless in its acid form and pink in its basic form. For each of the pH values, calculate [In-]/[HIn] and predict the color of a phenolphthalein solution. a. pH = 2.0 b. pH = 5.0 c. pH = 8.0 d. pH = 11.0

A 0.867-g sample of an unknown acid requires 32.2 mL of a 0.182 M barium hydroxide solution for neutralization. Assuming the acid is diprotic, calculate the molar mass of the acid.

Two 25.0-mL samples, one 0.100 M HCl and the other 0.100 M HF, are titrated with 0.200 M KOH. a. What is the volume of added base at the equivalence point for each titration? b. Is the pH at the equivalence point for each titration acidic, basic, or neutral? c. Which titration curve has the lower initial pH? d. Sketch each titration curve.

The Kb of hydroxylamine, NH2OH, is 1.10 * 10-8. A buffer solution is prepared by mixing 100.0 mL of a 0.36 M hydroxylamine solution with 50.0 mL of a 0.26 M HCl solution. Determine the pH of the resulting solution.
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