Chemistry 18.3

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Chemistry 18.3

© Copyright Pearson Prentice Hall

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Solubility Equilibrium

Barium sulfate is ingested by a patient before X-ray images of the digestive tract are taken. Barium sulfate absorbs the X-rays, thereby producing light areas on the developed X-ray film. However, barium salts are usually toxic. You will learn why patients can ingest this poisonous substance without harm.

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Solubility Equilibrium >

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The Solubility Product Constant

The Solubility Product Constant

What is the relationship between the solubility product constant and the solubility of a compound?

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>Solubility Equilibrium18.3 The Solubility Product Constant

The solubility product constant (Ksp), equals the product of the concentrations of the ions, each raised to a power equal to the coefficient of the ion in the dissociation equation.

The smaller the numerical value of the solubility product constant, the lower the solubility of the compound.

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>Solubility Equilibrium The Solubility Product Constant18.3

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>Solubility Equilibrium The Solubility Product Constant18.3

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>Solubility Equilibrium The Solubility Product Constant

Silver chloride is slightly soluble in water.

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>Solubility Equilibrium The Solubility Product Constant

Scale, formed by the precipitation of slightly soluble salts, builds up around faucets.

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SAMPLE PROBLEM

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SAMPLE PROBLEM

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SAMPLE PROBLEM

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SAMPLE PROBLEM

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Practice Problems for Sample Problem 18.3

Problem Solving 18.17 Solve Problem 17 with the help of an interactive guided tutorial.



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The Common Ion Effect


How can you predict whether precipitation will occur when two salt solutions are mixed?

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If the product of the concentrations of two ions in the mixture is greater than the Ksp of the compound formed from the ions, a precipitate will form.

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>Solubility Equilibrium The Common Ion Effect

A common ion is an ion that is found in both salts in a solution. The lowering of the solubility of an ionic compound as a result of the addition of a common ion is called the common ion effect.

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>Solubility Equilibrium The Common Ion Effect

A saturated solution of lead(II) chromate is pale yellow.

When a few drops of lead nitrate are added to the solution, more lead(II) chromate precipitates.

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SAMPLE PROBLEM

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SAMPLE PROBLEM

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SAMPLE PROBLEM

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SAMPLE PROBLEM

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Practice Problems for Sample Problem 18.4

Problem Solving 18.19 Solve Problem 19 with the help of an interactive guided tutorial.


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Section Quiz

-or-Continue to: Launch:

Assess students’ understanding of the concepts in Section

18.3 Section Quiz.

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18.3 Section Quiz.

1. What is the concentration of a saturated solution of silver sulfide?

The Ksp of Ag2S is 8.0 10-51.

a. 2.0 10-17M

b. 8.9 10-26M

c. 8.9 10-25M

d. 2.0 1017M


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2. Adding which of these solutions to a saturated solution of BaSO4 will cause the solubility of BaSO4 to decrease?

I. BaCl2(aq)

II. Na2SO4 (aq) a. (I) only

b. (II) only

c. (I) and (II)

d. neither solution

18.3 Section Quiz.


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18.3 Section Quiz.

3. The Ksp of AgBr is 5.0 10-13. When 7.1 10-6 mol/L solutions of NaBr(aq) and AgNO3(aq) are mixed, we would expect

a. no precipitate to form.

b. a definite precipitation reaction.

c. no reaction.

d. a saturated solution but no visible precipitation.


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18.3 Section Quiz.

4. After the common ion effect causes a precipitate to form in a solution,

a. the solution will no longer be saturated.

b. the solution will again be saturated.

c. the solution will be supersaturated.

d. there will be no solute left in the solution.

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Chemistry 18.3