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© Copyright Pearson Prentice Hall
Slide 2 of 27
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.
18.3
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Solubility Equilibrium >
Slide 3 of 27
The Solubility Product Constant
The Solubility Product Constant
What is the relationship between the solubility product constant and the solubility of a compound?
18.3
Slide 4 of 27
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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.
Slide 5 of 27
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>Solubility Equilibrium The Solubility Product Constant18.3
Slide 6 of 27
© Copyright Pearson Prentice Hall
>Solubility Equilibrium The Solubility Product Constant18.3
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© Copyright Pearson Prentice Hall
>Solubility Equilibrium The Solubility Product Constant
Silver chloride is slightly soluble in water.
18.3
Slide 8 of 27
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>Solubility Equilibrium The Solubility Product Constant
Scale, formed by the precipitation of slightly soluble salts, builds up around faucets.
18.3
© Copyright Pearson Prentice Hall
Slide 13 of 27
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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Solubility Equilibrium >
Slide 14 of 27
The Common Ion Effect
The Common Ion Effect
How can you predict whether precipitation will occur when two salt solutions are mixed?
18.3
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Solubility Equilibrium >
Slide 15 of 27
The Common Ion Effect
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.
18.3
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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.
18.3
Slide 17 of 27
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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.
18.3
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Slide 22 of 27
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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Slide 23 of 27
Section Quiz
-or-Continue to: Launch:
Assess students’ understanding of the concepts in Section
18.3 Section Quiz.
18.3.
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Slide 24 of 27
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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Slide 25 of 27
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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Slide 26 of 27
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.
© Copyright Pearson Prentice Hall
Slide 27 of 27
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.