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Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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. The solubility product of iron(III) hydroxide is very small: K sp = 4 × 10 38 at 25 °C. A classical method of analysis for unknown samples containing iron is to add NaOH or NH3. This precipitates Fe(OH)3, which can then be filtered and weighed. To demonstrate that the concentration of iron remaining in solution in such a sample is very small, calculate the solubility of Fe(OH)3in moles per liter and in grams per liter.

Interpretation Introduction

Interpretation:

The solubility of Fe(OH)3 in moles per liter and in grams per liter is to be calculated.

Concept Introduction:

The solubility product is represented by Ksp. The solubility product describes the solubility of the solid substance in the solvent at the particular temperature. The term “solubility product” is only used for those substances that are not completely soluble in water.

Explanation

The Ksp value of Fe(OH)3 is 4×1038. The chemical reaction for the solubility of Fe(OH)3 is,

Fe(OH)3(s)Fe3+(aq)+3OH(aq)x3x

Where x shows the solubility of each ion in mol/L.

The expression for the solubility product ( Ksp ) of iron (III) hydroxide is given as,

Ksp=[Fe3+][OH]3=x×(3x)3=27x4

Substitute the Ksp value for Fe(OH)3 in the given equation

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