   Chapter 17, Problem 65QAP ### Introductory Chemistry: A Foundati...

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

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
19 views

# . Approximately 1.5 × 10 − 3 of iron(II) hydroxide. Fe(OH)2(s), dissolves per liter of water at 18 °C. Calculate Kspfor Fe(OH)2(s) at this temperature.

Interpretation Introduction

Interpretation:

The Ksp value for iron (II) hydroxide, Fe(OH)2(s) at 18°C 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

Iron (II) hydroxide, Fe(OH)2(s) is soluble in water to the extent of approximately 1.5×103g/L at 18°C.

To calculate the solubility of iron (II) hydroxide, Fe(OH)2(s) in mol/L, the formula used is,

Solubility(mol/L)=SolubilitygL×1molar massmolg

Molar mass of CaSO4 is 89.87g/mol.

Substitute the value of molar mass and solubility (g/L) of calcium sulfate, CaSO4 in the given formula.

Solubility(mol/L)=1.5×103gL×189.87molg=1.7×105mol/L

The solubility of iron (II) hydroxide, Fe(OH)2(s) is 1.51×102mol/L.

The chemical reaction for the solubility of Fe(OH)2(s) is,

Fe(OH)2(s)Fe2+(aq)+2OH(aq)1

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