   Chapter 17, Problem 67QAP ### 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
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# . Magnesium fluoride dissolves in water to the extent of 8.0 × 10 − 2 g/L at 25°C. Calculate the solubility of MgF2(s) in moles per liter, and calculate Kspfor MgF2at 25 °C.

Interpretation Introduction

Interpretation:

The solubility in moles per liter and Ksp value for magnesium fluoride, MgF2(s) at 25°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

Magnesium fluoride, MgF2(s) is only soluble in water to the extent of 8.0×102g/L at 25°C.

To calculate the solubility of magnesium fluoride, MgF2(s) in mol/L, the formula used is,

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

Molar mass of CaSO4 is 62.31g/mol.

Substitute the value of molar mass and solubility (g/L) of magnesium fluoride, MgF2(s) in the given formula.

Solubility(mol/L)=8.0×102gL×162.31molg=1.3×103mol/L

The solubility of magnesium fluoride, MgF2(s) is 1.3×103mol/L.

The chemical reaction for the solubility of CaSO4 is,

MgF2(s)Mg2+(aq)+2F(aq)1

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