Chapter 2, Problem 95PS

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# Epsom salt is used in tanning leather and in medicine. It is hydrated magnesium sulfate, MgSO4 · 7 H2O. The water of hydration is lost on heating, with the number lost depending on the temperature. Suppose you heat a 1.394-g sample at 100 °C and obtain 0.885 g of a partially hydrated sample, MgSO4 · x H2O. What is the value of x?

Interpretation Introduction

Interpretation:

The value of x for the partially hydrated sample MgSO4.xH2O is to be calculated from the given data’s of Epson salt.

Concept introduction:

• Conversion formula for mass of a molecule and number moles,

Numberofmoles=MassingramsMolarmass

• Molar mass of a molecule can be calculated from its molecular formula by taking the sum of atomic masses of all the elements present in it.
Explanation

Given,

The mass of hydrated sample MgSO4.7H2O is 1.394g .

The mass of partially hydrated sample MgSO4.xH2O is 0.885g

Therefore,

The mass of water driven off in the sample after heating is 1.394gâˆ’0.885g=â€‰0.509g

Equation for finding number moles from mass of a molecule and molar mass is,

â€‚Â Â Â Â Â Numberâ€‰ofâ€‰molesâ€‰â€‰=â€‰â€‰Massâ€‰inâ€‰gramsâ€‰Molarâ€‰mass

Therefore,

The number of moles of water molecule lost is,

Â Â Â Â Numberâ€‰ofâ€‰molesâ€‰â€‰=â€‰â€‰0.509gâ€‰18gâ€‰â€‰=â€‰â€‰0

### Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

#### The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started