   Chapter 15, Problem 137CP ### 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
1 views

# Calculate the concentration of all ions present when 0.160 g of MgCl2 is dissolved in enough water to make 100.0 mL of solution.

Interpretation Introduction

Interpretation:

The concentration of all ions present when MgCl2 is dissolved to make a 100.0mL solution is to be calculated.

Concept Introduction:

The atomic mass of an element is defined as the sum of number of protons and number of neutrons. Molar mass of an element is determined from atomic mass of an element.

The number of moles is calculated by the formula,

Moles=MassgMolarmass

The molarity is calculated by the formula,

Molarity=NumberofmolesofsoluteVolumeofsolutionL.

Explanation

The mass of MgCl2 and volume of solution is given to be 0.160g and 100.0mL respectively.

The conversion of units of 100.0mL into L is done as,

100.0mL=100.1000L=0.1L

The molar mass of MgCl2 is 95.21g/mol.

The number of moles is calculated by the formula,

Moles=MassgMolarmass    (1)

Substitute the values of mass and molar mass in the equation (1).

Moles=0.160g95.21g/mol=0.0017mol

The molarity of MgCl2 is calculated by the formula,

Molarity=NumberofmolesofsoluteVolumeofsolutionL     (2)

Substitute the values of number of moles of solute and volume of solution in equation (2).

The MgCl2 compound has one Mg2+ and two Cl ions

### 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 