   Chapter 15, Problem 102AP ### 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
3 views

# You mix 225.0 mL of a 2.5 M HCl solution with 150.0 mL of a 0.75 M HCl solution. What is the molarity of the final solution?

Interpretation Introduction

Interpretation:

The molarity of the final 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 two solutions with the different molarities and the volume are given.

The molarity and volume of the first HCl solution is 2.5M and 225.0mL respectively.

The conversion of units of 225.0mL into L is done as,

225.0mL=225.01000L=0.225L

The number of moles in the first solution is calculated by the formula,

Moles=Molarity×Volume        (1)

Substitute the values of molarity and volume in the equation (1).

Moles=2.5M×0.225L=0.5625moles

The molarity and volume of the second HCl solution is 0.75M and 150.0mL respectively.

The conversion of units of 150.0mL into L is done as,

150.0mL=150.01000L=0.15L

Substitute the values of molarity and volume in the equation (1).

Moles=0.75M×0.15L=0.1125moles

The total number of moles of first and second solution is calculated as shown below.

Totalnumberofmoles=Molesoffirstsolution+Molesofsecondsolution=0

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