   Chapter 15, Problem 51QAP ### 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

# 51. An experiment calls for 125 mL of 0.105 M NaCl solution. What mass of NaCl is required? What mass of NaCl would be required for 1.00 L of the same solution?

Interpretation Introduction

Interpretation:

The mass required to prepare 1.00L of 0.105M

NaCl solution is to be calculated.

Concept Introduction:

There are many ways to determine the concentration of the solution. One of the most used methods is molarity. Molarity is be defined as the number of moles of the solute in one liter of the whole solution. Thus, the molarity can be calculated as:

M=MolesofsolutemoleTotalvolumeofsolutionL.

Explanation

The molarity and volume of NaCl solution is given to be 125mL and 0.105M respectively.

The conversion of milliliter to liter is as follows:

1mL=0.001L125mL=0.125L

The number of moles of solute is calculated by the formula,

Numberofmoles=Molarity×Volume

Substitute the values of molarity and volume in the above expression.

Numberofmoles=0.105M×0.125L=0.0131moles

Thus to make 125mL of 0.105M

NaCl solution, the number of moles required are 0.0131moles

The mass of NaCl in the solution is calculated by the formula,

Mass of salt=Numberofmoles×Molar mass of salt

Molar mass of NaCl is 58.44g/mol

Substitute the value of molar mass and number of moles of NaCl in the above formula.

Mass of NaCl=0.0131moles×58

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