   Chapter 15, Problem 132AP ### 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
14 views

# A sodium dihydrogen phosphate solution was prepared by dissolving 5.0 g of NaH2PO4 in enough water to make 500. mL of solution. What are the molarity and normality of the resulting solution?

Interpretation Introduction

Interpretation:

The molarity and normality of the resulting 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

The normality of the solution is calculated by the formula,

Normality=Molarity×NumberofH+orOHions.

Explanation

The mass of NaH2PO4 and volume of NaH2PO4 solution is given to be 5.0g and 500.mL.

The conversion of units of 500.mL into L is done as,

500.mL=500.1000L=0.5L

The molar mass of NaH2PO4 is 119.98g/mol.

The number of moles of NaH2PO4 in a solution is calculated by the formula,

Moles=MassgMolarmass    (1)

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

Moles=5.0g119.98g/mol=0.0417moles

The molarity is calculated by the formula,

Molarity=NumberofmolesofsoluteVolumeofsolutionL     (2)

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

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