   # For an acid or a base, when is the normality of a solution equal to the molarity of the solution and when are the two concentration units different? ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 10, Problem 23Q
Textbook Problem
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## For an acid or a base, when is the normality of a solution equal to the molarity of the solution and when are the two concentration units different?

Interpretation Introduction

Interpretation: The difference in two concentrations units are to be explained along with the equality in normality and molarity.

Concept Introduction:

The equivalent concentration of solution otherwise called as Normality is the measure of concentration in terms of the gram equivalent weight per litre of solution. The role of solute in the reaction is used for the calculation of normality of a solution. Normality can be given by the formula,

Normality=NumberofgramequivalentofsoluteVolumeofsolutioninlitre

The concentration of solution can be defined in terms of Molarity, as moles of solute (in grams) to the volume of solution (in litre). Molarity can be given by the formula,

Molarity(M)=Molesofsolute(ing)Volumeofsolution(inL)

### Explanation of Solution

To explain Normality

The number of equivalents per liter of a solution is called Normality.

For an acid, an equivalent is the mass of an acid than can give 1 mole of H+ ions.

For a base, an equivalent is the mass of base that can accept 1 mole of H+ ions.

H+ ions are basically called as protons.

To explain Molarity

The mole of solute per litre of a solution is called as molarity.

To explain when the molarity and normality will be equal.

The normality and molarity of a solution will be equal when the gram equivalent’s number will be equal to the number of moles of solute. The number of equivalent will be equal to be the number of moles of solute in an acid which has only one acidic proton present in the, and in those bases, which accepts only one proton per formula unit.

Examples for those bases and acid where equivalents and moles are equal

Those acids which has equal number of equivalents to the moles of solute are HCl,HNO3,HFandHC2

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