   Chapter 15, Problem 133AP ### 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
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# How many milliliters of 0.105 M NaOH are required to neutralize exactly 14.2 mL of 0. 141 M H3PO4?

Interpretation Introduction

Interpretation:

The milliliters of 0.105M

NaOH required to neutralize the given H3PO4 solution is to be calculated.

Concept Introduction:

Solution is composed of solute and solvent particles. Solute particles are always present in lower amount as compared to amount of the solvent in the solution. 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 molarity is calculated by the formula,

Molarity=NumberofmolesofsoluteVolumeofsolutionL.

Explanation

The values of M1, V1 and M2 is given to be 0.141M, 14.2mL and 0.105M respectively.

The equation for the given chemical reaction is shown below.

H3PO4aq+3NaOHaqNa3PO4aq+3H2O

The above equation exhibits that three moles of NaOH are required to neutralize H3PO4 solution.

Hence, the relationship between molarity and volume of both the given solutions is shown below.

3×M1V1=M2V2

Where,

• M1 is the molarity of H3PO4 solution.
• V1 is the volume of H3PO4 solution

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