   Chapter 15, Problem 142CP ### 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
23 views

# A 50.00-mL sample of aqueous Ca(OH)2 requires 34.66 mL of a 0.944 M nitric acid for neutralization. Calculate the concentration (molarity) of the original solution of calcium hydroxide.

Interpretation Introduction

Interpretation:

The concentration of CaOH2 required to neutralize 34.66mL of 0.944M nitric acid is to be calculated.

Concept Introduction:

Neutralization is the process in which an acid and a base react with each other to give salt and water. The general reaction of acid and base is represented as:

AH+BOHAB+H2O

The molarity of a solution is defined as the number of moles of solute dissolved in one liter of the solution. The formula for molarity is given as:

M=nV

Where,

• n represents the number of moles of the solute.
• V represents the volume of the solution.
Explanation

The molarity of the given HNO3 solution is 0.944M.

The volume of the given CaOH2 solution is 50.00mL.

The volume of the HNO3 is 34.66mL.

The neutralization reaction between HNO3 and CaOH2 is represented as:

2HNO3aq+CaOH2aqCaNO32aq+2H2Ol

The relation between molarities of HNO3 and CaOH2 is given as:

M1V1=2M2V2

Where,

• M1 represents the molarity of HNO3

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