   Chapter 15, Problem 40QAP ### 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

# 40. An alcoholic iodine solution (“tincture” of iodine) is prepared by dissolving 5.15 g of iodine crystals in enough alcohol to make a volume of 225 mL. Calculate the molarity of iodine in the solution.

Interpretation Introduction

Interpretation:

The molarity of iodine in the 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 elementis determined from atomic mass of an element.

The formula to calculate the number of moles is,

Moles=MassgMolarmass

Molarity is used to find out the concentration of solution.

The formula to calculate molarity is,

Molarity=NumberofmolesofsoluteLitersofsolution.

Explanation

It is given that 5.15g of iodine crystals are added to total volume of 225mL.

The molar mass of iodine I2 is,

Molarmass=nAtomicmassofI=2126.9g/mol=253.8g/mol

The formula to calculate the number of moles is,

Moles=MassofI2gMolarmassofI2

Substitute the values of mass and molar mass of iodine in the above expression.

Moles=5.15g253.8g/mol=0

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