   Chapter 15, Problem 96AP ### 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
1 views

# 96. Strictly speaking, the solvent is the component of a solution that is present in the largest amount on a mole basis. For solutions involving water, water is almost always the solvent because there tend o be many more water molecules present than molecules of any conceivable solute. To see why this is so, calculate the number of moles of water present in 1.0 L of water. Recall that the density of water is very nearly 1.0 g/mL under most conditions.

Interpretation Introduction

Interpretation:

The number of moles of water present in 1.0L of water 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 number of moles is calculated by the formula,

Moles=MassgMolarmass.

Explanation

The volume and density of water is given to be 1.0L and 1.0g/mL respectively.

The mass of water is calculated by the formula,

Mass=Volume×Density        (1)

Substitute the values of volume and density in the equation (1).

Mass=1L×1.0g/mL×1000mL1L=1000g

The molar mass of water is 18.015g/mol

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