**Problem Statement:**An aqueous solution is prepared by adding 16 g of NaCl and diluting to a volume of 100 ml. The density of this solution is 1.09 g/ml. Find the molarity, molality, and mole fraction of the NaCl in this solution.**Explanation:**To solve this problem, we are required to calculate three different concentration measures for the NaCl solution: molarity, molality, and mole fraction.1. **Molarity (M)** - the number of moles of solute per liter of solution. - To find molarity, first calculate the moles of NaCl (using its molar mass), then divide by the volume of the solution in liters.2. **Molality (m)** - the number of moles of solute per kilogram of solvent. - Determine the mass of the solvent by subtracting the mass of NaCl from the total mass of the solution, given the solution's density.3. **Mole Fraction (X)** - the ratio of the number of moles of a component to the total number of moles of all components in the solution. - Calculate the moles of water (solvent) using its molar mass, and use this in conjunction with the moles of NaCl to find the mole fraction.This problem requires an understanding of the methods for interconverting between mass, volume, and moles, as well as the ability to use the physical property of density to link these quantities.

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An aqueous solution is prepared by adding 16 g of NaCl and diluting to a volume of 100 ml. The density of this solution is 1.09 g/ml. Find the molarity, molality, and mole fraction of the NaCl in this solution.

An aqueous solution is prepared by adding 16 g of NaCl and diluting to a volume of 100 ml. The density of this solution is 1.09 g/ml. Find the molarity, molality, and mole fraction of the NaCl in this solution.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

**Problem Statement:**

An aqueous solution is prepared by adding 16 g of NaCl and diluting to a volume of 100 ml. The density of this solution is 1.09 g/ml. Find the molarity, molality, and mole fraction of the NaCl in this solution.

**Explanation:**

To solve this problem, we are required to calculate three different concentration measures for the NaCl solution: molarity, molality, and mole fraction.

1. **Molarity (M)** - the number of moles of solute per liter of solution.
- To find molarity, first calculate the moles of NaCl (using its molar mass), then divide by the volume of the solution in liters.

2. **Molality (m)** - the number of moles of solute per kilogram of solvent.
- Determine the mass of the solvent by subtracting the mass of NaCl from the total mass of the solution, given the solution's density.

3. **Mole Fraction (X)** - the ratio of the number of moles of a component to the total number of moles of all components in the solution.
- Calculate the moles of water (solvent) using its molar mass, and use this in conjunction with the moles of NaCl to find the mole fraction.

This problem requires an understanding of the methods for interconverting between mass, volume, and moles, as well as the ability to use the physical property of density to link these quantities.

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