Chapter 7, Problem 7.20E

Interpretation Introduction

(a)

Interpretation:

The molarity of $1.25\text{L}$ of solution containing $0.455\text{mol}$ of solute is to be calculated.

Concept introduction:

A solution is prepared by mixing proper amount of solute and solvent. The concentration of solution when measured on the basis of solution volume, is expressed in terms of percent weight by volume $\left(\text{\%}\text{w}/\text{v}\right)$, percent volume by volume $\left(\text{\%}\text{v}/\text{v}\right)$ and molarity $\left(\text{M}\right)$. When concentration is measured on the basis of mass of solvent, it is expressed in terms of percent weight by weight $\left(\text{\%}\text{w}/\text{w}\right)$.

Interpretation Introduction

(b)

Interpretation:

The molarity of $250\text{mL}$ of solution containing $0.215\text{mol}$ of solute is to be calculated.

Concept introduction:

A solution is prepared by mixing proper amount of solute and solvent. The concentration of solution when measured on the basis of solution volume, is expressed in terms of percent weight by volume $\left(\text{\%}\text{w}/\text{v}\right)$, percent volume by volume $\left(\text{\%}\text{v}/\text{v}\right)$ and molarity $\left(\text{M}\right)$. When concentration is measured on the basis of mass of solvent, it is expressed in terms of percent weight by weight $\left(\text{\%}\text{w}/\text{w}\right)$.

Interpretation Introduction

(c)

Interpretation:

The molarity of $0.175\text{mol}$ of solute present in $100\text{mL}$ of solution is to be calculated.

Concept introduction:

A solution is prepared by mixing proper amount of solute and solvent. The concentration of solution when measured on the basis of solution volume, is expressed in terms of percent weight by volume $\left(\text{\%}\text{w}/\text{v}\right)$, percent volume by volume $\left(\text{\%}\text{v}/\text{v}\right)$ and molarity $\left(\text{M}\right)$. When concentration is measured on the basis of mass of solvent, it is expressed in terms of percent weight by weight $\left(\text{\%}\text{w}/\text{w}\right)$.