Chapter 14, Problem 65A

How do 0.5M and 2.0M aqueous solutions of NaCl differ?

Interpretation Introduction

Interpretation:

0.5M and 2.0M aqueous solutions of NaClhave to be differentiated.

Concept introduction:

Composition of a solution can be defined by expressing its concentration. The concentrations of solutions can be expressed in different ways, which are involved in the quantity of solute and the quantity of solution or solvent. Several ways are there by which we can describe the concentration of the solution quantitatively. Some commonly used quantitative concentration terms are percent by mass, percent by volume, molarity, molality and mole fraction.

Molarity: Molarity is defined as the number of moles of solute present in one litre of the solution and is expressed as:

$\mathrm{Molarity}ofthesolution=\frac{Numberofmolesof the solute}{ Volume of the solution(inlitre)}$

Answer to Problem 65A

The basic difference between 0.5 M and 2.0 M aqueous solution of NaCl is the number of moles of NaCl present in the fixed volume of solution. 2.0 M solution contains more number of moles of solute NaCl per volume of water than the 0.5M solution.

Molarity is ratio between the number of moles of solute present and volume of the solution. For the fixed volume of solvent, the solution having higher molarity contains more no of moles of solute than other. 2.0 M solution contains more number of moles of solute NaCl per volume of water than the 0.5M solution.

Explanation of Solution

Molarity is ratio between the number of moles of solute present and volume of the solution. For the fixed volume of solvent, the solution having higher molarity contains more no of moles of solute than other. 2.0 M solution contains more number of moles of solute NaCl per volume of water than the 0.5M solution.