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Chapter 13: Problem 2

Basing your answer on intermolecular force considerations, explain what "like dissolves like" means.

Short Answer

Expert verified
'Like dissolves like' means that solutes will dissolve best in solvents that have the same type of intermolecular forces. Polar solutes will dissolve in polar solvents, and nonpolar solutes will dissolve in nonpolar solvents, due to the type of bonds they can form with each other.

Step by step solution

01

Identify the concept of 'like dissolves like'

'Like dissolves like' is a term used in chemistry to explain that polar solvents dissolve polar solutes, and nonpolar solvents dissolve nonpolar solutes.
02

Define Polar and Nonpolar Substances

Polar substances have positive and negative ends or poles, while nonpolar substances do not. Polar substances include water and alcohol, while fats and oils are nonpolar substances.
03

Explain Intermolecular Forces

The forces of attraction between molecules of the same substance are called intermolecular forces. These forces can be either polar or nonpolar.
04

Apply the Concept to Intermolecular Forces

In a polar solvent like water, the positive end of one water molecule is attracted to the negative end of another, creating a strong bond. Nonpolar solutes, on the other hand, lack these poles and are not able to form these strong connections with the water molecules. As a result, they don't dissolve well in water, which is a polar solvent.
05

Conclude with a final explanation of the concept

'Like dissolves like' means that solutes will dissolve best in solvents that have the same type of intermolecular force. Polar substances will dissolve in polar solvents, and nonpolar substances will dissolve in nonpolar solvents due to their similar nature.

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Most popular questions from this chapter

What is the osmotic pressure (in atmospheres) of a \(12.36 M\) aqueous urea solution at \(22.0^{\circ} \mathrm{C} ?\)

The osmotic pressure of \(0.010 M\) solutions of \(\mathrm{CaCl}_{2}\) and urea at \(25^{\circ} \mathrm{C}\) are \(0.605 \mathrm{~atm}\) and \(0.245 \mathrm{~atm},\) respectively. Calculate the van't Hoff factor for the \(\mathrm{CaCl}_{2}\) solution.

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