Solutions

This section covers the fundamentals of solutions, including types, concentrations, solubility factors, and colligative properties.

Introduction

This section introduces solutions as homogeneous mixtures and outlines the importance of understanding their properties and behavior.

Types Of Solutions

This section discusses the various types of solutions based on physical states and solute amounts, along with important concepts associated with solution concentrations.

Physical State Of Solute And Solvent

This section explores the classification of solutions based on the physical state of the solute and solvent, outlining examples for each type.

Based On Amount Of Solute

This section discusses different types of solutions based on the amount of solute present: unsaturated, saturated, and supersaturated solutions.

Concentration Of Solutions

This section discusses the various methods of expressing the concentration of solutions, such as mass percentage and molarity, along with colligative properties related to the number of solute particles.

Mass Percentage (W/w)

Mass percentage (w/w) is a way to express the concentration of a solution, showing the mass of the solute relative to the total mass of the solution.

Volume Percentage (V/v)

Volume percentage (v/v) is a measure of concentration that expresses the volume of a solute divided by the total volume of the solution, typically multiplied by 100.

Mass By Volume Percentage

The mass by volume percentage expresses the concentration of a solute in a solution, calculated by the mass of the solute divided by the volume of the solution in milliliters.

Molarity (M)

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution.

Molality (M)

Molality is a measurement of concentration that denotes the number of moles of solute per kilogram of solvent, providing an essential way to express solution concentration particularly in colligative property calculations.

Mole Fraction (X)

Mole fraction is a key term for expressing the concentration of components in a solution, representing the ratio of moles of a component to the total moles of all components.

Normality (N)

Normality is defined as the number of gram equivalents of solute per liter of solution, a critical concept in understanding solution concentrations.

Solubility

Solubility defines the maximum amount of a solute that can dissolve in a solvent at a specific temperature, influenced by factors such as the nature of the solute and solvent, temperature, and pressure.

Factors Affecting Solubility

The solubility of substances is influenced by the nature of the solute and solvent, temperature, and pressure.

Henry’s Law

Henry's Law states that the solubility of a gas in a liquid is directly proportional to the pressure of that gas above the liquid.

Vapour Pressure Of Liquid Solutions

This section discusses the vapour pressure of liquid solutions, focusing on Raoult's Law and the colligative properties associated with it.

Raoult’s Law (For Ideal Solutions)

Raoult's Law states that the partial vapor pressure of a component in an ideal solution is proportional to its mole fraction.

Ideal Solution

This section discusses ideal solutions, their characteristics, and relationships with Raoult’s Law.

Non-Ideal Solution

Non-ideal solutions deviate from Raoult’s Law, displaying different properties than ideal solutions.

Colligative Properties

Colligative properties are properties that depend solely on the number of solute particles in a solution, regardless of their chemical nature.

Relative Lowering Of Vapour Pressure

The relative lowering of vapour pressure is a colligative property, illustrating how the presence of a solute reduces the vapour pressure of a solvent.

Elevation In Boiling Point

Elevation in boiling point is a colligative property that reflects how solute particles impact the boiling point of a solvent.

Depression In Freezing Point

Depression in freezing point is a colligative property that describes how the boiling point of a solution is reduced compared to the pure solvent due to the presence of solute particles.

Osmotic Pressure (Π)

Osmotic pressure (π) is a colligative property that measures the tendency of a solvent to move from a dilute to a concentrated solution through a semipermeable membrane.

Abnormal Molar Mass And Van’t Hoff Factor (I)

The section discusses how the van’t Hoff factor (i) explains deviations in colligative properties due to solute dissociation or association.

Summary

This section summarizes the key concepts of solutions including types, concentration classes, solubility, and colligative properties.