Solutions

Colligative Properties

Created byVinay Arya

Last updated 4/2019

English

What you'll learn

Types of Solutions

Course content

1 section • 18 lectures • 3h 22m total length

Introduction5:06
Explore the types of solutions, concentration concepts, and colligative properties in this introduction to solutions. Learn about boiling point and freezing point depression, ideal vs non-ideal solutions, and Henry's law.
Types of Solutions10:07
Explore the concept of solutions, distinguishing homogeneous and heterogeneous mixtures, and examine solubility, saturated and unsaturated solutions, plus how temperature and states of matter affect dissolution (solid–liquid, liquid–liquid, gas–liquid).
Concentration Representation: Molality and formality13:44
Learn to express solution concentrations using mass percent, weight/volume, volume/volume, ppm, mole fraction, and formality with practical formulas and examples.
Concentration Representation : Normality and Molarity10:39
Explore two representations of solution concentration—normality and molarity—and learn their conversions and practical use in laboratory calculations.
Colligative Properties10:10
Explore colligative properties, including boiling point elevation, freezing point depression, and vapor pressure lowering, which depend on solute concentration and non-electrolyte status, enabling molecular mass determination.
Relative lowering of Vapour Pressure15:15
Derive the relative lowering of vapor pressure using Raoult's law for nonvolatile solutes, relate solvent vapor pressure to mole fractions, and discuss applicable limitations.
Elevation in Boiling Point13:50
Explain how solutes elevate boiling point, demonstrate measurement via a solvent–solution graph, and show how to determine an unknown nonvolatile solute's molecular mass from boiling point elevation.
Depression in freezing point17:23
Explore how solutes depress the freezing point of water, derive the relationship between freezing point depression and solution concentration, and review practical applications like road de-icing and automotive antifreeze.
Osmotic Pressure14:22
Explore osmosis and osmotic pressure across semi-permeable membranes, define osmotic pressure as the excess pressure needed to stop solvent flow, and relate it to solute particle number and molar mass.
Ideal Solutions9:35
Learn how ideal solutions follow Raoult's law, exhibit zero enthalpy and zero volume of mixing, and explain gas solubility in liquids, temperature effects, and vapor-pressure relationships.
Non-ideal Solutions10:19
Compare ideal and non-ideal solutions, explain the three conditions for ideal behavior, and show how A and B interactions cause positive or negative deviations and varied mixing behavior.
Abnormal Molar Masses10:12
Explore how abnormal molecular masses arise from association and dissociation, causing observed masses to differ from normal values, with boiling point, freezing point, and nmr spectroscopy revealing these anomalies.
Vant Hoff's factor8:55
Explain van't hoff's factor i, showing how molecular association or dissociation alters colligative properties like boiling and freezing point depressions, using observed versus normal properties to determine i.
Numerical - Molarity and Normality12:06
Master numerical problems in molarity and normality by calculating concentrations from mass, volume, and density, and applying these concepts to acids, solutions, and solution composition.
Numerical - Molality and Mole fraction11:42
Demonstrates calculating molality and mole fraction, plus mass percent, for ethanol-water and benzene-containing solutions, with density and solution composition as key tools.
Numerical on Boiling Point and Freezing Point10:16
Numerical on Vapour Pressure and Osmotic Pressure9:46
Solve numerical problems on vapor pressure and osmotic pressure using the given data, applying key relations to compute vapor pressure lowering and osmotic pressure in solutions.
Numerical based on Henry’s law9:27
Explore numerical problems based on Henry's law to solve pneumatic gas solubility and pressure calculations. Build exam-ready skills for CBC and related assessments with guided practice and stepwise solutions.
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Requirements

Description

A solution is a mixture in which substances are intermixed so intimately that they can not be observed as separate components”. The dispersed phase or the substance which is to be dissolved is called solute, while the dispersion medium in which the solute is dispersed to get a homogenous mixture is called the solvent.

Solubility : “Solubility of a substance may be defined as the amount of solute dissolved in l00 gms of a solvent to form a saturated solution at a given temperature”.

A saturated solution is a solution which contains at a given temperature as much solute as it can hold in presence of dissolving solvent. Any solution may contain less solute than would be necessary to saturate it.

When the solution contains more solute than would be necessary to saturate it then it is termed as supersaturated solution.

Kinds of solutions : All the three states of matter (gas, liquid or solid) may behave either as solvent or solute. Depending on the state of solute or solvent, mainly there may be following nine types of binary solutions.

Among these solutions the most significant type of solutions are those which are in liquid phase and may be categorised as,

(1) Solid in liquid solutions,

(2) Liquid in liquid solutions and

(3) Gas in liquid solutions.

Who this course is for:

Beginners and 12 grade students