CBSE Class 12 Chemistry Solutions Chapter 1 Notes

CBSE Class 12 Chemistry Solutions Chapter 1 Notes

Class 12 Chemistry Solutions explores the concept of solutions, including definitions, classifications, and strength measurements. Key topics include the types of solutions, such as gaseous, liquid, and solid solutions, along with methods for calculating mass percentage, volume percentage, and molarity. This resource is essential for CBSE students preparing for exams, providing detailed explanations of Raoult's Law, colligative properties, and the impact of temperature on solubility. It serves as a comprehensive guide for understanding the principles of solutions in chemistry.

Key Points

  • Defines solutions and categorizes them into gaseous, liquid, and solid types.
  • Explains the strength of solutions through mass percentage, volume percentage, and molarity calculations.
  • Covers Raoult's Law and its application to volatile and non-volatile solutes.
  • Discusses colligative properties, including vapor pressure lowering and boiling point elevation.
  • Taslima Sarah
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Class XII Chemistry www.vedantu.com 1
Revision Notes for Class 12 Chemistry
Chapter 1 – Solutions
1.1 Definition
A solution is a mixture of two or more components that is homogeneous.
Take, for instance, ordinary salt in water.
1.2 Classification
Binary solutions are solutions that have two components in them. Components are substances
that are used to make a solution.
The solvent is the component that is present in the greatest quantity. The physical condition of
a solution is determined by the solvent.
Solute refers to the other component in the solution that is present in smaller amounts.
Each element could be solid, liquid, or gaseous.
Types of
Solution
Solute
Solvent
Common Examples
Gaseous
Solutions
Gas
Gas
Oxygen and nitrogen gas mixture
Liquid
Gas
a mixture of chloroform and nitrogen
gas
Solid
Gas
nitrogen gas with camphor
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Liquid
Solutions
Gas
Liquid
Water with oxygen dissolved in it
Liquid
Liquid
Ethanol is a liquid that can be
dissolved in water.
Solid
Liquid
Glucose that has been dissolved in
water
Solid
Solutions
Gas
Solid
Hydrogen solution in palladium
Liquid
Solid
Mercury and sodium amalgam
Solid
Solid
dissolving copper in gold
1.3 Strength of Solutions
Strength of solution refers to the amount of solute dissolved per unit of solution or solvent.
There are several methods for determining the strength of a solution.
1. Mass Percentage (%w/w): “It denotes the mass of a component in 100 g of solution.”
Mass
%
of a component
Mass of component in the sol.
100
Total Mass of sol.
=
2. Volume Percentage (%v/v): "It represents the volume of a component in a solution of
100 mL
."
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Volume
%
of a component
3. Mass by Volume Percentage (% w / v): "It denotes the mass of the solute in grams in
100 mL
of solution."
Mass by vol, percent
Mass of solute in g
100
Vol. of sol. in mL
=
4. Parts Per Million (ppm):
Parts per million
6
No. of parts of the component
10
Total no. of all the components of sol.
=
Mass to mass, volume to volume, and mass to volume are all ways to express concentration in
parts per million.
5. Mole Fraction (x): "It denotes the number of moles of a solute in one mole of solution."
Mole fraction
No. of molos of the component
Total no. of moles all the components
=
If the amount of moles of
A
and
B
in a binary mixture is
A
n
and
B
n
, respectively, the mole
fraction of
A
will be
A
A
AB
n
x
nn
=
+
6. Molarity, M: "It represents the number of moles of solute in 1 litre of solution."
Molarity,
Moles of solute
M
Vol. of sol in L
=
Molarity is measured in milligrams per litre and is denoted by the letters '
M
' or 'Molar.' "The
density of a solution is its mass per unit volume."
Density,
Mass of sol.
d m/ V
Vol. of sol.
==
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End of Document
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FAQs of CBSE Class 12 Chemistry Solutions Chapter 1 Notes

What are the different types of solutions covered in this chapter?
This chapter categorizes solutions into three main types: gaseous, liquid, and solid solutions. Gaseous solutions include mixtures like oxygen and nitrogen gases. Liquid solutions are exemplified by mixtures such as water with dissolved oxygen or glucose. Solid solutions are represented by examples like alloys, where metals like copper are dissolved in gold. Each type is defined by the state of the solute and solvent, highlighting their unique characteristics.
How is the strength of a solution measured?
The strength of a solution can be measured using several methods, including mass percentage, volume percentage, and molarity. Mass percentage indicates the mass of solute in 100 grams of solution, while volume percentage represents the volume of solute in 100 mL of solution. Molarity measures the number of moles of solute per liter of solution. These calculations help in understanding the concentration of solutions, which is crucial for various chemical applications.
What is Raoult's Law and its significance in chemistry?
Raoult's Law states that the partial vapor pressure of each component in a solution of volatile liquids is directly proportional to its mole fraction. This principle is significant as it allows chemists to predict how the vapor pressure of a solution will change when different solutes are added. It applies to both volatile and non-volatile solutes, providing a foundational understanding of how solutions behave under varying conditions, which is essential for fields like physical chemistry and chemical engineering.
What are colligative properties and why are they important?
Colligative properties are characteristics of solutions that depend on the number of solute particles rather than their identity. Key colligative properties include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. These properties are important because they influence how solutions behave in different environments, impacting processes such as boiling, freezing, and osmosis. Understanding these properties is crucial for applications in chemistry, biology, and various industrial processes.

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