Solutions Chemistry Class 12 | Chapter 2 | CBSE NEET JEE

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Timestamps:
0:00 Introduction
0:45 Solutions
5:53 Solutions:Solvent&Solute
8:55 Solutions:BinarySolutions
9:29 Solutions:Types
9:53 Solutions:GaseousSolution
11:25 Solutions:Liquid Solution
12:37 Solutions:Solid Solution
14:45 Solutions:Concentration
17:15 Solutions:Quantitative concentration
17:52 Mass Percentage
19:36 Volume Percentage
21:05 Mass by VolumePercentage
22:16 Parts per million
25:30 Mole Fraction
27:17 Mole Fraction:Example
32:57 Molarity
34:58 Molarity:Example
38:07 Molality
40:42 Molality:Example
43:44 Solutions:Quantitative Concentration
45:50 Problem 1
48:08 Problem 2
56:17 Problem 3

In this video we will cover:
1.NCERT solutions class 12 Chemistry chapter 2 solutions
2.NCERT Class 12 Chemistry chapter 2 Solutions notes
3.What are solutions?
4.Difference between solution and solvent.
5.Explain binary solutions.
6.Different types of solutions.
7.Calculate the mole fraction of ethylene glycol (C2H6O2) in a solution containing 20% of C2H6O2 by mass.
8.Calculate the molarity of a solution containing 5 g of NaOH in 450 mL solution
9.Calculate molality of 2.5 g of ethanoic acid (CH3COOH) in 75 g of benzene
10.Calculate the mass percentage of benzene (C6H6) and carbon tetrachloride (CCl4) if 22 g of benzene is dissolved in 122 g of carbon tetrachloride
11.Solution of glucose in water is labelled as 10% w/w, what would be the molality and mole fraction of each component in the solution? If the density of solution is 1.2 g mL–1, then what shall be the molarity of the solution?
13.A solution is obtained by mixing 300 g of 25% solution and 400 g of 40% solution by mass. Calculate the mass percentage of the resulting solution.

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plz like for hard work😅
0:00 Introduction
0:45 Solutions
5:53 Solutions:Solvent&Solute
8:55 Solutions:BinarySolutions
9:29 Solutions:Types
9:53 Solutions:GaseousSolution
11:25 Solutions:Liquid Solution
12:37 Solutions:Solid Solution
14:45 Solutions:Concentration
17:15 Solutions:Quantitative concentration
17:52 Mass Percentage
19:36 Volume Percentage
21:05 Mass by VolumePercentage
22:16 Parts per million
25:30 Mole Fraction
27:17 Mole Fraction:Example
32:57 Molarity
34:58 Molarity:Example
38:07 Molality
40:42 Molality:Example
43:44 Solutions:Quantitative Concentration
45:50 Problem 1
48:08 Problem 2
56:17 Problem 3
THANKS ME LATER❤

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Timestamps:
0:00 Introduction
0:45 Solutions
5:53 Solutions:Solvent&Solute
8:55 Solutions:BinarySolutions
9:29 Solutions:Types
9:53 Solutions:GaseousSolution
11:25 Solutions:Liquid Solution
12:37 Solutions:Solid Solution
14:45 Solutions:Concentration
17:15 Solutions:Quantitative concentration
17:52 Mass Percentage
19:36 Volume Percentage
21:05 Mass by VolumePercentage
22:16 Parts per million
25:30 Mole Fraction
27:17 Mole Fraction:Example
32:57 Molarity
34:58 Molarity:Example
38:07 Molality
40:42 Molality:Example
43:44 Solutions:Quantitative Concentration
45:50 Problem 1
48:08 Problem 2
56:17 Problem 3

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INTRODUCTION
In normal life we rarely come across pure substances. Most
of these are mixtures containing two or more pure
substances. Their utility or importance in life depends on
their composition. The air around us is a mixture of gases
primarily oxygen and nitrogen; the water we drink contains
very small amounts of various salts dissolved in it. Our blood
is a mixture of different components. Alloys such as brass,
bronze, stainless steel, etc. are also mixtures. In this Unit,
we will consider mostly liquid solutions and their properties.
1. SOLUTIONS
1.1 Definition
A solution is a homogeneous mixture of two or more than
two components.
1.3 Strength of Solutions
The amount of solute dissolved per unit solution or
solvent is called Strength of solution. There are various
methods of measuring strength of a solution. :
1. Mass Percentage (%w/w):
“It represents mass of a component present in 100 g of
solution”
Mass of component in the sol. Mass % of a component 100
Total Mass of sol.


2. Volume percentage (%v/v):
“It represents volume of a component in 100 mL of solution”
Vol. of component Vol. % of a component = ×100
Total vol. of solution
For example, common salt in water.
1.2 Classification
Solutions which contain two components in it are called
Binary Solutions.
Substances which are used to prepare a solution are called
as Components.
The component that is present in the largest quantity is
known as Solvent. Solvent determines the physical state in
which solution exists.
The other component present in lesser quantity in the
solution is termed as Solute.

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[rudrapratap]

0:00 Introduction
0:45 Solutions
5:53 Solutions:Solvent&Solute
8:55 Solutions:BinarySolutions
9:29 Solutions:Types
9:53 Solutions:GaseousSolution
11:25 Solutions:Liquid Solution
12:37 Solutions:Solid Solution
14:45 Solutions:Concentration
17:15 Solutions:Quantitative concentration
17:52 Mass Percentage
19:36 Volume Percentage
21:05 Mass by VolumePercentage
22:16 Parts per million
25:30 Mole Fraction
27:17 Mole Fraction:Example
32:57 Molarity
34:58 Molarity:Example
38:07 Molality
40:42 Molality:Example
43:44 Solutions:Quantitative Concentration
45:50 Problem 1
48:08 Problem 2
56:17 Problem 3

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After this video
Ma'am : we have so much sugar and salt solution. What should we do now?
Me : Let's make shikanji
😂😂🤣🤣