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Class XII Chemistry Ch 2: Solutions Important formulae & Concepts
Number of moles of solute Molarity Volumeof solution in litres = 6 Number of moles of solute Molality Mass of solvent in kilograms = 7 Number of gram |
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Class XII Chemistry Ch 2: Solutions Important formulae & Concepts 1 Mass percentage of a component (w/w) = Mass of component in solution 100 Toal mass of solution × 2 Volume percentage of a component (v/v) Volume of the component = 100 Total volume of solution × 3 Mole fraction of a component (x) = Number of moles of the component |
What is chemical formula Class 12?
The chemical formula of a compound means the symbolic representation of the composition of a compound.
A chemical formula for a molecule is represented by the group of symbols of the elements that constitute the molecule, and the number of atoms of each element present in one molecule.What is the formulae of solution?
Once the molecular weight of the solute is known, the weight of chemical to dissolve in a solution for a molar solution less than 1M is calculated by the formula: grams of chemical = (molarity of solution in mole/liter) x (MW of chemical in g/mole) x (ml of solution) ÷ 1000 ml/liter.
There are three types of chemical formulae:
Molecular Formula.
Empirical Formula.
Structural Formula.
Osmotic Pressure
Osmotic Pressure is the best colligative property to determine the molecular weight of non-volatile substances. byjus.com
Types of Solutions
Fluids in the body generally aren’t found in pure forms. They are usually found in three types of solutions: isotonic, hypotonic and hypertonic. 1. Isotonic solutions – An isotonic solution has the same solute concentration as another solution. 2. Hypotonic solution –A hypotonic solution has a lower solute concentration than another solution. 3. Hy
Van’T Hoff Correction Factor
To explain the abnormal values of colligative properties and consequently molecular masses a correction factor known as Van’t Hoff Factor is employed. byjus.com
Relative Lowering of Vapour Pressure
It is the ratio of lowering of vapour pressure to vapour pressure of pure solvent. Relative lowering of vapour pressure is byjus.com
Raoult’s Law
The partial pressure of a solvent is equal to the product of mole fraction of the solvent and its vapour pressure in a pure state. byjus.com
Determination of Molecular Mass of A Solute
Measurement of boiling point elevation or freezing point depression using Beckmann thermometer is a convenient method for the determination of the molecular masses of the solutes. In fact, it is a method of determining the number of moles of the solute particles present in a solution. Mass of solute present in 1kg solvent. Using the relation Simila
Ideal Solutions
The solutions are said to be ideal if they fulfil the following requirements. They obey Raoult’s law ΔHmix= 0 ΔVmix= 0 In case of ideal solutions, the vapour pressure of the solution is a linear function of mole fraction. byjus.com
Non-Ideal Solution with Positive Deviations
Non-ideal solutions exhibit positive deviations from Raoult’s law. In such solutions. ΔHmix> 0 ΔVmix> 0 The vapour pressure of the solution, in this case, is always larger than that expected from ideal behaviour. byjus.com
Non-Ideal Solution with Negative Deviations
Non-ideal solutions exhibit negative deviations from Raoult’s law. In such solutions. ΔHmix< 0 ΔVmix< 0 The vapour pressure of the solution, in this case, is always smaller than that expected from ideal behaviour. byjus.com
Henry Law
Henry law deals with the variation of solubility of gases in liquids with pressure. It states that solubility of gas at a given temperature is directly proportional to the pressure at which it is dissolved. This expression is identical with Raoult’s law for a volatile solute. All systems which obey Raoult’s law must satisfy Henry’s law, but the rev
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