Download CBSE Class 12 Chemistry Important Formulas All Chapters in PDF format. All Revision notes for Class 12 Chemistry have been designed as per the latest syllabus and updated chapters given in your textbook for Chemistry in Standard 12. Our teachers have designed these concept notes for the benefit of Grade 12 students. You should use these chapter wise notes for revision on daily basis. These study notes can also be used for learning each chapter and its important and difficult topics or revision just before your exams to help you get better scores in upcoming examinations, You can also use Printable notes for Class 12 Chemistry for faster revision of difficult topics and get higher rank. After reading these notes also refer to MCQ questions for Class 12 Chemistry given our website
Important Formulas Class 12 Chemistry Revision Notes
Class 12 Chemistry students should refer to the following concepts and notes for Important Formulas in standard 12. These exam notes for Grade 12 Chemistry will be very useful for upcoming class tests and examinations and help you to score good marks
Important Formulas Notes Class 12 Chemistry
Solution
1. Mole fraction (x)
if the number of moles of A and B are nA and nB respectrively, the mole fraction of A and B will be
XA= X/nA+nB , AND XB = nB / nA+nB
2. Molarity (M) = Moles of solute/ Volume of solution in litres
3. Moality (m) = Moles of solute / Mass of solvent in kilograms
4. Parts per million (ppm) = Number of parts of the component 106 / Total number of parts of all components of the solution
5. Raoult's law for a solution of volatile solute in volatile solvent :
pA = pA° xA
pB = pB° xB
Where pA and pB are partial vapour pressures of component 'A' and component 'B' in solution. pA° and pB° are vapour pressures of pure components 'A' and 'B' respectively.
6. Raoults law for a solution of non-volatile solute and volatile solvent :
p °A – p °A/ p °A = i nB /nA = i WB* MA / MB* WA (for dilute solution)
Where xB is mole fraction of solute, i is van't Hoff factor and A A
p °A – p °A / pA ° IS N relative lowering of vapour pressure.
7. Elevation in boiling point (ΔTb)
ΔTb = i.Kb m
where ΔTb = Tb – Tb°
Kb = molal boiling point elevation constant
m = molality of solution.
8. Depression in freezing point (ΔTf)
ΔTf = i.Kf m
where ΔTf = Tf° – Tf
Kf = molal depression constant
m = molality of solution.
9. Osmotic pressure (π) of a solution
πV = inRT or π = i CRT
where π = osmotic pressure in bar or atm
V = volume in litres
i = Van't Hoff factor
c = molar concentration in moles per litres
n = number of moles
T = Temperature on Kelvin Scale
R = 0.083 L bar mol–1 K–1
R = 0.0821 L atm mol–1 K–1
10. Van't Hoff factor (i)
i = Observed colligative property/Theoretically calculated colligative property
i = Normal molar mass/Abnormal molar mass
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