As a science student, you always look for chemistry formulas for class 12 pdf to download and use offline. After reading this article, chemistry class 12 all formulas pdf can be downloaded.
Class 12 Chapter 1 Solutions Chemistry Formulas List
7).Molarity (M) = `\frac{\text{mass of solute}}{\text{molar mass of solute}} \times \frac{1000}{\text{volume of solution in mL}}`
14).Mole fraction of solute (`X_A`)= `\frac{n_A}{n_A + n_B}`
15).Mole fraction of solute (`X_B`)= `\frac{n_B}{n_A + n_B}`
16). Solubility of a Gas in a Liquid (Henry’s law)
P= KHX [KH = Henry’s law constant, X= mole fraction of gas, P= partial pressure]
17). Raoult’s law [Partial vapour pressure of two components of solution]
`P_A= P_A^o X_A`
`P_B= P_B^o X_B`
Where
[ `P_A` & `P_B` are partial pressure of components A &B
`P_A^o` & `P_B^o` are vapour pressure in a pure state, `X_A` & ` X_B` mole fractions of A and B in solution.]
18). Lowering of Vapour Pressure
`X_B = \frac{P_A^0 - P_A}{P_A^0}`
`X_B = \frac{n_B}{n_A + n_B}`
`X_B = \frac{W_B/M_B}{W_A/M_A + W_B/M_B} = \dfrac{W_B M_A}{W_A
M_B + W_B M_A}`
Where
[`X_B` = mole fraction of solute,
`n_A` and `n_B` are the number of moles of solvent and
solute respectively,
`W_B` and `W_A`are the masses of solute and solvent,
`M_A` and `M_B` are the molecular masses of solvent
and solute.]
19). Elevation
of boiling point
`∆T_b=K_b m`
Where
[`∆T_b`=elevation of boiling point,`K_b`=molal elevation constant,m=molality of solution]
20). Depression
of Freezing point
`∆T_f= K_f m`
Where
`∆T_f`= depression in freezing point,
`K_f` = molal elevation constant,
m =molality of solution.
21). Calculation
of molecular mass of an unknown non-volatile compound from depression of
freezing point
`M_B=\frac{K_f}{∆T_f} × \frac{W_B}{W_A} ×1000`
Where
MB= molar
mass of solute
WA= mass of solvent
WB= mass of solute
22). Osmotic
pressure
`Ï€=\frac{n}{V} RT or `Ï€=CRT`
Where
23). Calculation
of molar mass from osmotic pressure
`M_B=\frac{W_B RT}{Ï€V}`
Where
MB= molecular
weight of solute
WB= mass of solute
24). Van’t Hoff’s factor
`i = \frac{\text{normal molar mass}}{\text{abnormal molar mass}}`
After reading this, the class 12 chemistry solutions formulas pdf can be downloaded from the given link below
`i = \frac{\text{observed colligative
property}}{\text{theoretical colligative property}}`
`i = \frac{\text{Total number of moles of particles after
association/dissociation}}{\text{Number of moles of particles before
association/dissociation}}`
Where
i= Van't Hoff's factor
Here you have been given all formulas of chemistry class 12 chapter-wise pdf
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All Formula of Solid State Class 12
1.`\text{Packing efficiency} = \frac{\text{volume occupied by atoms}}{\text{volume of unit cell}}\times100`
i.`\text{Packing efficiency in hcp and ccp} = \frac{\text{volume of 4 speheres}}{\text{Total volume of unit cell}}\times100`
ii.`\text{Packing efficiency in bcc}= \frac{\text{volume of 2 speheres}}{\text{Total volume of unit cell}} \times100`
iii. `\text{Packing efficiency in simple cubic cell}= \frac{\text{volume of 1 speheres}}{\text{Total volume of unit cell}} \times100`
2. Calculations involving unit cell dimensions
i. Mass of unit cell = `z\times m`
[z= number of atoms, m=mass of atom]
ii.Mass of atom(m)= `\frac{M}{N_A}`
[M= molar mass, NA= Avogadro number]
iii.Density of unit cell(d)= `\frac{n\ \times\ M}{a^3\ \ \ \ \times\ \ N_A}`
[n= number of atoms, M=molar mass, a=edge length of unit cell, NA= Avogadro number]
3. Relation between distance (d) and the edge(a) of the unit cell
i. For simple cell d = a
ii.For fcc `d=\ \frac{a}{\sqrt2}`
iii.For bcc `d=\ \frac{\sqrt3a}{2}`
4. Relation between atomic radius (r) and the edge (a) of the unit cell
i.For simple cell `r=\frac{a}{2}`
ii.For fcc ` r=\frac{a}{2\sqrt2}`
iii.For bcc `r=\frac{\sqrt3a}{4}`
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