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Some Basic Concepts of Chemistry
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Aditya Singh
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Outline
Basic Concepts of
Chemistry
Mole Facts
1 Mole =
Atomic/Molecular
weight of
element/compound
(in grams)
1 Mole of
atoms
Gram Atomic
Mass
6.022×1023
1 Mole of
Molecules
Gram
Molecular
Mass
22.4L at S.T.P.
6.02×1023
Molecules
Mole-related
Formlae
Number of
entities/Avogadro's
number = Moles(n) =
Mass of substance/
Molar Mass
No. of entities = Moles
X Avogadro's Number
Molar Mass (M) = Sum
of the atomic masses of
the elements present in
a molecule.
Avogadro's No.(NA) =
6.022×1023
Definition:No. of atoms/
molecules present in one
moleof an element/
compound.
Atomic mass (A) =
Mass of 1 mole of atom
Mole of atoms/molecules/
ions/electrons = (No. of
atoms/molecules/ions/
electrons)/Avogadro's No.
Percentage
Composition (mass %)
= No. of parts by mass
of the element or
contituents/ Molecular
mass of the compound x 100
Empirical
Formula vs
Molecular
Formula
Molecular Formula =
n x Empirical Formula
Mass/Volume =
Density
Mole Concept
in Solutions
Mass percent (%) =
(mass/given mass of
solute)/mass of given
solution x 100
Mole fraction (x) = No.
of moles of the component/
total no. of moles of the
component
Mole fraction of the solute =
(Xa) - nA/nA+nB
Molarity (M) = No. of the
moles of the solute(n)/Volume
of the solution in litres (V),
where n-w(given mass) /
(molar mass)
If the solution of
molarity M1 & volume
V1 is diluted to volume
V2 and its new molarity
M2, no. of moles of the solute
does not change. Hence,
M1V1 = M2V2
Molality (m) - no.of
moles of the solute
(n)/mass of solvent in
kg, where n-w(given
mass)/(molar mass)
Parts per million
(ppm) = mass of the
component/mass of
solution x 106
