1 Mole =Atomic/Molecularweight of element/compound(in grams)

Number ofentities/Avogadro'snumber = Moles(n) = Mass of substance/Molar Mass

No. of entities = MolesX Avogadro's Number

Molar Mass (M) = Sumof 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.

PercentageComposition (mass %)= No. of parts by massof the element or contituents/ Molecularmass of the compound x 100

Molecular Formula =n x Empirical Formula

Mass/Volume = Density

Mass percent (%) = (mass/given mass of solute)/mass of givensolution 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 & volumeV1 is diluted to volumeV2 and its new molarity M2, no. of moles of the solutedoes not change. Hence, M1V1 = M2V2

Molality (m) - no.ofmoles of the solute(n)/mass of solvent inkg, where n-w(given mass)/(molar mass)

Parts per million(ppm) = mass of thecomponent/mass of solution x 106