Empirical formula and molecular formula:

✅ Empirical formula and molecular formula:

➖Molecular Formula:-

Represents the actual number of each individual atom in any molecule is known as molecular formula. 

➖Empirical Formula:-

Expresses the smallest whole number ratio of the constituent atom within the molecule. 

Molecular formula = (Empirical formula)n

Molecular weight = n × Empirical weight

also,

Molecular weight = 2 × Vapour density 

➖Limiting Reagent:

The reactant which is totally consumed during the course of reaction and when it is consumed reaction stops.

For a balanced reaction reaction:

A +B →  C + D

B would be a limiting reagent if nA / nB>nB/nA

Similarly, A is a limiting reagent if nA / nB<nB/nA

♻️ Concentration of the solutions:

➖Mass by Mass Percentage:-

Amount of solute in gram present per 100 gm of the  solution. 

Mass percentage of solute = [(Mass of solute)/(Mass of solution)] x100

➖Mass by Volume Percentage:-

Amount solute in gram present per 100 mL of the solution.

➖Volume by Volume Percentage:-

Volume of solute per 100 mL of the solution

Volume by volume percentage of solute = [(Volume of solute)/(volume of solution)] x100 

➖Parts per million ( ppm) :-

The amount of solute in gram per million (106) gram of the solution.

ppm = [(mass of solute/mass of solution)]x 106 

➖Mole fraction:-

Ratio of the moles of one component of the solution to the total number of moles of solution

Total mole fraction of all the components of a solution is equal to 1.

For binary solutions having two components A and B

Mole fraction of A   

XA =  (nA)/(nA+nB)]

Mole fraction of B

 XB =  (nB)/(nA+nB)] 

or  XB = 1- XA

➖Molarity(M):-

Number of moles of solute per 1000 mL of the solution.

M =  (Number of moles of solute)/(Volume of solution in L)  

➖Molality(m):-

number of moles of solute per 1000 gram of the solvent.

m =  (Number of moles of solute)/(Weight of solvent in kg)