Chemistry > Stoichiometry > 4.0 Volumetric Analysis
Stoichiometry
1.0 The Mole
2.0 The Limiting Reagent
3.0 Gravimetric Analysis
4.0 Volumetric Analysis
5.0 Calculation of n-factor
6.0 Redox Reactions
7.0 Titration
7.1 Simple Titration
7.2 Double Titration
7.3 Method
7.4 Titration of the solution containing both $N{a_2}C{O_3}$ and $NaHC{O_3}$
7.5 Titration of the solution containing both $NaOH$ and $N{a_2}C{O_3}$
7.6 Back Titration
8.0 Iodimetric and Iodometric Titrations
9.0 Volume strength peroxide solution
10.0 Percentage Labeling of Oleum
11.0 Hardness of Water
4.2 Molarity $(M)$
7.2 Double Titration
7.3 Method
7.4 Titration of the solution containing both $N{a_2}C{O_3}$ and $NaHC{O_3}$
7.5 Titration of the solution containing both $NaOH$ and $N{a_2}C{O_3}$
7.6 Back Titration
The no. of moles of solute present in one litre of solution is called the
molarity $(M).$
Molarity = $\frac{{{\text{No}}{\text{. of moles of solute}}}}{{{\text{Volume of solution in litre}}}}$
or Molartiy $=$ $\frac{{Wt.{\text{ of solute/Molecular wt}}{\text{. of solute}}}}{{Volume{\text{ }}of{\text{ }}solution{\text{ in litre}}}}$
So, no. of moles of solute $=$ Volume of solution (in litre) $ \times $ Molarity of solution.