Volumetric analysis

            Volumetric analysis is a quantitative analysis. It involves the measurement of the volume of a known solution required to bring about the completion of the reaction with a measured volume of the unknown solution.

         Titration : The process of addition of the known solution from the burette to the measured volume of solution of the substance to be  estimated until the reaction between the two is just done, is known as titration. Thus, a titration involves two solutions;

      (i) Unknown solution : The solution consisting the substance to be estimated is termed unknown solution. The substance is termed titrate.

      (ii) Standard solution : The solution in which an accurately known amount of the reagent (titrant) has been dissolved in a known volume of the solution is termed standard solution. There are two types of reagents (titrants) :

         (a) Primary standards : These can be accurately weighed and their solutions are not to be standardised before use. Oxalic acid (H₂C₂O₄.2H₂O), potassium dichromate (K₂Cr₂O₇), silver nitrate (AgNO₃), copper sulphate (CuSO₄.5H₂O), ferrous ammonium sulphate [FeSO₄(NH₄)₂SO₂.6H₂O], sodium thiosulphate (Na₂S₂O₃.5H₂O), etc., are the examples of primary standards.

        (b) Secondary standards : The solutions of these reagents are to be standardised before use as these cannot be weighed accurately. The examples are potassium hydroxide (KOH), sodium hydroxide (NaOH), hydrochloric acid (HCl), potassium permanganate (KMnO₄), iodine, sulphuric acid (H₂SO₄)etc.

         Law of equivalence : It is applied in all volumetric estimations. According to it, the chemical substances react in the ratio of their chemical equivalent masses.

         or gram equivalent of A = gram equivalent of B

         or milli-gram equivalent of  A = milli-gram equivalent of B

         The point at which the amounts of the two reactants are just equivalent is known as equivalence point or end point. An auxiliary substance which helps in the usual detection of the completion of the titration or equivalence point or end point is termed as indicator, i.e., substances which undergo some easily detectable changes at the equivalence point are used as indicators.

Methods of showing concentrations of solutions

         The concentration of a solution can be given in several ways.

         (1) Percent by mass

         (2) Molarity

         (3) molality

         (4) Mole fraction

         (5) Normality

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