These slides represents the analytical techniques used for analysis of unknown samples.

1. Titration or Titrimetry

2. - Rishabh Sharma
(M.Sc. ES)
CEEES Department
Deen bandhu Chhotu ram University of
Science and Technology (DCRUST),
Murthal, Sonepat Haryana.

3. CONTENTS
• Introduction
• Principle of titration
• Terms used in titration
• Concentration Terms
• Titrimetric calculation
• Titrimetric apparatus
• Types of titration
• Fields of use
• Advantages of titration

4. Introduction
 A technique for determining the
concentration of a solution by
measuring the volume of one solution
needed to completely react with
another solution. Titration process
involves addition of solution of known
conc. from burette to the measured
volume of analyte.

5. Principle of titration
 Principle of titration:- It is based on the
complete chemical reaction between
the analyte and the reagent (titrant) of
known concentration.
Analyte + Titrant → Product

6. Terms used in titration Analyte
 Analyte:- The solution of unknown
concentration but known volume.
 Titrant:- The solution of known
concentration.

7.  Standard solution:- A solution of
known concentration is called the
standard solution.
 Types of standard solution:-
1) Primary standard:- It has certain
properties:
(a)Extremely pure.
(b)Highly stable.
(c) Can be weighed easily.
For e.g. Na2CO3.

8. 2) Secondary standard:- It has certain
properties:-
(a) Less pure than primary standard.
(b) Less stable than primary standard.
(c) Can not be weighed easily. For e.g.
NaOH, HCl

9. Equivalence Point
 Equivalence Point:- Point where the
amount of two reactants are just
equivalent .
 End point:- The point at which the
reaction seems to be complete, this
point is usually seen with the help of
indicator.

10. Indicator
 Indicator:- An auxiliary substance
which helps in the usual detection of
the completion of the titration process
at the end point.
 For examples:- Methyl orange,
Phenolphthalein, Cresol red, Thymol
blue.

11. Concentration Terms
 Concentration Terms:- The concentration
of standard solutions (titrants) are
generally expressed in units of either
molarity (CM, or M) or normality (CN, or
N).
 Molarity (M):-It is the number of moles of
a solute dissolved per liter of the
solution.
 Normality(N):- It is the gram equivalent
weight of solute dissolved per litre of
solution.
 Molality(m):- It is the number of moles of

12. Titrimetric calculation
 Titrimetric calculation:- It is based on the
following law of equivalence:-
NaVa = NsVs or MaVa = MsVs
 Where, Na is the normality of analyte.
 Va is the volume of the analyte.
 Ns is the normality of standard solution.
 Vs is the volume of standard solution
used.
 Ma is the molarity of analyte.
 Ms is the molarity of standard solution.

13. Titrimetric apparatus

14. Types of titration
 Types of titration:-
1.Acid-base titrations
2.Complexometric titrations
3.Redox titrations
4.Precipitation titrations

15. Acid – base
Titration(neutralization)
 Acid base Titration( neutralization):-
A sample of unknown concentration
of acid is estimated with a known
concentrated base or vice-verse.
acid + base → water + salt
HCl + NaOH ------> H2O + NaCl

16. Complexometric Titrations
 Complexometric Titrations:- As the
name indicates, the end point is
seems by formation of a complex
molecule. Here titrant and titrand react
to form a complex till end point is
reached. Once complex is formed, the
complex is stable and not further
reaction takes place.
Ca+2 + EDTA-4 ------> CaEDTA-2
Mg In + EDTA-4 ------> MgEDTA-2 +
-2

17. Redox titration
 Redox titration:- Redox titration is
based on the redox reaction
(oxidation-reduction) between analyte
and titrant.
For example:-
 6 Fe2+
+ 14 H+
+ Cr2O7
2-
=> 6 Fe3+
+
2Cr3+ + 7 H2O
 MnO4 –(Purple Pink) + 8 H+ + 5 Fe2+
==>Mn2+(colorless) + 5 Fe3+ + 4 H2O

18. Precipitation titrations
 Precipitation titrations:- The titrations
which are based on the formation of
insoluble precipitates, when the
solutions of two reacting substances
are brought in contact with each other,
are called Precipitation titration.
Ag+(aq)+ Cl−(aq)⇌ AgCl(s)

19. Fields of use
 Fields of use:- Titration is a widely
applied analytical technique. Some
areas where titration is used are
given below:-
 Agriculture, Oil Industry, Chemical
industry, Pharmaceuticals, Food
Industry.

20. Advantages of titration
 There are several reasons why titration is
used in laboratories worldwide:-
1)Titration is an established analytical
technique.
2)It is fast
3) It is a very accurate and precise technique.
4) Titration offers a good price/performance
ratio as compared to more sophisticated
techniques.
5) It can be used by low-skilled and low- trained
operators.