Titration is the slow addition of one solution of a known concentration (called a titrant) to a known volume of another solution of unknown concentration until the reaction reaches neutralization, which is often indicated by a color change.

1. By : Hagar Ibrahem
Prof, Shimaa

2. chemical
analysis
Quantitative
analysis
Volumetric
analysis
Mass
analysis
Descriptive
analysis

3.  Titration is the slow addition of one solution of a
known concentration (called a titrant) to a known
volume of another solution of unknown concentration
until the reaction reaches neutralization, which is
often indicated by a color change.

4.  To be calibrated there must be several conditions
including :
1. Be a quick interaction
2. To be a single interaction without any accompanying
secondary interactions .
3. We can fully consider it
4. There is away we can determine the end of
interaction .

5. Acid base
H2o+
salt

6. Strong acid
+
Strong base
PH=7
Weak acid
+
Strong base
PH>7
Strong acid
+
Weak base
PH<7

7.  A measured volume of an acidic or basic solution of unknown
concentration is placed in a beaker. The electrodes of a pH meter
are immersed in this solution, and the initial pH of the solution
is read and recorded.
 A buret is filled with the titrating solution of known
concentration. This is called the standard solution, or titrant.
 Measured volumes of the standard solution are added slowly and
mixed into the solution in the beaker.
 The pH is read and recorded after each addition.
 This process continues until the reaction reaches the equivalence
point, which is the point at which moles of H+ ion from the acid
equal moles of OH- ion from the base.
MAVA = MBVB

8. MA = Molarity of the acid
VA = Volume of the acid
MB = Molarity of the base
VB = Volume of the base

11.  Add 15 ml from phosphoric acid solution to 38.5 ml
from sodium hydroxide solution with a concentration
of 0.15 M
 Calculate the molocal concentration of the phosphoric
acid solution if it occurs according to the following
reaction
 H3PO4 + NaOH H2O+ NaH2PO4
 H3PO4 +3 NaOH 3H2O+ Na3PO4

12. 𝑀𝐴𝑉𝐴
𝑎
=
𝑀𝐵𝑉𝐵
𝑏
 (Ma)(15 mL) = (0.15)(38.5 mL)
Ma = 0.385 M

13. Calculate the number of sodium
hydroxide moles you need for
neutralizing 0.2 mol of nitric acid
Answer
HNO3 + NaOH H2O + NaNO3
𝑀𝐴𝑉𝐴
𝑎
=
𝑀𝐵𝑉𝐵
𝑏
𝑛𝑎
𝑎
=
𝑛𝑏
𝑏
0.2
1
=
𝑛𝑏
1
Nb= 0.2 moler

14. what was concentration of the acid
solution ?
Ba(OH)2
0.0154
M
27.4
ml
HCL
??
M
20
ml

15.  Ma Va = Mb Vb
 Ma = ?? Va =20 ml na = 2
 Mb = 0.0154 M Vb = 27.4 ml nb = 1
X =0.0422 M
Ba(OH)2 + HCL H2O + BaCl222
(𝑥𝑀)(20𝑚𝐿)
2
=
(.0154𝑀)(27.4𝑚𝐿)
1

17.  Definition: A weak organic acid, that
has a different color than its conjugate
base, In-, with the color change
occurring over a specific and relatively
narrow pH range.

18.  is key in performing a successful titration reaction
 The purpose of the indicator is to show when enough
standard solution has been added to fully react with the
unknown concentration.
 However, an indicator should only be added when
necessary and is dependent upon the solution that is being
titrated. Therefore, indicators must only be added to the
solution of unknown concentration when no visible
reaction will occur.
 Depending on the solution being titrated, the choice of
indicator can become key for the success of the titration.

20.  The point at which the indicator used in a titration
changes color is called the end point of the titration.
 BUT for strong-strong titrations, the pH change is so
steep and so large, that the are approximately equal.
Equivalence
point
End
point

21. Acid-Base Indicators
Color on basic
side
Range of color
change
Color on acidic
side
Indicator
Violet0.0–1.6YellowMethyl violet
Blue3.0–4.6YellowBromophenol blue
Yellow3.1-4.4RedMethyl orange
Yellow4.4-6.3RedMethyl red
Blue5.0-8.0RedLitmus
Blue6.0-7.6YellowBromothymol blue
Pink8.3-10.0ColorlessPhenolphthalein
Red10.1-12.0YellowAlizarin yellow

22. equivalence point
14.0
12.0
10.0
8.0
6.0
4.0
2.0
0.0
0.0 10.0 20.0 30.0 40.0

23. Titration
Curve
PH
volume

24. Titration of a Strong Acid
With a Strong Base
Titration of a Weak Acid With
a Strong Base
equivalence
point
14.0
12.0
10.0
8.0
6.0
4.0
2.0
0.0
0.0 10.0 20.0 30.0
14.0
12.0
10.0
8.0
6.0
4.0
2.0
0.0
40.0
equivalence point
0.0 10.0 20.0 30.0
pH

25. Titration of a Weak Base
With a Strong Acid
equivalence point
14.0
12.0
10.0
8.0
6.0
4.0
2.0
0.0
0.0 10.0 20.0 30.0 40.0 50.0

26.  There are several reasons why titration is used in
laboratories worldwide:
 Titration is an established analytical technique.
 It is fast.
 It is a very accurate and precise technique.
 A high degree of automation can be implemented.
 Titration offers a good price/performance ratio compared
to more sophisticated techniques.
 It can be used by low-skilled and low-trained operators.
 No need for highly specialised chemical knowledge.