2. Introduction
• Titration is simply defined as the procedure wherein an
acid reacts with a base, whose volumes are known and
concentrations are unknown. Using the known values, the
concentration of the compound (analyte or titer) can be
calculated by reacting or neutralizing it with another
chemical compound called titrant
3. •
• In this experiment involving a reaction between sodium
hydroxide (titrant) and sulfuric acid (titer), an indicator
called phenolphthalein is used. It is colorless in acids,
and its endpoint is marked by a color change to pink,
when the entire volume of the analyte has reacted with
a small amount of the titrant.
• H2SO4 + 2NaOH → Na2SO4 + 2H2O
4. • .
• The molecular formula of sulfuric acid is H2SO4. It is a highly
corrosive acid made from sulfur dioxide, and is known to be
among the most extensively used products in the chemical
industry. Sodium hydroxide (NaOH) is also an important base
that is used in factories, which is involved in the manufacture of
cleaning products, water purification techniques, and paper
products. This compound is a strong alkali, and is also known as
lye and/or caustic soda. The following paragraphs will explain
the entire titration procedure in a classic chemistry experiment
5.
6. Principles
•
The sulphuric acid has an unknown concentration. Then
you will fill a BURETTE with sodium hydroxide (a base)
that has a known concentration. ... Finally, the sodium
hydroxide in the burette is added to the acid/indicator
solution until the indicator changes colour
7. phenolphthalein
• Phenolphthalein is an acid-base indicator that is colorless
in acidic solutions and pink in basic solutions.
If phenolphthalein is added to the original sample
of sulfuric acid, the solution is colorless and will remain so
while hydrogen ions are in excess
8. Procedures
1. CAREFULLY pour 20mL of H2SO4 into a 100mL
graduated cylinder
2. CAREFULLY pour the measured H2SO4 from the
100mL graduated cylinder into a 100 mL beaker.
Rinse the graduated cylinder in the sink.
9. 3. Add 2-3 drops of Phenolphthalein and a stir bar to the H2SO4.
4. Have the burette loaded by the instructor and replace it in the
burette stand
5. Now, hold the flask just below the burette tip, and slowly turn
the stopcock so as to release the NaOH solution in a drop-
by-drop manner into the beaker
10. 6. When a slight pink color can be seen in the mixture, stop
adding the base by turning off the stopcock
7. See if the pink color disappears. If it remains, then the
reaction is complete, and if the mixture again turns
colorless, then start adding the base slowly till a color
change is noticed
11. 8. Record the reading of the volume of NaOH used to react
with the acidic solution. This is done by observing the
position of the lower meniscus in the burette
13. Introduction
• You can use the technique of titration to determine the
concentration of a sodium carbonate solution using a
solution with a known concentration of hydrochloric
acid, or vice versa.
14. Principle
• Na2CO3 IS ASALT OF STRONG BASE NAOH AND WEAK
ACID H2CO3 IT CAN BE ANALYZED USING ACIDIC
TITRANT HCL ACCORDING TO THE FOLLOWING
STEPWISE EQUATIONS
16. procedure
• ADD 10ML Na2CO3 +10 DROP PHPH AND TITRATION
BY 0.95 HCL END POINT FIRST FINT PINK COLOR
17. • Phenolphthalein is a good indicator for the first reaction
because it responds to the pH change caused by the
formation of sodium hydrogen carbonate It is pink in basic
solutions and turns colorless as soon as the solution
becomes acidic. Methyl orange, on the other hand, responds
to pH changes associated with the formation of NACL,
changing from yellow to red as the solution becomes more
acidic. At neutrality, it is a distinct orange color
18. • Measure out a suitable amount of a sodium carbonate
solution of unknown concentration and a hydrochloric
acid solution of known concentration in separate
graduated beakers
• Put a few drops of phenolphthalein in the sodium
carbonate solution. The indicator will turn pink
19. • Carefully add HCL to sodium carbonate solution until
the solution becomes colorless. Record the volume of
HCL solution you added
• Calculate the number of moles of HCL in the original solution and
derive from this the number of moles of Na2CO3 in the target
solution, keeping in mind that 1 mole of HCL reacts with 1 mole of
Na2CO3. Determine the concentration of the Na2CO3 solution using
a volumetric analysis
20. • In this part of the titration, HCL is reacting with NaHCO3, but the
proportion is still one mole to one mole. After MOLARITY
calculations and a volumetric analysis, the results should be
identical to those using phenolphthalein
21. conclusion
• At the end in our presentation we should know The
difference between the neutralization analytical and
complex analytical
22. In chemistry, neutralization is a chemical reaction in which acid
and a base react quantitatively with each other. In a reaction in
water, neutralization results in there being no excess of hydrogen
or hydroxide ions present in the solution. The pH of the
neutralized solution depends on the acid strength of the reactants
23. Complex analysis, traditionally known as the theory of functions of a
complex variable, is the branch of mathematical analysis that investigates
functions of complex numbers. It is useful in many branches of
mathematics, including algebraic geometry, number theory, analytic
combinatorics, applied mathematics; as well as in physics, including the
branches of hydrodynamics, thermodynamics, and particularly quantum
mechanics. By extension, use of complex analysis also has applications in
engineering fields such as nuclear, aerospace, mechanical and electrical
engineering
