FREE ESSAY ON TITRATION

TITRATION

Titration
Problem: When adding acids and bases what is the titration of the two?
Research:
Amounts of reactants and products in a reaction are commonly investigated in two ways in
the lab, gravimetrically (by mass), and volumetrically (by volume and concentration).
Titration is the name we give to the process used to determine the volume of a given
solution needed to react with a given mass or volume of a sample. We will use the
quantitatively study a neutralization reaction, in a neutralization reaction an acid and
base are combined to produce a salt water. Phenolphthalein will be used as the indicator
in this experiment. This indicator is clear in the acidic solution, dark purple or pink
in the basic solution and light pink in the solution that has reached its equivalence
point. This is the point when the number of moles of acid equal the number of moles of
base.
Procedure:
1. Obtain two burettes. Clean and rinse both with distilled water. Each burette is
labeled acid or base. Rinse the burette labeled acid with a few ml of HCl and allow to
drain into the sink with ample water. Now fill the burette with about 40ml of the HCl.
Repeat the rinsing and filling procedure with the base using the NaOH of unknown molarity
in the burette labeled base.
2. Record the volume in each burette by reading the bottom of each meniscus to the
nearest .01ml.
3. Add 15ml of acid to a 250ml Erlenmeyer flask, then add 3 drops of phenolphthalein to
the flask.
4. Holding the neck of the Erlenmeyer flask with one hand and manipulating the burette
with the other add some base and gently swirl the flask so the solution will mix.
Continue adding base until the first faint pink color develops. If the pink disappears
upon mixing the solution add more base drop by drop until pink color persists for at
least 10 seconds.
5. Once the equivalence point has been reached record the volume in each burette again by
reading the bottom of each materials.
6. Rinse the contents of the Erlenmeyer flask down the drain and rinse the flask with
distilled water. Refill the burettes with the proper solutios.
7. Repeat the titration at least two more times starting with step #2.
8. After completing all three trials and collecting the necessary data clean up the lab
as directed by your instructor.
Materials:
1. 2 burettes
2. distilled water 
3. ample water
4. NaOH
5. Erlenmeyer flask 
6. HCL
Observations
Trial #1 1ml 12.3ml 15ml
Trial #2 12.3ml 22.8ml 15ml
Trial #3 22.8ml 33.7ml 15ml
A. #1= (.20)(.0113)= Molarity 2.26
B. #2 =(.20)(.0105)=Molarity 2.1
C. #3=(.20)(.0109)= Molarity 2.18
15-11.3 x 100 = 24% Error
15
15-10.5 x 100 = 30% Error
15
15-10.9 x 100 = 27% Error
15
Balanced Chemical Equation
HCl + NaOH a H2O + NaCl
Discussion:
When pouring the last amount of base right before it turned pink accidentally a lot was
poured so it might have had too much. The base also over flowed and poured out all over
the place. The bottom part of the meniscus fell out so the results might have been a
little off.
Conclusion:
There wasn't a lot of error compared to how many problems occurred. The acid and based
diluted causing neutralization. Because of the neutralization a color change occurred.
The results of the titration were similar, meaning that the experiment conducted was
correct all three times. The molarity found in the observation were around the same also.
Therefore the experiment worked as planned and the titration of the acid and bases became
neutralized.