Larkin Lab Report- Titration
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Transcript of Larkin Lab Report- Titration
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7/28/2019 Larkin Lab Report- Titration
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Cristian Rodriguez
May 13, 2013
Period 4
Whos the One to Blame?
Introduction:
A titration is a lab technique used to determine the exact concentration of an
unknown acid or base. Often times, acids and bases are identified based on their physical
properties. An acid is a typically sour substance that gives away their hydrogen ions
when dissolved in water with a base and turns litmus paper red. The characteristics of a
base are the opposite of an acid. They absorb hydrogen ions and turn litmus paper blue
The purpose of this lab is to identify who killed Mr. M by analyzing and matching the
Molarity of the Crime Scene HCl acid sample to the Molarity of the suspects found in the
investigation. In this lab, the acid samples will behave as the solvents of the solution or
the substance that takes up most of the volume and the bases will behave as solutes or
substances that take up less volume when both are blended. The result of this mixture
should be a neutralization reaction, a reaction in which an acid and a base in an aqueous
solution react to produce neutral water and salt. In addition, after the experiment, it will
be necessary to identify the Molarity of HCl by using the formula (moles/ liters) in order
to compare the different Molarity to find the killer.
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Procedures:
1. Before starting, the students wore their goggles on and obtained the following
materials:
A 50 ml graduated cylinder
A 50 ml burette, stand, and cylinder
A 125ml Erlenmeyer flask Phenolphthalein indicator
Glass funnel
2. The stopcock was turned towards the bottom and remained perpendicular to
the tube of the burette in a closed position.3. The burette was filled with 1.0 M NaOH base. Then the initial volume was
recorded.
4. The graduated cylinder was utilized to measure 20ml exactly for each acid
sample.5. 3 drops of phenolphthalein indicator were added to the acid samples ( the acid
remained clear).6. The stopcock was opened until there was a slow stream of NaOH in order to
titrate the unknown acid.
7. When the drops fell, the flask was swirled and the coloring disappeared.
Observations were recorded in the results section.8. When a solution was approaching neutralization, it became piker more rapidly
and will later clear itself.
9. Then, the stopcock was gently, partially opened and little drops were pouredinto the acid sample.
10. When the coloring did not disappeared, the stopcock was quickly closed. If
the solution had a very faint pink color, then it was a good titration. Though, if
the titration was dark pink, it was necessary to redo the proceadures over intrial 2.
11. The Final Volume of NaOH in the burette was recorded.
12. The Total Volume (in mL) of NaOH was calculated. It neutralized thesuspects sample and the data was recorded.
13. The burette was refilled with NaOH and the procedures were repeated with
the other 3 samples.
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Data:
(Table 1): Data for in search of the Final Volume of NaOH
Exact
Volume of
HCl (mL)
Initial
Volume of
NaOH(mL)
Final
Volume of
NaOH(mL)
Total
Volume of
NaOHUsed in
titration(mL)
Molarity
of HCl
(M)
Observatio
/ Notes
Suspect A
Kirkpatrick
HCl Acid
Trial
1
20mL 10mL 20mL 10mL .5M. -dark pink
Trial
2
20mL 20.5mL 30mL 9.5mL -light pink
Suspect B
Larkin
HCl
Acid
Trial
1
20mL 3mL 8.5mL 5.5mL -dark pink
Trial
2
20mL 8.5mL 13mL 4.5mL .225M -light pink
Suspect C
Nguyen
HCl Acid
Trial
1
20mL 13mL 27mL 14mL .7M -light pink
Trial
2
20mL 27mL 43mL 14mL -light pink
Crime Scene
HCl Acid
Trial
1
20mL 1mL 5.5mL 4.5mL -dark pink
Trial
2
20mL 5.5mL 9.5mL 4mL .2M -light pink
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Calculation Table 2:
Acid Sample 1. Moles of NaOH 2. Moles of HCl 3. Molarity of HCl
(moles HCl/Liters HCl
used)
Suspect AMrs.Kirkpatrick
.01 mol 0.1 mol HCl0.5 mol HCl
Suspect B
Mr. Larkin
.0045 mol .0045 mol HCl
0.23 mol HCl
Suspect C
Ms.Nguyen
.014 mol .014 mol HCl 0.7 mol HCl
Crime Scene
Sample
.004 mol .004 mol HCl 0.2 mol HCl
Conclusion:
At the end of the titration lab, it was concluded that Mr. Larkin is responsible for
Mr. Mehkatarians death. The acid samples, the solvents of the solution, were mixed with
drops of phenolphthalein and NaOH, both solutes, created a homogenous reaction. For
example, the acid sample for Mrs. Kirkpatrick was mixed with both the phenolphthalein
indicator and with NaOH, and turned the acid sample into a dark pink for the first trial
and a light pink for the second trial. This indicates when the solution is light pink, it is a
weak, less concentrates acid. However, if the acid was dark pink after the solvents were
poured into it, then acid was strong thus more concentrated. After the experiment, the
Moles HCl were found. But first, the equation was balanced forNaOH + HCL and
obtained NaCl + H2O. The balanced equation demonstrates that an acid donates its
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Hydrogen ions to the base when both are dissolved in water. When the moles of HCl
were found and its Molarity, the Molarity of each acid sample, including the crime scene
were compared in order determine the rue killer. In the end, the concentration of the acid
sample of Mr. Larkin was similar to the sample found in the crime scene, indicating that
Mr. Larkin was found guilty.
Although the results and data were obtained, there were sources of error present
as well. One source of error that affected the data was the testing materials such as the
Erlenmeyer flask. The materials were not fully cleaned and perhaps the actual amount of
NaOH needed when added to the HCl is inaccurate. As a result, multiple trials were
performed for each acid sample, making trial 1 for each acid sample unreliable. Another
source of error was the stand because it was loose. When NaOH was poured into the acid
sample, the students had to read the scale of the 50mL burette; however, the burette was
difficult to read because it was slanted. As a result, the column for the Final Volume of
NaOH is unreliable. If the materials were fully rinsed before the experiment and if the
stand was not slanting, the data could have been more accurate.
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