MORGAN Spectroscopic Analysis Of A Dye Chemistry Lab Report Help EXPERIMENT: Spectroscopic Analysis of a Dye PLEASE PLEASE PLEASE REWORD EVERYTHING IN YELL

MORGAN Spectroscopic Analysis Of A Dye Chemistry Lab Report Help EXPERIMENT: Spectroscopic Analysis of a Dye PLEASE PLEASE PLEASE REWORD EVERYTHING IN YELLOW SO ITS NOT PLAGIARIZED. Please write the discussion and conclusion.Please write an A+ paper. EXPERIMENT #7: Spectroscopic Analysis of a Dye
General Chemistry Laboratory, Spencer Hall 207
Morgan State University, Baltimore, MD
April 31, 2019. 8:00 a.m. – 10:50 a.m
Title: Spectroscopic Analysis of a Dye
Abstract:MAIN GOAL/PURPOSE, HYPOTHESIS, KEY QUESTION, RESULTS,
CONCLUSION.
This lab dealt with the absorbance a of a new cyanine dye developed and used in things
such as labeling proteins and nucleic acids in biomedical imaging that has a lot of
applications in drug development.The purpose of this experiment is to understand how
light interacts with a dye solution and to use this knowledge to determine the amount of
dye in an unknown. This experiment is based on assumptions that there is a correlation
between absorbance and the concentration of dye in the solution. The hypothesis is that
as the concentration the dye increases the absorbance the dye also increases. For the
experiment, a stock solution using a given mass of the cyanine was made, along with 5
different standard solutions using the made stock solution the controls involved in the
experiment are spectrophotometer used, the stock solution used, and the concentration
of the dye used. The experiment could not be completed due to errors occurring when
trying to measure the absorbance of the standard solutions.
Introduction:DISCUSS THE MAIN GOAL AND PURPOSE , KEY CONCEPTS OR
THEORIES
The objective of this laboratory exercise is to become familiar with a typical
spectrophotometric analysis and to examine the effect of an interfering substance. This lab
was the calculation of the concentration of the dye solution; and using the prepared series of
standard solutions, made from a stock solution, to measure absorbance with a
spectrophotometer. The spectrophotometer is a vital machine for researchers, scientists, and
biological and chemical engineers in studying various substances. Understanding the function
and output results of spectrophotometry can be essential for future studies involving light
absorbance of a wavelength and the concentration of a sample. This lab discusses the
important relationship between material concentration and the intensity of light over a
function of wavelength. A spectrophotometer is defined as an instrument used to measure the
intensity of wavelengths in a spectrum of light, and commonly used for the measurement of
transmittance or reflectance of solutions, transparent or opaque solids, such as polished glass,
or gasesThe key concepts in this experiment are Absorbance, beer’s law, absorptivity, path
length and Calibration curves. Absorbance is a measure of the capacity of a substance to
absorb light of a specified wavelength. It is equal to the logarithm of the reciprocal of the
transmittance. Absorptivity is a measurement of how strongly a chemical species absorbs
light at a given wavelength. Path length is considered to be the overall length of the path
followed by a light ray or sound wave. Calibration Curve is a method for determining the
concentration of a substance in an unknown sample by comparing the unknown to a set of
standard samples of known concentration. Beer Law is a physical law that states the quantity
of light absorbed by a substance dissolved in a non absorbent solvent is directly proportional
to the concentration of the substance and the path length of the light through the solution and
Absorptivity which is a measurement of how strongly a chemical species absorbs light at a
given wavelength.. The key question/purpose of this experiment is determined whether the
absorbance of the dye in influenced by the concentration of the dye in the solution. It is
important to know that transmittance because it is presented as a percentage and absorbance
is unitless. And it is important to use the Beer-Lambert law because it is represented as an
equation that shows the relationship between the absorbance and transmittance.
The equation represents the molar absorptivity, the concentration of the compound inside the
solution, and the length of the light that is passed through the sample. These equations are
used to calculate the data in this experiment to get the final results.
Experimental Details
Objective
-To establish how to relate the abstract of a solution containing the dye concentration in the
solution.
-To determine the concentration of the dye in an unknown solution using the concentration.
Materials
-250mL beaker
-25mL cleaning solution
-50mL beaker (For cleaning solution)
-Spectrophotometer
-Distilled water
-Sample stock solution
-Test tube
-solvent-ethanol
Procedures:
-Fill a 50mL beaker with 25mL cleaning solution
-Clean all Apparatus/materials using solution, distilled water and cleaning brush.
-Dry all materials with paper towels.
Experiment :
During this experiment David and I understood the three main procedures that were needed
to calculate all data. First, David and I expected to perform all calculations which helped
determine the absorbance of the solvent ethanol solution. David and I then used the
spectronic spectrophotometer to help determine the concentration of the unknown substance
by using all recorded information. Before David and I begin the lab experiment we begin
calculating the given data to find the number of moles and molarity of for concentration.
After, David and I allowed the instrument to warm up for 10 minutes while setting the percent
transmittance (%T) to zero. Next, we gathered 100 mL of the ethanol. After gathering the
solution we then filled the dye (5.4g of dye with the ethanol solution transfering into a
volumetric flask repeating until all the dye had dissolved. David and I then filled each clean
with no air bubbles or fingerprints test tube with ethanol solution and inputted into
spectroscopic till the data reach 100. Following the steps David and I then calculated the VI
value for number 1-5. After David and I tested each test tube in three trials. David and I then
added the NOT NULL to a clean test tube and tested in three trials recording (0.696, 0.694
AND 0.692).
Results and Calculations:
For David and I record, we put all the absorbance reading in a chart below. Our information
we calculated into excel. This chart David and I considered to be important as it displays the
final results of our experiment. Other data David and I recorded was the final results were
we calculated the dilution of each solution for the number of moles and molarity.
H COUNT
40
(1.008 X 40) = 40.32
C COUNT
34
(12.011 X 34) =408.34
I COUNT
1
(126.904 X 1)= 126.904
CI COUNT
1
(33.5 X 1) =35.5
N COUNT
2
(14.01 X 2) =28
=
639.06 g/mol
Concentration
Absorbance
2.96
0.915
0.885
0.855
5.92
1.270
1.270
1.270
8.87
1.470
1.460
1.440
11.85
1.400
1.400
1.420
14.79
1.600
1.560
1.580
NOT NULL
TRIAL #1
0.696
X= Concentration
Y= Absorbance
TRIAL #2
1.694
TRIAL #2
0.692
1.[11.85 +1.407]
2. [1.580 +14.29]
Formula: Y=MX + B
Y2-Y1
X2-X1
1.580 – 1.407
14.79 – 11.85
=
0.173
2.94
M=0.054 (Slope)
1.580 = 1.159 (14.79) + B
0.059 X 14.79
=0.87
=1.580 / 0.8 =1.816 = B
UNKNOWN: c =a/eb
c=?
a= 0.694 (Absorbance)
eb= 0.059 (Slope)
?=0.694
0.059
= 11.76 = Unknown concentration
1 graph line graph
Discussion: DISCUSS RESULTS OBTAINED
Conclusion: DISCUSS THE MAIN GOAL/PURPOSE , MAJOR RESULTS
OBTAINED
.
References:
General Chemistry Laboratory Manual, An integrated Critical Thinking Approach, By Angela J
Winstead, Morgan State University, McGraw Hill 2013.

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