Food Dyes: What Wavelengths Do They Absorb?
Food Dyes: What Wavelengths Do They Absorb?
GoalsThe objectives of this experiment are to:
obtain the visible spectra and record the max of the FD&C dyes: blue #1, blue #2, yellow #5, yellow #6, red #3, and red #40.
use max values to identify the food dyes added to a set of fruit drinks
to prepare a set of working dilutions of one food dye
to construct a Beer’s law graph using the set of dilutions prepared.
use data from the Beer’s Law plot to determine the concentration of food dye in an artificially colored drink.
- to analyze the chemical structures of the food dyes and learn what makes them colored.
Background
In the experiment Atomic Spectra, you observed that when a certain gas is heated, it emits light with a few characteristic wavelengths. Just as the energy levels in an element or compound can accommodate the emission of light, a process called absorption can take place as well. Simply put, some substances absorb light.
When a substance absorbs light in the ultraviolet-visible range, electrons in the molecules undergo transitions from lower energy levels to higher energy levels. The difference in energies between the two levels is the amount of energy absorbed, E, and is related to the frequency, , or wavelength, , of the absorbed light as follows:
E = h = hc/
where h is Planck’s constant and c is the speed of light.
Visible radiation, that is the light that we see, is comprised of the spectrum of colored light that we know as the rainbow, ROYGBIV. Different parts of this spectrum are characterized by different wavelengths. A particular substance may absorb some of these wavelengths, while the rest are either reflected or transmitted. If the absorbing substance is opaque, like the blue dye in a sweater, then all the light that is not absorbed is reflected and the reflected color is what we see. If the substance in transparent, like a clear green solution, then the light that is not absorbed is transmitted (it passes through the solution) and we see the transmitted color.
Imagine an aqueous solution of copper(II) sulfate which is blue and perfectly clear. The transmitted color that we see is in the blue part of the spectrum (400-500 nm). Thus the color that is absorbed by copper(II) sulfate is mainly in the red part of the spectrum (>600 nm).
Figure 1. Simplified Schematic of a Typical Spectrometer
The type of instrument that is used to measure how much light is absorbed by a solution is called a spectrometer (more sophisticated versions are sometimes called spectrophotometers.) A spectrometer compares the intensity of the light that enters the solution (Io) to the intensity of the light that is transmitted (I). When some of the light is absorbed as shown in Figure 1, the intensity of the transmitted beam is lower than that of the initial beam (IIo). This relationship is expressed as the transmittance (T) or percent transmittance (%T):
T = I/Io%T = I/Io x 100
While transmittance indicates how much light passes through the solution, the quantity absorbance (A) expresses how much light is actually absorbed:
A = -log T = -log I/Io = -log(%T/100)
A simple spectrometer can be used to measure the absorbance of a certain substance at each and every wavelength in the visible range. The graph of absorbance versus wavelength is called the absorption spectrum of that substance. A typical absorption spectrum has one or more peaks in absorbance. The wavelength at which the absorbance is a maximum is called max, “lambda max.”
The amount of absorbance is directly related to the concentration of the absorbing substance in the solution. A higher concentration means more molecules per volume, resulting in more light absorbed. This relationship is expressed by Beer’s Law:
A = cl
in which c is the molar concentration of the absorbing substance, is the molar extinction coefficient, a characteristic property of a given substance that depends on its nature (how wells it absorbs), and l is the path length in centimeters (the distance that the light travels in the solution). Usually, the diameter of the cuvette containing the solution is one centimeter, so l = 1 cm. Since is a constant for a given substance, then we can say that absorbance is directly proportional to concentration, and a graph of A versus c would have slope that is numerically equivalent to ? .
Since a Beer’s Law plot (A vs. c) expresses the relationship between absorbance and concentration for a given substance, it can be used in analytical chemistry as a calibration curve to determine an unknown concentration of that substance. In this experiment you will plot the visible absorption spectrum for a food dye and determine its max. Other teams will do the same with a different food dye and everyone should share their data. Then you will plot the visible spectrum of one artificially colored fruit drink and compared it to those obtained by the class. You will use the max values to determine which dye(s) were added to the fruit drinks. You will construct a Beer’s Law plot using a set of prepared dilutions of the stock food dyes to help you determine the concentration of food dye added to one of the artificially flavored fruit drinks.
Procedure
1. Start a new page in your lab notebook and include the usual complete heading. Your instructor will assign your team one FD&C dye and one fruit drink, but you will need to record class data to complete this experiment.
2.For this experiment you will actually have to write up your own procedure. Make sure you take all the needed notes so that you can type up a thorough and detailed procedure as part of your lab report.
3.Determine the visible spectrum of one dye using the Vernier Spectrometers. You will need to calibrate the spectrometer with deionized water. Set the spectrometer to give you an absorbance vs. wavelength spectrum. Find the absorbance maxima of the dye (max), the point with highest absorbance (peak) and record in your notebook.
4.Design a table to record all the max values, the “absorbed colors”, and the “transmitted” color of each of the five food dyes. Rotate around the lab and check out the visible spectra obtained by other teams. Roughly sketch each of the five spectra in your notebook. Make sure to make a note of the location of the observed peaks in terms of range of color and wavelengths .Record all the relevant information in your lab notebook.
5.Take a sample of one of the artificially flavored fruit drinks and obtain a visible spectrum, just like you did for the stock food dye solution. Based on the maxvalues of the five food dyes and the maxvalue of your team’s fruit drink, can you determine which dye(s) was(were) added to your fruit drink? Note: you may have more than one dye. Record your conclusion in your notebook and share with the class.
6.You will need to use the stock food dye solution to make a series of working dilutions so you construct a Beer’s Law calibration curve. For example, measure 3, 5, and 7 mL of stock into 10.00 mL volumetric flasks and dilute with deionized water to the mark. Mix well.
7.Prepare a table in your notebook with one column with a list of the final concentration of the dilutions prepared and the concentration of the initial stock food dye solution used. The second column should be used to record the absorbances measured at the same wavelength (max).
8.Choose the maxfor your food dye, measure and record the absorbance for your samples in your table. Always record the absorbance at the same wavelength. You will have to share this data with the class because another team will need your data.
9.Using Excel plot absorbance vs. concentration in grams/Liter. Find the equation of the line, the intercept should be very close to 0.0. The slope of the line is characteristic to the dye.
10.Determine the concentration of the dye in the fruit drink using the line equation, the absorbance measured for the drink sample, and solving for x (concentration in g/L). Remember that the slope is provided by the line equation and the y value is the absorbance obtained from the drink sample.
ApparatusChemicals
Cuvettes (at least two)Artificially colored drinks
10 mL volumetric flasks (at least 3)Deionized water in squirt bottles
Measuring pipets ( 1 to 10 mL )FD&C Blue 1 & 2, Red 3 & 40, Yellow 5 & 6
Pipet bulbs0.010 g/mL Stock Food Dye Solutions
Laptop computer
Vernier Spectrophotometer
Conclusions
Gracefully incorporate the following points into your Conclusions section wherever appropriate (i.e., do not make it look like you are answering a list of questions!)
- What is max for each of the food dyes tested? What color light does each dye absorb and how does this determine its appearance?
- Why is it important to make absorbance measurements at max instead of some other wavelength?
- What is the value of the extinction coefficient for the dye your team tested?
- What is the calculated concentration of the dye present in the fruit drink you tested?
- What is the significance of the R2 value in this experiment? What would be the best possible value for R2 and how does it compare to what you obtained?
- How important was accuracy in preparing the standard solutions? What are the other sources of error in this experiment and specifically how would you expect them to have affected your final result?
- Compare the structures of the 6 food dyes. What do they have in common? Find out what special feature about their structure is responsible for their absorbance in the visible range of the spectrum.
- Lone electron pairs are missing in the handout with the structures, clearly add dots to the proper atoms to indicate the location of the missing lone electron pairs.
- For each of the structures indicate how many pi bonds are present, how many sp2 hybridized carbons are there? Label any sp3 and sp hybridized carbons in the structures provided in the handout. Also indicate the hybridization on the nitrogen atoms.
- Which atom(s) do not follow the octet rule in the structures provided? Explain.
- All of these dyes are obviously soluble in water. What portions of the structures help the overall solubility of these molecules?
Lab Report
The report for this lab will consist of copies of all the notebook pages that are relevant to this lab. Make sure you complete the heading ( Name, partner’s name, date, title, and objective). These pages should also include the detailed procedure, the raw data tables, observations, and sample calculations.
In addition you should include any prepared Excel graphs and a typed Conclusion section that includes the information listed above.
Same blue dye in M&Ms linked to reducing spine injury
- Researchers find way to reduce secondary damage caused by spinal injuries
- Compound BBG is similar to blue food dye used in sweets, sports drinks
- Only side effect of intravenous injection was that it turned test rats blue
- Researchers are planning to apply to the FDA for permission for human tests
-- The same blue food dye found in M&Ms and Gatorade could be used to reduce damage caused by spine injuries, offering a better chance of recovery, according to new research. Researchers at the University of Rochester Medical Center found that when they injected the compound Brilliant Blue G (BBG) into rats suffering spinal cord injuries, the rodents were able to walk again, albeit with a limp. The only side effect was that the treated mice temporarily turned blue. The results of the study, published in the "Proceedings of the National Academy of Sciences," build on research conducted by the same center five years ago.
In August 2004, scientists revealed how Adenosine TriPhosphate, which is known as ATP and described as the "energy currency of life," surges to the spinal cord soon after injury occurs. Researchers found that the sudden influx of ATP killed off healthy cells, making the initial injury far worse. But when they injected oxidized ATP into the injury, it was found to block the effect of ATP, allowing the injured rats to recover and walk again.
"While we achieved great results when oxidized ATP was injected directly into the spinal cord, this method would not be practical for use with spinal cord-injured patients," said lead researcher Maiken Nedergaard, professor of Neurosurgery and director of the Center for Translational Neuromedicine at the University of Rochester Medical Center.
"First, no one wants to put a needle into a spinal cord that has just been severely injured, so we knew we needed to find another way to quickly deliver an agent that would stop ATP from killing healthy motor neurons. Second, the compound we initially used, oxidized ATP, cannot be injected into the bloodstream because of its dangerous side effects."
Back in 2004, Nedergaard's team discovered that the spinal cord was rich in a molecule called P2X7, which is also known as "the death receptor" for its ability to allow ATP to latch onto motor neurons and send the signals which eventually kill them. Nedergaard knew that BBG could thwart the function of P2X7, and its similarity to a blue food dye approved by the Food and Drug Administration (FDA) in 1982 gave her the confidence to test it intravenously. It worked. The rats given BBG immediately after their injury could walk again with a limp. Those that didn't receive a dose never regained their mobility. Nedergaard told CNN that there is currently no standard treatment for patients with spinal injury when they reach the hospital emergency room.
"Right now we only treat 15 percent of the patients we receive with steroids and many hospitals question if that even works for that 15 percent; it's a very moderate benefit to only a subset of patients. So right now 85 percent of patients are untreated," she said. Nedergaard said the research team isn't claiming that BBG can cure spinal injuries, instead that it offers a potential improvement in patients' condition.
"Even a moderate improvement in functional performance of the patient is a big, big event for these patients," she said. "They can control their bladder. If they can just take small steps instead of sitting in a wheelchair all the time, it's a tremendous benefit for these patients," she added. The dose must be administered immediately after the injury, before additional tissue dies as a result of the initial injury. Researchers are currently pulling together an application to be lodged with the FDA to stage the first clinical trials of BBG on human patients.
"Our hope is that this work will lead to a practical, safe agent that can be given to patients shortly after injury, for the purpose of decreasing the secondary damage that we have to otherwise expect," said Steven Goldman, Chair of the University of Rochester Department of Neurology.
Chemical Structures of Food Dyes