Contents
1.0 Introduction 3
1.1 Objective 3
1.2 Background 3
1.3 Technique Analysis 4
2.0 Experimental Procedure 6
3.0 Results 8
3.1 Table of Concentration of Vanillin with Absorbance 8
3.2 Calculation 9
4.0 Discussion 10
5.0 Conclusion 11
6.0 Reference 12
1.0 Introduction
1.1 Objective
The objective of this experiment is to analyze the concentration of active ingredient vanillin in artificial vanilla essence by UV-Visible spectrometry.
1.2 Background
Vanilla is one of the most common flavors that are used in food addictive such as ice cream, and milk. There are two types of vanilla which are pure vanilla and imitation vanilla. Pure vanilla is made up from the vanilla bean while the imitation vanilla is made up from the clove oil that extracts from the bean then combined with ethanol and sugar or glycerin (Correspondent, 2003). Inside of the vanilla, there is a molecule name vanillin or known as 4-hydroxy-3-methoxybenzaldehyde. The chemical bonding structure of vanillin is shown in figure 1 below. Vanillin in vanilla is mainly to give the flavor and smell of vanilla.
Today, the consumption of pure vanilla is lower than imitation vanilla as the production of it is time-consuming and labour intensive. Therefore the vanilla extract cost is higher than imitation vanilla (Correspondent, 2003).
Figure 1: Vanillin (Wikimedia Common, 2014)
1.3 Technique Analysis
Determination of concentration of vanilla in this experiment involves three main steps, which are extraction of the vanillin from the other components of the essence using an organic solvent, back extraction of the vanillin as its sodium salt into aqueous phase using dilute sodium hydroxide and determination of the concentration of vanil...
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...ferent in accuracy of the data.
6.0 Reference
Correspondent, D. Y. (2003). Daytona Beach News - Journal, The. Know beans about vanilla, imitation: [WEST VOLUSIA Edition].
Elder, K. (n.d.). How accurate are your experiments? Retrieved from Kennewick High School Science: http://kehsscience.org/How%20accurate%20are%20your%20experiments.pdf
Oliva-Chatelain, B. L., & Barron, A. R. (2010). Basics of UV-Visible Spectroscopy. Retrieved from openstax cnx: http://cnx.org/content/m34525/latest/
Schneider, R. F. (2013). Retrieved from Beers Law: http://www.ic.sunysb.edu/Class/che133/lectures/beerslaw.html
W. H. Bunnelle, L. A. (n.d.). Extraction. Retrieved from Univesity of Missouri: http://www.chem.missouri.edu/chem2050/expt_2.pdf
Wikimedia Common. (2014). File:Vanillin.png. Retrieved from Wikimedia Common: http://commons.wikimedia.org/wiki/File:Vanillin.png
Absorbance was defined as: log I_o/I where I_o is incident light and I is the transmitted light. Fluorescence emission spectrum is different from fluorescence excitation spectrum because it records different wavelengths of chemical s...
The purpose of this experiment was to learn and preform an acid-base extraction technique to separate organic compounds successfully and obtaining amounts of each component in the mixture. In this experiment, the separation will be done by separatory funnel preforming on two liquids that are immiscible from two layers when added together. The individual components of Phensuprin (Acetylsalicylic acid, Acetanilide, and Sucrose as a filler) was separated based upon their solubility and reactivity, and the amount of each component in the mixture was obtained. Also, the purity of each component will be determined by the melting point of the component.
The objective of this experiment was to perform extraction. This is a separation and purification technique, based on different solubility of compounds in immiscible solvent mixtures. Extraction is conducted by shaking the solution with the solvent, until two layers are formed. One layer can then be separated from the other. If the separation does not happen in one try, multiple attempts may be needed.
The results of this experiment are shown in the compiled student data in Table 1 below.
Starting this experiment, we knew that the extraction was going to form varies layers due to the density differences. When placing three different substances, we saw that two layers formed because the Clove Oil is soluble in MTBE, but not in water. In order, to get the organic layer we used separatory funnel to take out the excess substances and leave the oil layer. Then we transferred to a beaker and dried with Magnesium Sulfate. Lastly, we filtered the liquid using funnel; we placed the liquid to boil, let it cool to room temperature. The purpose of drying and evaporation is to help us with the Gas Chromatography analysis of the product.
In conclusion the experiment was carried out and had great success proving my prediction to be correct and enabling solid and valid results which were able to be put in a graph. I believe my prediction could have been more accurate or more backed up if I had made a quantitative prediction. Though what I believed would happen did happen during the experiment which helped to understand the graph and the results which led me to be able to write a thorough report on them.
Possible sources of error in this experiment include the inaccuracy of measurements, as correct measurements are vital for the experiment.
Discussion: The percent of errors is 59.62%. Several errors could have happened during the experiment. Weak techniques may occur.
In this experiment, lipids from ground nutmeg are extracted using a combination of solvents and identify the lipids through chromatography. The purpose of using solvent combinations is to elute the lipids based on their polarity to binding of the silica gel. The chromatography is performed on a silica gel plate and the use of iodine to visualize the lipids. By calculating the Rf values for each compound and comparing them to the known lipids, we are able to distinguish the lipids within the grounded nutmeg.
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Eugenol was extracted from cloves through the process called steam distillation. A total of 50ml of distillate were collected with temperature monitoring for every 5.0ml of collected liquid. The distillation curve showed that the temperature of volatilization of eugenol is from 98°C to 99°C which is way below its boiling point at 2540C. Chemically active extraction was conducted in order to remove impurities particularly eugenol acetate and caryophyllene. This involves the addition of several solvents particularly hexane, NaOH, HCl, then hexane again in succession.
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