Laboratory Exercise #2 Pre Lab This lab will teach me how to use a spectrophotometer. The use of the spectrophotometer is to measure the concentration of solute. The solute being measured must be colored and is determined based on the adsorption of light photons on a wavelength. The spectrophotometer uses a beam of light that strikes the diffraction grating that basically forms of prism of light. Then only a specific wavelength of light shines through the spectrophotometer and interacts with
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Lab 6 Prelab Spectrophotometry This is due at the beginning of lab 6. Read the lab protocol for this week and type your individual answers to the following questions. Each student should turn in answers at the beginning of class. You may consult other resources (textbook‚ library‚ etc.) Remember to cite information and put responses in your own words to avoid plagiarism (and loss of credit on the assignment). 1. Refer to step 2 in the protocol for lab 6. Calculate the concentration of the sample
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Paragraph I In the study conducted by Haines‚ Cambon & Hull (2003)‚ they examined the impact of temperature change from 294 to 1073K on the structural development of FePO4. Initially‚ at low temperature‚ FePO4’s structure is of tetrahedral. This α-quartz structure is illustrated in the following diagram. However‚ as temperature increases‚ the tilting of the tetrahedral angles began to drop. This continues as it approaches 980K to the β-phase‚ where it gradually forms an octahedral structure. In
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Discussion Questions 1. 2. What is a spectroscope and what is it used for? A spectroscope is a scientific instrument that is used to measure the intensity of the light at different wavelengths by calculating the amount of light energy that is being absorbed by the electrons at different wavelengths. 3. 4. 6. How might the difference in the brightness of spectral lines be explained? In other words‚ why are some lines in a spectra easier to see and appear brighter? Some lines in a spectra are easier
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Main aim of experiment 5 is to use the biuret test to quantify the concentration of the Bovine Serum Albumin (BSA) then constructing a standard curve graph and to use the spectrophotometer to perform an enzyme assay using different concentration of the BSA. Experiment 5 also verifies the Beer-Lambert Law‚ which is the linear relationship between absorbance and concentration of an absorbing species. Absorbance formula is shown in fig. 1.1. However‚ the Beer-Lambert Law is not obeyed at high concentration
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Discussion of Results and Scientific Explanation: In order to observe how much a chemical substance absorbs light a spectrophotometer can be used. A spectrophotometer measures the amount of light absorbed by measuring the difference in the intensity of the light before and after a beam of light passes through a sample solution. The area in which light is absorbed can provide information about the molecule‚ such as the concentration‚ by identifying the most preferentially absorbed wavelength.1
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Background Information: Spectrophotometry is a method that measures how much light is absorbed by using the electromagnetic spectrum. By seeing which colors are absorbed and which are reflected scientists can determine what a substance is without having to touch them. This is possible because each substance has a specific absorbance spectrum‚ meaning that the absorption spectrum of two different substances cannot be the same. Purpose/Hypothesis: 1. The purpose of the experiment was to determine
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To construct a calibration curve‚ three samples with different known concentrations and a blank solution are prepared and their absorbances are measured with a UV-Vis spectrophotometer (Table 1). The absorbances of three unknown samples with same concentration and a blank are measured (Table 2). The blank solutions are used as a reference solution to calibrate the colorimeter. The volumes of Fe solution for the delivery volume errors in the 10 ml graduated pipet are corrected (Table 3). The molarity
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The 13C NMR spectrum was useful to help finding the structure of the unknown. It showed six different signals in the spectrum. Signal 1 had an observed peak value of 19.242 ppm‚ and its peak calculated value was 19.1 ppm. This signal was first to most upfield and shielded in the spectrum because of the high electron density of carbon. This signal was agreed to a literature value for a CH3 group between 5-30 ppm. Signal 2 was branched to signal 1‚ and had the same value‚ but it was agreed for the
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produced by energy. When a chemical burns‚ the common atomic structures of chemicals excites the electrons and makes them go crazy. This ends up in the emission of visible light and forms into multiple colors. What is spectroscopy and how is it used by physicists and chemists? Spectroscopy is an important tool used in astronomy. It is detailed study of light that comes from an object. Light is energy that moves through space. It can be thought of either waves or particles. The distance between the high
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