Determining the Absorbance Maximum Wavelength and Molar Extinction Coefficient to Find the Molarity of the Unknown DCPIP Background Information: A spectrophotometer is an instrument used to help determine the absorption spectrum of chemicals. It does this by reading the absorbance of the chemical at different wavelengths. All chemicals absorb light in their own distinct way. This distinction helps to identify unknown chemicals. The absorption of light within a chemical is also very important because
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Boiling Point Lab Introduction: The purpose of this lab is to learn about the calibration of a thermometer. In addition‚ we also investigated the boiling point of an unknown liquid to determine its identity. Chemical Responsibility: 1. Make sure to use glycerine (lubricant) and a towel to safely insert the thermometer into the rubber stopper. 2. Carefully operate the Bunsen burner and make sure to use rubber gloves when handling the boiling water of beaker 3. Always wear goggles
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Melting Point Determination and Thermometer Calibration Lab Background: The melting point of a substance‚ a solid in this case‚ signifies the temperature at which the first crystal starts to melt until the temperature at which the last crystal disappears is reached. That being said‚ melting points are expressed in ranges‚ am organic compound will have a sharp range depending on the purity of the compound. Impurity of an organic substance will register an abnormal melting point based on its
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Experiment #1: Mass‚ Volume and Density Performed: 2/2/11 Turned in: 2/9/11 The purpose of this experiment is to verify the independence of X and Y motion for a projection. We watch the professor perform this experiment. The equipment used in this experiment was a projectile launcher (ME-6800)‚ a drop shoot accessory (ME-9859)‚ one photogate (ME-9204A)‚ white paper‚ carbon paper‚ two time-of-flight timing pad (ME-6810)‚ two balls (ball 1 and ball 2)‚ and an interface computer. Ball 1 is dropped
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Collecting Butane Gas The purpose of the lab was to determine the molecular mass of Butane‚ and this was done by using the ideal gas law (PV=nRT). The materials used were: match‚ funnel‚ bucket‚ cylinder‚ thermometer‚ lighter‚ scale‚ and a wooden flynt. These materials are used to help collect and test the Butane gas. Butane gas was used because it is ideal at standard temperature and pressure. Procedure: 1. Rinse bucket and fill three fourths full. 2. Rinse all glassware. 3. Place
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Buffer Post Lab Calculation 1. We added too much NaOH to our buffer 1 solution. The original pH was 5.32‚ with 10mL of buffer and 10mL of DI water. We added 5mL of NaOH and the pH changed to 12.12. If 5 mL changed the pH by about 7‚ then we predict that about 2 mL of NaOH would change the pH by about 2. This prediction is based on the fact that 2.5mL is half of 5mL‚ and 3.5 is half of 7‚ so adding a little less than 2.5mL would give us a difference of about 2. For the buffer 2 solution‚ the original
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Name Date: Graded Assignment Meeting Needs Head On Answer the questions. When you are finished‚ submit this test to your teacher by the due date for full credit. (50 points) 1. After you have completed your research and examined first-hand accounts of people who lived through the Great Depression‚ write a detailed summary of your findings‚ highlighting at least three examples. Include information on these topics: The impact that the Great Depression had on the people you studied. For example: What
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I. Abstract: By manipulating the ideal gas law (PV=nRT)‚ we will be determining the molar mass of an unknown volatile liquid. Heating a flask filled with an unknown‚ easily evaporated liquid will allow for measurements that can be taken to work out the ideal gas equation. This lab will require knowledge of basic equations used in chemistry. Using these equations‚ such as density and number of moles(n)‚ we can substitute different values into the ideal gas law to manipulate it.
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Haylee McHale February 3‚ 2013 Organic Chemistry Lab 226 Section 6 Techniques Lab 1. % Recovery= grams recovered compoundgrams crude compound X 100 % Recovery= 0.040 grams0.256 grams X 100 % Recovery= 0.16 x 100=16% There are many reasons why the percent recovery is much less than 100%. For example‚ one source of error may have been that the separatory funnel containing the acidified phenylalanine and ethyl acetate may not have separated well enough after being shaken together in the
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Molar Volume of a Gas Objective: The objective is to determine the volume‚ of one mole of hydrogen gas at STP using experimental data‚ known mathematical relationships‚ and a balanced chemical equation. Theory: The goal of this lab is to find the volume of one mole of hydrogen at STP. The experimenters will be working with hydrochloric acid and magnesium to find the objective. The acid in this lab will react to the magnesium and cause the water in the eudiometer to rise because of the reaction
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