1. The final yield of the cells can be determined by use of an automated cell counter or by use of a hemocytometer (Neubauer chamber). In our laboratory‚ we determine the number of purified cells in a Neubauer-improved‚ bright line chamber with V-slash with a depth of 0.1 mm and a counting area of 0.0025 mm2 from Marienfeld (Lauda Königshofen‚ Germany‚ PN # 0650030). 2. For determination of the final cell yield‚ mix a 10 µl aliquot of the purified cells (Figure 9D) with 10 µl of trypan blue solution
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Experiment 3: Separating and Determining the Mass of Calcium Ion in a Calcium-Enriched Tablet In this lab‚ we dissolved a calcium-enriched tablet and participate the calcium ion as calcium carbonate. Our purpose is to determine the masses of calcium carbonate and calcium ion‚ to determine the mass percent of calcium ion in the tablet and to compare the masses and the percent with the listed tablet ingredients. This time we used a 150mL beaker‚ analytical balance‚ forceps‚ a 50mL graduated cylinder
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I. Objective: The objective of this experiment is to determine the mass percent of iron in an iron compound using a spectrophotometer. From there‚ determine which iron compounds are in the stock room bottles based off of the experimental mass percent results. II. Introduction: The objective is to determine the mass percent of iron in an iron compound using a spectrophotometer. From there‚ determine which iron compounds are in the stock room bottles based off of the experimental mass percent results
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Figure 1: Titration curve of 0.160 grams of an unknown diprotic acid that was dissociated in distilled water. Shown is the pH versus the volume in milliliters of 0.1 M NaOH‚ a strong base‚ added to the solution. The initial pH reading of the solution was a pH of 2.60. Although the pH of the ½ equivalence point was unknown‚ it could be estimated by halving the volume of NaOH used at the first equivalence point. At the first equivalence point‚ 13.63 milliliters of NaOH had been added to the unknown
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Computer Lab Rules & Regulations Electronic workstations may only be used by current Swinburne University students and staffs. Swinburne identity card must be presented on request. Swinburne computing facilities should only be used for educational‚ research and administrative purposes of Swinburne. All other uses are strictly prohibited. The following rules and terms apply to all computers on campus. Terms and Conditions 1. All users must abide by the license requirements of any software
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First‚ prepare a data table. Record what you see throughout the laboratory activity. Your teacher will demonstrate for the class the reaction of metallic copper with concentrated nitric acid‚ HNO3. This must be done in the fume hood. (Caution: Avoid breathing poisonous gases. Avoid contact of skin with nitric acid. It burns skin and clothing.) One student will be asked to feel the side of the demonstration beaker and report to the group. The products formed are copper(II) nitrate solution‚ Cu(NO3)2(aq)
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MODULE 2 WORKSHEET 6 CALCULATIONS INVOLVING GASES Syllabus reference 9.3.2 1 Two identical gas flasks‚ A and B‚ are kept at the same temperature and pressure. Flask A contains 10 g of ethane gas‚ C2H6. Flask B contains sulfur dioxide gas‚ SO2. Calculate the mass of sulfur dioxide gas in flask B. moles ethane 10/30 0.33 mol moles SO2 0.33 mol mass SO2 0.33 64 21 g 2 What mass of nitric oxide‚ NO‚ is present in a 2.5 L flask at a pressure of 100 kPa and 0ºC? mole NO 2.5/22.71
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Class average for a 80 and 120 drop count was recorded to be 0.041+/- 0.005 mL/drop. If a graduated cylinder is not available there is another way of adding more of the solution. The disposable pipet can transfer 0.5mL of the solution to the chemical reaction. When comparing a 10mL graduated cylinder‚ a 100mL beaker‚ and a 50mL graduated cylinder‚ the most precision peace of glass wear would be the 10 mL graduated cylinder with the true volume of water (calculated)‚ class average‚ and uncertainties
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1 Weigh the beaker. 2 Add 50 milliliters of the solution you want to test to the beaker and record its mass. The mass of the solution is equal to the total mass minus the mass of the beaker. 3 Divide the mass of the solution by its volume -- in this case‚ 50 milliliters -- to find its density. 4 Empty‚ rinse and dry the beaker. Add 4.3 grams of sugar to the empty beaker‚ then add water until the contents reach 50 milliliters in volume. Stir until the sugar dissolves‚ then measure the
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Name of the Student:………………… Date:………….. What is the volume of 1 mole of hydrogen gas? One mole of any gas occupies the same volume when measured under the same conditions of temperature and pressure. In this experiment you will calculate the volume of 1 mole of hydrogen at room temperature and pressure. Intended lesson outcomes By the end of this practical you should be able to: • further develop skills in manipulating apparatus and accurate measurement; • use the mole concept; • calculate
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