Making aspirin Pass Introduction: In this assignment I will describe making aspirin by using Method 2. Risk assessment: |Hazardous chemical or | | | |microorganism being used or made‚ | | | |or hazardous procedure or |Nature of the hazard(s) |Control measure
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Small samples of acetaminophen‚ acetylsalicylic acid‚ cellulose‚ starch‚ and caffeine were obtained. These samples were then placed into seperate sets of test tubes that contained water‚ acetone‚ or dichloroethane. Solubilities were then tested for each sample in each solution which can be seen in Table 5. Next‚ four random pills were obtained and weights were taken of each. Each of the pills were grinded up using a separate mortar and pestle. The grinded up pills were then weighed. The grinded
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hours. Apparatus/Materials: Three Conical Flasks‚ Three Filter Funnels‚ Cotton Balls‚ Measuring Cylinder‚ Loam Soil‚ 225ml of Water‚ Paper‚ Pencil Methods/Procedures: Obtain and clean out three conical flasks. Label each flask Sand‚ Loam and Clay. Plug three funnels with cotton balls and place one in each flask. Place 20g of each soil in respected filter funnels. Measure and pour 75ml of water into each flask. Record he time for the first drop
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1. | | | What is the pressure‚ in atm‚ of a tank of gas with a regulator that reads 1250mmHg? | | | Student Response | Correct Answer | A. | 1.64 | | B. | 490 | | C. | 1.79 | | D. | 0.608 | | E. | 1.25 | | | Score: | 0/1 | | | 2. | | | A 147.9-L sample of dry air is cooled from 88.0°C to 22.1°C while the pressure is maintained at 2.85 atm. What is the final volume in L? (Do not type the units.) | | | Student Response | Correct
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68.04g * Mass of Na2CO3 = 10.6g 1. 10.6g of Na2CO3 was weighed in a dry beaker. Small amount of distilled water was added and the salt was dissolved. 2. The contents of the beaker were transferred to clean volumetric flask of 100ml. 3. Collection of washings was done 3-4 times. 4. The solution was made 100ml. Shook well to ensure the uniformity of the solution. 5. The contents were transferred to the storing bottle and it was labeled 1M Na2CO3 solution.
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of Na2CO3 = (23 x 2) + ( 16 x 3) = 106 g mol-1 250cm3 x 0.1moldm-3 x 106 gmol-1 = 2.650g 1000cm3 I will use 2.650g of Na2CO3 in 250cm3 of distilled water. Apparatus · Weighing bottle · Clamp stand · Glass rod · 250cm3 volumetric flask · Small conical flask · 50cm3 burette · 100cm3 beaker · 25cm3 pipette · Pipette filler · Plastic pipette · Small filter funnel · Balance · Distilled water · Sulphuric acid · 2.650g of sodium carbonate · Spatula · White tile · Methyl orange indicator
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performed as follows: For run 1‚ 20cm3 of acetone‚ 10cm3 of sulphuric acid and 145cm3 of water was added to a conical flask. 25cm3 of iodine was then added to this solution which started the reaction and immediately‚ 20cm3 samples of this mixture was added to six flasks. After successive 5 minute intervals‚ sodium acetate was added to each of the conical flasks in order to stop the reaction. Flask 1 and 2 were then titrated‚ (3 to 6 turned colourless) using 0.01M sodium thiosulfate and a starch indicator
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Chemistry Internal Assessment Title: Determination of the percentage (%) of ethanoic acid in vinegar Date Experiment was performed: 1st April 2011 Criteria Assessed: DCP‚ CE Apparatus: 2 conical flasks 1 250cm3 volumetric flask ±0.30cm3 Electronic Balance ±0.10g 50cm3 Burette±0.1cm3 25cm3 Pipette±0.06cm3 Materials: 0.20M HCl (±0.02moldm-3) 1.1g solid NaOH (±0.1g) A solution of vinegar of unknown concentration (density= 1.05gcm-3) Phenolphthalein Method: * A solution of NaOH was
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In this experiment the initial mass of the sodium carbonate used was 2.69g. In each titration‚ 3 drops of methyl orange was added to the sodium carbonate solution. With this information the titration can begin‚ and the results obtained are shown below: Titration readings Titration Rough 1 2 3 4 5 Initial 0.00 4.30 22.00 21.00 15.00 25.90 Final 4.30 22.00 38.60 37.60 32.60 42.20 Titre (cm3) 4.30 17.70 16.60 16.60 17.60 16.30 Therefore‚ the average titre would be calculated as follows;
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The first flask was placed under a buret. Finally we titrated the KHP by adding the base until the end point was reached‚ which was when it turned pink completely. We repeated this twice and then cleaned up. The procedure does not include very difficult math‚ however the calculations did. The harder math calculations included finding moles of the acid‚ moles of the base that was used to neutralize‚ and the molarity of the base. After all calculations‚ below is what we concluded. The molarity you
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