V. PRODUCTION ASPECT A. Raw Materials 1. Herbs Number of Units | Raw Materials | Price/Kilo | Total Price | 5 KilosI KiloI KiloI KiloI KiloI KiloI Kilo | Kasitas (Acapulco) NeemPaliahanKalilongMakabuhayMalunggayGuava | Php 25.00 20.00 20.00 20.00 20.00 25.00 20.00 | Php 125.00 20.00 20.00 20.00 20.00 25.00 20.00 | TOTAL
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along with the caffeine. The column now only contains the desired compound caffeine and to extract caffeine from the column‚ a smaller one-armed Erlenmeyer flask that is clean will used to hold this extraction and 5 mL of ethyl acetate will be passed through SPE column‚ to obtain and remove the caffeine from the SPE column. A small one-armed Erlenmeyer flask containing 5 mL of ethyl acetate along with the compound caffeine‚ should be the result after using the SPE column
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solution was added to 100 ml sulfuric acid and placed in an Erlenmeyer flask for titration. The solution was then heated to around 60 degrees Celsius. The solution was then titrated until a faint pink/purple color remains for about thirty seconds. The Molarity of the KMnO4 can then be determined. This step was repeated. About 0.3 g of cobalt oxalate hydrate was then weighed (to the nearest 0.1 mg) and placed in an Erlenmeyer flask with 100 ml of 0.5 M sulfuric acid. This solution was then
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Experiment #4A- A Separation and purification Scheme Amena Alkeswani‚ PHCC Dhanlal Murally‚ PHCC September 27‚ 2012 Abstract: There are millions of different organic compounds. Most of them are found in mixtures and in order to achieve a pure form they need to be separated‚ isolated‚ and purified. However‚ there are endless numbers of possible mixtures‚ which make it impossible to have a pre-designed procedure for every mixture. So chemists often have to make their own procedures. The purpose
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layers are now separated. The student was able to observe that the organic layer was less dense than water‚ thus‚ making it sit at the bottom of the seperatory funnel. The student drained the organic layer into a flask and the aqueous layer was also drained into a labeled Erlenmeyer flask. Similar too this procedure‚ to compare the efficiency of multiple extractions‚ the only difference in the procedure was that To compare the efficiency of multiple extractions‚ the same procedure was carried
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and placed in a pre-weighed 25 mL round bottom flask‚ along with 2.5 mL of glacial acetic acid and a magnetic stir bar. Then the reaction apparatus was assembled‚ the dry tube was charged with conc. sodium bi sulfate‚ the 25 mL round bottom was attached to the apparatus‚ and 5 mL of Br2/HBr mixture was obtained and placed in the round bottom. The reaction took place for 20 minutes. An orange liquid was obtained and placed in a 125 mL Erlenmeyer flask along with 25 mL of water and 2.5 mL of conc
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with a second 300 mL sample of deionized water. Clean a 500 mL Florence flask‚ rinse it twice with 10 to 20 mL of your boiled water‚ and fit it with a good rubber stopper. Take the flask to your instructor‚ who will give you about 2.5 mL of 50% NaOH(aq). Fill the flask about two-thirds full with boiled water and mix well‚ with swirling. Then fill with boiled water to just below the neck and mix again. Label the flask. It now contains about 500 mL of approximately 0.1 M NaOH. Check out
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then reweigh. Repeat until there is a constant temperature. Experiment 2 – Percentage of copper in water in sample. Next the percentage of copper in the hydrous copper sulfate needs to be determined. Clean the glassware then get four 50 mL Erlenmeyer flasks with 25 mL of the stock solution and aqueous solvent. Prepare all the unknown sample solutions for determining Beer’s Law Graph. Turn on colorimeter at 100% T then calibrate. Get the data and analyze it if it is correct. Experiment 3 – Percentage
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stirred until the solid dissolved and the solution was then transferred to a 100cm3 standard flask. The beaker was then rinsed with deionised water and the rinsings were added to the standard flask. This procedure was repeated until the solution reached within a centimetre of the graduation mark on the standard flask. Using a dropper‚ the solution was made up to the graduation mark with deionised water. The flask was stoppered and inverted several times to ensure the contents were thoroughly mixed. The
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industries such as dairy farms‚ mining corporations‚ wineries and many more. Equipment list: Equipment why I used it Conical flask To hold the solution and mix the indicator and NAOH Burette To let me pour the HCL into the conical flask at a continuous rate Boss clamp To hold the burette Pipette sucker To pull up the chemicals Beakers To hold the chemicals into so they won’t spill Pipette To accurately measure out the 25
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