need help writing the theory on a oxidation reduction reaction like the re-dox reaction based on Preparation of Cyclohexanone by Hypochlorite Oxidation
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I need help writing the theory on a
Preparation of Cyclohexanone by Hypochlorite Oxidation
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- Procedure: Place 25 mL sample of vinegar, which contains acetic acid, CH3COOH, in a 250 mL Erlenmeyer flask. Then add 3-5 drops of phenolphthalein solution in the vinegar inside the flask. In the base burette, place 0.4600 M NaOH up to the zero mark. Slowly add the NaOH solution from the burette to the vinegar in the flask, with constant but careful swirling of the content of the flask upon each addition of NaOH. Continue the dropwise addition of NaOH from the burette until the color of the solution in the flask changes to a very pale pink, which indicates the end of titration. Make sure that the burette does not touch the flask or its content. Do the same procedure for two more samples of vinegar. LABORATORY REPORT DATA AND RESULTS Volume of vinegar used __________ Concentration of NaOH __________ Brand of vinegar: Maasim Ito! Trial 1 Trial 2 Trial 3 Initial reading, NaOH burette 00.00 mL 00.00 mL 00.00 mL Final…If you have an empty burette in a burette clamp, in what order do you do these steps to fill the burette with liquid (either water for washing, or the titrant)? Drag the steps below into the correct order. Step 1: Close the tap. Step 2: Step 3: Step 4: Step 5: Step 6: Step 7: Return burette to burette clamp. Remove burette from clamp. Hold burette with top below eye level. Put plastic funnel into top of burette. Fill burette with liquid. Remove plastic funnel.Color BEFORE adding Color AFTER adding Intensity of color AFTER adding FeCl3 Test Tube # FeCl3 FeCl3 #1 (salicylic acid) clear lilac 100% #2 (commercial aspirin A) clear slightly pink 50% #3 (commercial aspirin B) clear lilac 95% #4 (aspirin from your clear pink 20% synthesis above) #5 (control) clear clear 0% Based on this data and the melting point of Aspirin, how pure is the synthesized product?
- If you have an empty burette in a burette clamp, in what order do you do these steps to fill the burette with liquid (either water for washing, or the titrant)? Drag the steps below into the correct brder. Step 1: Step 2: Step 3: Step 4: Step 5: Step 6: Step 7: Close the tap. Remove burette from clamp. Hold burette with top below eye level. Put plastic funnel into top of burette. Fill burette with liquid. Remove plastic funnel. Return burette to burette clamp.Volumetric pipettes are designed to deliver a precise amount of liquid, but only if you a. submerge the end of the pipette into a solution you are delivering. b. allow the pipette to drain freely, and leave any residual solution in the pipette. c. hold the pipette at a 45 degree angle and ensure that all the liquid is delivered.Anion Test - Nitrate (NO3‾) Procedure : Mix H2SO4 4 M into 5 drops of NO3‾ solution (NaNO3 0.5 M) until the solution become acidic (check with litmus paper). Add 5 drops of FeSO4 0.1 M and 2 mL of 4 M H2SO4. When adding in the 4 M H2SO4, make sure the test tube in the position 45°, so that the sulfuric acid can flow through the wall of test tube and form a different layer at the bottom part of the test tube. Results : NO3- solution after adding H2SO4 becomes acidic and is checked by litmus paper and has turned into red colour. Clear solution is obtained at the bottom of the test tube. What is the Chemical equation involved and Discuss the Nitrate test?
- PART 3- LABORATORY EQUIPMENT EQUIPMENT NAME FUNCTION To hold test tubes. Attaches to a retort stand to support glassware being heated. To pour liquid from a large container into a small container. To provide a flame during an experiment. ones To light the Bunsen burner. To attach test tubes to a retort stand. To clean substances out of a test tube. To hold a hot crucible or flask. To hold a hot test tube. To place on the lab bench to prevent burning or to use with ring clamp. To transfer small amounts of liquid. To grow bacteria or contain small experiments. To hold liquids. To measure liquids. To contain experiments (a stopper can be used to close the flask). To hold a hot beaker. To perform an experiment with a different substance in each well. To hold chemicals and perform experiments in. To scoop and transfer small amounts of substances, To stir during experiments that involve mixing or dissolving.SERIAL DILUTION: PROBLEM SOLVING. Set up five (5) tubes on the test tube rack and label them 1-5. Place 0.9 ml of saline to tube #1 and 0.5 ml of saline to tubes # 2-5. Add 0.1 ml of patient's serum to tube #1, mix and transfer 0.5 ml of the mixture to tube # 2. Then, mix and transfer 0.5 ml of the mixture to tube # 3. Mix and continue dilutions through tube # 5. Discard O.5 ml from tube # 5. Finally, add 0.5 ml of the reagent to each tube # 1-5. Compute for the initial dilution of tube #1 and final dilution of tube #5. Show your computation and encircle your final answer.Procedure: Step 1: Pipet 25 mL of prepared sample solution, which has been prepared into a 250 mL Erlenmeyer flask. Step 2: Add 3-5 drops of phenolphthalein indicator solution to the sample solution in the 250 mL Erlenmeyer flask. Step 3: Rinse the buret with three 10 mL portions of standardized 0.1 M HC1 acid solution, before fill this acid solution into the buret and record the initial volume of this acid solution in the burette. Step 4: Titrate the sample solution with the standardized 0.1 M HC1 to the endpoint and record the final volume of this acid in the burette. (Note: phenolphthalein endpoint is from pink color to colorless) Step 5: Repeat the titration for two more times. Step 6: Repeat the same procedure from step 1 to step 5 by using methyl orange as an indicator rather than phenolphathelein. (Note: methyl orange endpoint is from orange to red color). Calculate the alkalinity of the sample for both the indicators and potentiometric method using the following equation: [Alk]…
- read the Procedure and answer the post lab questions below: Using a balance, mass between 1.50 – 2.00 grams of sodium carbonate in a pre-massed 150mL beaker. Add 20 mL of distilled water and stir thoroughly to make sure all the crystals are dissolved. Rinse the stirring rod with a little distilled water after stirring. Using a balance, mass between 1.50 – 2.00 grams of calcium chloride dihydrate in a pre-massed 50 mL beaker. Repeat Step 2 for the solution in the 50 mL beaker. Pour the calcium chloride solution into the 150mL beaker containing the sodium carbonate solution and stir. Mass a piece of filter paper. Fold the filter paper and place it into the funnel. Wet it with a little distilled water to ensure that it is stuck to the sides of the funnel. Slowly pour the mixture from the beaker into the funnel and collect the filtrate into a 125mL erlenmeyer flask. Do not allow the mixture to rise above the edge of the filter paper. Rinse the beaker with about 10 mL of distilled water.…read the Procedure and answer the post lab questions below: Using a balance, mass between 1.50 – 2.00 grams of sodium carbonate in a pre-massed 150mL beaker. Add 20 mL of distilled water and stir thoroughly to make sure all the crystals are dissolved. Rinse the stirring rod with a little distilled water after stirring. Using a balance, mass between 1.50 – 2.00 grams of calcium chloride dihydrate in a pre-massed 50 mL beaker. Repeat Step 2 for the solution in the 50 mL beaker. Pour the calcium chloride solution into the 150mL beaker containing the sodium carbonate solution and stir. Mass a piece of filter paper. Fold the filter paper and place it into the funnel. Wet it with a little distilled water to ensure that it is stuck to the sides of the funnel. Slowly pour the mixture from the beaker into the funnel and collect the filtrate into a 125mL erlenmeyer flask. Do not allow the mixture to rise above the edge of the filter paper. Rinse the beaker with about 10 mL of distilled water.…Which of the following are properties of a good recrystallization solvent? Check all correct answers. Group of answer choices boiling point of solvent < melting point of crystals boiling point of solvent > melting point of crystals Crystals are soluble in solvent at low temperature and soluble at high temperatures. Crystals are soluble in solvent at high temperatures but insoluble or slightly soluble at low temperatures. Solvent boiling point is about room temperature. Impurities should be either soluble at all temperatures or insoluble at all temperatures. An abundant amount of crystals must be recoverable from the solvent.