You are tasked with performing a recrystallization. You have 3 potential solvents to use, but you don't know which one will work. How will you go about deciding which solvent to use?
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- Step 1: In tube 1, you add 100 ul of plasma to 900 ul of distilled water. Step 2: In tube 2, you then take 100 ul from tube 1 and add 900 ul of distilled water. Step 3: In tube 3, you then take 100 ul from tube 2 and add 900 ul of distilled water. What is the final/total dilution factor in tube 3 at the end of step 3?50 mL of stock solution were taken and added to flask. Then 50 mL of Di water were added to the flask. This is solution 1. Then 50mL of solution 1 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 2. Then 50mL of solution 2 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 3. Then 50mL of solution 3 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 4. Find the concetrations of each solution. Information of stock solution - molar mass- 534.3g/mole 0.587g in MilliQ5. Suppose you have a mixture of water and your 2-chloro-2-methylbutane product in a separatory funnel. Use densities to predict which phase will be the top layer in the funnel. a. 2-chloro-2-methylbutane (organic phase) b. water (aqueous phase) c. there would only be one phase since the substances are miscible
- Procedure A: Molarity (M=g/MM/L) Step 1. Place one-eighth of a teaspoon (this weighs approximately 0.5 grams) of NaCl (table salt) in the graduated cylinder provided. Then add distilled water to that graduated cylinder until the level of the water reaches 45.00 mL. Mix thoroughly about 1 minute. Pour solution into a somewhat clear cup. Remember what this looks like for Procedure B. Questions: Is this a saturated solution? Why or why not? Take a picture and insert a picture (compress your image) of your solution here. Save this solution for Step 2. Calculations: Determine the Molarity of this solution using the formula M = g/MM/L. You know the grams (one-eighth of a teaspoon weighs approximately 0.5 grams), look up the Molar Mass of NaCl, and convert your mL to L to solve the problem.) Show your calculations for Molarity here. C % 31 D < hp & * ✔Pre-lab question #8: Suppose you were dissolving a metal such as zinc with hydrochloric acid. How would the particle size of the zinc affect the rate of its dissolution? As the particle size of the zinc increases, the rate of dissolution AA (decreases/increases).• Rinse the test tubes with distilled water. Part B Follow these steps to complete the table: 1. Reuse the same test tubes from part A, labeled Fe2+ and Fe3+. Be sure they're clean. 2. Add 4 milliliters of iron(II) sulfate to the test tube labeled Fe2*. 3. Add 4 milliliters of iron(II) nitrate to the test tube labeled Fe3+. 4. Add 4 milliliters of potassium iodide to each test tube. 5. Add 1 milliliter of the prepared starch solution to each test tube. 6. Record your observations, noting any evidence of a chemical reaction. If there is no evidence of a reaction, write "no reaction." В I U 三E E三 三 X, Font Sizes A - Substances Mixed Iron lon Present Description of the Reaction iron(II) sulfate, potassium iodide, and starch iron(II) (Fe2+) iron(III) nitrate, potassium iodide, and starch iron(III) (Fe)
- 4. To set up your seed assay, you’ll conduct serial dilutions of a fuel derived from a renewable feedstock. To begin, you’ll make 20 mL of a 10% solution of your assigned fuel. a. How many grams of fuel will you need to make your solution? Hint: The definition of a 10% solution is 10 grams of solute (fuel in this case) in 100 mL of solution. b. You will then pour 10 mL of your 10% solution into an empty beaker. How much water (in mL) should you add to the beaker to create a 5% solution? Hint: Assume all of your fuel is completely dissolved and the volumes of the solutions are additive.Rank a series of molecules by expected solubility in water based on polarity and hydrogen bonding. Some slightly soluble compounds are included in this exercise. Rank the organic compounds from most soluble to least soluble. To rank items as equivalent, overlap them. View Available Hint(s) Reset Help Η Η Η Η H H H H ннно Н-С-С — С —С— ОН Н-С-С-С —С -Н Н-С—С—С — С -ОН Η Η Η Η Η Η Η Η Η Η Η нн Η Η Н-С—С— О—С—С — Н нн нн Most soluble Least solublePlease help me fill in the highlighted. I don't know. Please explain how to get the answers. Thank you in advance.
- Materials Needed solid I2 solid CUSO4-5H20 food dye solid (NH4)2SO4 heavy metals waste container halogenated waste container non-halogenated waste container semi-micro test tubes and rack regular test tubes and rack squash pipettes acetone cyclohexane propan-2-ol Method Part A: Solubility of ionic and molecular solids 1. Place a small amount (about the size of 1 grain of rice, see picture) of copper sulfate into each of three DRY semi-micro test tubes. Add 20 drops of water to the first test tube and gently flick the test tube with your finger to ensure mixing. 2. Repeat step 1 using acetone in place of water as the solvent in the second test tube. 3. Repeat step 2 replacing acetone with cyclohexane in the third test tube. Hold the test tubes against a white background to compare the solubility of copper sulfate in the three solvents and record your results. Discard these mixtures into the heavy metals waste container in the fume cupboard. Once these test tubes have been emptied you…Blank 1 is a condition that happens when the rates of dissolution and crystallization become equal. Blank 1 Add your answerb) Will the sample be contaminated with any of the impurities? Calculate the percent purity of the initial sample (in terms of compound A) - ( i.e. express the amount of compound A in the initial sample as a percentage of the mass of initial sample). Calculate the percent purity of the final sample (in terms of compound A) - (i.e. express the amount of compound A in the final sample as a percentage of the mass of final sample). Did the recrystallization procedure result in an increase of the percent purity of compound A in the sample? Comment on the results.