David decides that it is better to create a blend containing 50% NaCI, 33% KCI and 17% CaCl2, than to buy the pre-prepared blend. Calculate how much it will cost to produce 65 tons of his recommended blend. Don't forget the $5/ton mixing fee. You may find it helpful to refer to Table 2.1 in your lab manual.
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- 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.…#1. Part A. in a drug discovery program, a hit compound________. A. Shows activity in an animal model of disease B. Is active in target/ whole-cell assays in vitro C. Is purchased from a commercial vendor D. Is derived from screening natural product libraries Part B. When using TLC to monitor an organic chemistry reaction, which could be an indication that your desired reaction has gone to completion? A. the stationary phase changes colors B.the mobile phase runs to the top of the tlc plate C.the starting material spot disappears and a new spot appears D,the starting material spot remains on the tlc plateVOLUMENTRIC ANALYSIS Instructions: Answer each of the problems below by showing your solutions neatly and logically. Copy and answer each problem and please box your final answers. 5. Calculate the Mgo content of milk of magnesia, 12.32 g of which was dissolved in 50.00 mL of 1.0340 N sulfuric acid, producing a mixture that required 24.60 mL of 1.1265N NaOH. NOTE: KINDLY WRITE THE SOLUTIONS ON A SEPARATE SHEET OF PAPER
- Which statement is true? Statement 1: In chromatography, the compound mixture moves along with the mobile phase through the stationary phase and the components get separated depending on the degree of interaction and adhesion Statement 2: Compound A is more soluble in the mobile phase compared to compound B. Thus, compound A would most probably have a higher Rf value.How to determine the difference between primary , secondary and tertiary alcohol in the laboratoryHow do you separate sodium hydroxide from the crude mixture?
- How many grams of NaAsO, should be weighed out to prepare a stock solution of 100 mg/L in 500 mL deionized water. Use the stock solution to prepare 4 different standard solution that can be used to prepare an analytical calibration curve to measure the concentration of 750 sample in the concentration range of 10-35 mg/L. Draw a proposed calibration curve (based on the results you achieved).Show the theoretical and % yield calculations for your synthesis. Please be sure to use appropriate identifiers and conversion factors. 5.0mL acetic acid (5.3g) 3.0mL 1-octanol (0.829 g/mL) 25 drops of concentrated sulfuric acid (1.5mL total). If necessary, assume 1 drop to be 0.05mL.Draw a schematic diagram using this information. Preparation of the solution Take about 25-30 ml of distilled water in a beaker and add powdered crude copper sulphate while stirring the solution so that the powder dissolves. Keep adding the powdered sample till a little of it remains undissolved, even if it is stirred thoroughly. Now add 2-3 ml of dil. H2SO4 to make the solution clear. This prevents the hydrolysis of copper sulphate. Filtration of the solution Take a funnel and fix a filter paper in it and clamp it to a stand. Place a china dish under the funnel. The stem of the funnel should touch the wall of the china dish to avoid the solution splashing out. Pour the solution into the funnel over a glass rod and collect the filtrate in a china dish. The insoluble impurities are left in the filter paper as residue. Concentration of the filtrate to crystallisation point Heat the china dish on a sand bath till the solution is reduced to about one-third of its original volume. To…
- 1.Each of the student statements below is wrong. You will need to explain why they are not correct. (a) All my compound dissolved right away in the small amount of solvent I added at room temperature, and I didn’t need to heat it at all. This means I’m going to get lots of pure compound out. (b) I did a recrystallization of naphthalene and my percent recovery was very high (99%), so I must have pure product. (c) When you’ve dissolved all your compound in hot solvent, and you’re in a hurry, it’s ok to just place it straight into the ice bath.A student rushed through this experiment. Describe the effect that the following procedural changes would have on the percent recovery of acetanilide. Briefly explain the basis of each answer.(a) Rather than adding 0.5-mL portions of boiling solvent to the acetanilide, the student added 5-mL portions of boiling solvent.(b) The student did not pre-heat the gravity filtration apparatus.(c) The student forgot to cool 5 mL of solvent in Part 5 and washed the crystals with room-temperature solvent.2. Any organic solvent waste (besides methanol and ethanol) generated in this experiment should be collected in your fume hood and poured into the waste container as directed. This waste should not be poured down the drain. true or false