Which of the following is NOT a property of a potentially good recrystallization solvent? Impurities are always insoluble. Impurities are soluble at room temperature. Compound of interest is only soluble at elevated temperatures. Compound of interest is soluble at room temperature.
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- You need 300. mL of 0.500-M K2Cr2O7. Which method is best to prepare this solution? Explain your choice. (a) Dilute 250. mL of 0.600-M K2Cr2O7 to 300. mL. (b) Add 50.0 mL water to 250. mL of 0.250-M K2Cr2O7. (c) Dilute 125 mL of 1.00-M K2Cr2O7 to 300. mL. (d) Add 30.0 mL of 1.50-M K2Cr2O7 to 270. mL of water.Explain how you could separate an equimolar mixture of Compound X, Y and Z. (a flow chart). NH2 画 HO. Compound X Compound Y Compound ZAn ideal solvent to use for recrystallization is one that: Group of answer choices dissolves the desired compound in ice-cold water temperature but does not dissolve the desired compound at its boiling temperature. a solvent in which the desired compound dissolves at any temperature. a solvent that reacts with the desired compound. dissolves the desired compound at its boiling temperature but does not dissolve the desired compound in ice-cold temperature.
- 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…b) 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.A sample (50 mL) of a bottled water was added to a 100 mL volumetric flask and then diluted to the mark. From this stock solution, 50 mL was taken, added to a 100 mL volumetric flask and diluted to the mark. Final concentration of the serial dilution: 587.7161ppm. 1. what is the concentration in the original bottle (ppm)
- The followings methods are useful to induce crystallization EXCEPT adding a small crystal of the desired compound, called a seed crystal, to the solution adding anhydrous potassium carbonate to the solution and cooling it in an ice bath scratching the inner wall of the Erlenmeyer flask with a glass stirring rod reheating the solution to boiling to boil off some of the solvent, and then allow the solution to cool to room temperature again to effect crystallizationUsing recrystallization techniques, a student attempts to purify 0.50 g of compound H. Based on the solubility of H in the chosen solvent at collection temperature, the maximum percent recovery is 82%. The student obtains 0.396 g of purified crystals. What is their percent recovery? Group of answer choices 41% 64% 79% 82% 97% none of theseSix 50.0 ml volumetric flask 1 through 6 are labeled. 10.00 ml of 2.00 x 10-1 M Fe(NO3)3 solution was then pipet into each volumetric flask. A 1.00,2.00,3.00,4.00 and 5.00ml of 2.00 x 10-3M NaSCN solution was then pipetted to flask 2 through 6 respectively. A sufficient amount of 0.10 M nitric acid was then added to each flask to make each a total volume of 50.00ml. Hint M1V1=M2V2 a)what would be the concentration of Fe(NO3)3 in 0.10M HNO3? b)what would be the concentration of NaSCN in 0.10M HNO3?
- A 690 g of 59% strontium bromide solution is cooled from 60 oC to a certain temperature. Upon addition of around 2 g of strontium bromide, excess solute above saturation started to crystallize. Total recovered crystals is 146.003 g. How many solute is initially dissolved?A sample with a density of 0.502 kg/L was tested in the laboratory. Upon the arrival, a 3 uL of the sample was diluted until the volume was 250 uL. The laboratory assistant who used a different analysis method, computed the molarity of the sample solution was 0.159 M. Determine the concentration of the original sample in percent by volume in a solution (% v/v).Four students are investigating how temperature affects solubility rates of different solutes in water. After preparing their own saturated solutions at 50 ⁰C, they allowed them to cool down to 25 ⁰C. Saturated Solutions in Water Student Solute Temperature ⁰C Quantity Dissolved (g/100 g H2O) Amber LiCl 25 82 50 97 James KCl 25 36 50 44 Rachel NaCl 25 35 50 37 Timothy C12H22O11 25 103 50 130 Analyzing the results of their investigation, how would you rank the students with the quantity of grams that came out of their solutions from GREATEST to LEAST? A James > Rachel > Timothy > Amber B Amber > James > Timothy > Rachel C Timothy > Amber > James > Rachel D Rachel > James > Amber > Timothy