A mixture of 5.0 gA, 5.0 g B, and 5.0 g C were separated by recrystallization using ethyl acetate as the recrystallizatic solvent. Shown below are the solubilities (in g/100 mL solvent) of A, B, and C in ethyl acetate. A cold hot cold hot cold Hot 1.7 2.5 2.2 3.6 1.6 5.3 What is the percent recovery of the purified crystal after one recrystallization? Answer: 51.33
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- Although other solvents are available, dichloromethane(CH₂Cl₂) is still often used to “decaffeinate” drinks because thesolubility of caffeine in CH₂Cl₂ is 8.35 times that in water.(a) A 100.0-mL sample of cola containing 10.0 mg of caffeine is extracted with 60.0 mL of CH₂Cl₂. What mass of caffeine re-mains in the aqueous phase? (b) A second identical cola sampleis extracted with two successive 30.0-mL portions of CH₂Cl₂.What mass of caffeine remains in the aqueous phase after each extraction? (c) Which approach extracts more caffeine?Cyclonite, also known as RDX (Research Department Explosive), is used to make Semtex, a plastic explosive, when mixed with PETN. Semtex was used in the bomb that brought down PanAm flight 103 over Lockerbie, Scotland in 1988 killing 270 people. RDX is typically recrystallized from acetone. 1 gram of RDX is soluble in 100 mL of cold acetone (0 0C) and in 25.0 mL of boiling acetone. A student performed recrystallization starting with using 5.0 mL of acetone. a. What is the maximum amount of crude RDX the student can purify given this volume of acetone in order to maximize the % recovery? b. A student reported 65% recovery from the process of recrystallization after using 5.0 mL of acetone and the mass that can be used with that volume (part a). Is 65% the maximum % recovery of RDX using the volume you calculated in part a? Show your work.A nearly saturated solution of 0.40 g L-ascorbic acid in 75 mL water is to be extracted into 75 mL diethyl ether. How much percentages of L-ascorbic acid would be extracted using multiple extraction of three equal portions of fresh diethyl either? (Taking the ratio of the compound's solubility in diethyl ether compared to water gives an approximate K of 5). Show your calculation steps in the answer.
- The Henry’s law constant for CO2 in water at 25 °C is3.1x 10-2 M atm-1. (a) What is the solubility of CO2 inwater at this temperature if the solution is in contact withair at normal atmospheric pressure? (b) Assume that all ofthis CO2 is in the form of H2CO3 produced by the reactionbetween CO2 and H2O:CO2(aq) + H2O(l)------>H2CO3(aq)What is the pH of this solution?Below is a solubility table for an unknown organic soli. The solid is white with a melting point of 75°C . Which of the solvent would you use for recrystallization? Explain your choice2.3 - At temperature of 18°C was 4,7 g of silver molybdate (M = 376 g mol–1) mixed with 500 cm3 of a) distilled water b) solution of AgNO3 with concentration of 0,02 mol dm–3 c) solution of Na2MoO4 with concentration of 0,02 mol dm–3 Determine, how many percent of Ag2MoO4 will dissolve in each case. Solubility equilibrium of Ag2MoO4 is 3,1.10-11.
- How much 1.0 M sodium bicarbonate solution (in mL) is needed to stoichiometrically react with 25 mL of 4.5% (w/v) acetic acid? Molecular weight of sodium bicarbonate = 84.007 gmol, molecular weight of acetic acid = 60.052 g/mol please provide explanationYou are given a substance that is qually soluble in water and hexane (two immisible solvents) a) what is Kd B) if you start with 10g of the substance dissolved in 100ml of water and are given 100ml of hexane to extract with, algebriaically show that it is better to do two smaller extractions using 50 ml of hexane for each extraction than it is to do one extraction using 100ml of hexaneThe compound lead(II) sulfate has a solubility of 4.824E-3 g/100mL at 25 degC.What is the molar solubility of this solution at saturation? 0.0002 mol/L What is the Ksp at 25 degC for lead(II) sulfate? What is the molar solubility of lead(II) sulfate in 0.28 M lead(II) nitrate ?
- 50.0 mL of a 0.60 M solution of pyridine in ethanol is to be prepared by measuring out a known volume of pure liquid pyridine and diluting to 500 mL with ethanol. The molar mass of pyridine is 79.1 g/mol, and its density at room temperature is 0.982 g/mL. What volume of pyridine is required for this solution?3. On a separate sheet show calculations for: 5.0 mL of water Solubility (g/L) of NiCl₂ = 0.67 Molar solubility of NiCl2 [Ni²+] = [CI] =_ - Ksp for NiCl2 = - g/L 3.35g of Nicla, net 3.359 Nicl₂ /0.0 NICI M M MIf you know that sodium bicarbonate has a solubility of 8.4 g in 100g water at 18 °CI. Calculate (a) the molarity and (b) the molality of 8.4 g of Sodium bicarbonate in water II. if you had 200 mls of water, what is the minimum amount of Sodium bicarbonate that you will require to achieve supersaturation? III. If 150 mls of a stock solution of sodium bicarbonate having a concentration of 0.5 M was diluted to 300 mls. What will be the final concentration of the diluted solution?