A mixture of 5.0 gA, 5.0 g B, and 5.0gC were separated by recrystallization using ethyl acetate as the recrystallization solvent. Shown below are the solubilities (in g/100 mL solvent) of A, B, and Cin ethyl acetate. A B.
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- Hexanoic acid was added to an immiscible biphasic solvent system, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D2) of hexanoic acid in water with respect to CCl4.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?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 M
- You 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 hexaneOne litre of a saturated aqueous solution of Ag2SO4 (MW = 311.79 g mol- 1) at 25 °C is evaporated to dryness. 4.844 g of Ag2SO4 residue was produced. What is the solubility product (Ksp)?You are asked to make the compound [Ni(en)3]SO4. - By using 2.611 grams of NiSO4*6H2O (s) you dissolve the sample in deionized water completely. - You then add 10ml of 25% en into the solution and mix until a single product forms - When the addition of the en is complete, you then add 15ml of ethanol and mix. - using a bench vaccine and Buchner funnel, you filter the precipitate while carefully breaking up the solid until powder form. - the product is the washed with 15ml of ethanol and 15ml of acetone. Powder the solid and leave to dry Which is the limiting reagent? Write a balanced chemical equation for the reaction. How many miles of the product can you theoretically prepare?
- A worker in a dye factory accidentally mixed the compound labeling and you were tasked in identifying one of the dyes. One solution states it contained a saturated 0.25302% dye by mass in ethanol solvent. By measuring its weight and volume, the density of the solution was determined to be 0.79046 g/mL. The solution was further analyzed and determined to have a concentration of 0.00239266 M pink dye. What is the molecular weight of the dye? Hint: %w/v(1a) Pure benzophenane freezes at 66.6 °C. A solution of 7.75 g of biphenyl (C12H10; molar mass = 154.2g/mol) plus 200.08 g of benzophenane froze at 59.9 °C. Calculate the Kf of benzophenane in °C*kg/mol. (b) An unknown solution with possible cations (Ag+, Hg22+, Pb2+) is treated with 6M HCl and a white precipitate forms. Hot water is added to the precipitate, and a white solid remains after filtration. The white solid is treated with aqueous NH3, and the precipitate turns grey or black. The resulting solution is treated with HNO3 and no precipitate forms. What cations can you determine to be present, absent or maybe present? Explain your reasona. Assume a certain extraction has a distribution co-effecient of 7.5. The combination is made up of a certain quantity of caffeine dissolved in 100 ml of water. b. Re-crystallization was used to purify a 25 g organic compound. The amount recovered upon re-crystallization was 8 g. (Write the balancing equations for C,H, and O.:)
- Dissolved 0.273 grams of pure sodium oxalate (Na2C204) in distilled water and added sulfuric acid and titration the solution at 70 °C by using 42.68 ml of KMNO4 solution and has exceeded end point limits by using 1.46 ml of standard oxalic acid (H2 C204) with 0.1024 N. Calculate the normlity of KMNO4. Note that the molecular weight of sodium oxalate (Na2C204) = 134 and its equivalent weight = 67 * %3DThe following evidence was obtained from an experiment to determine the solubility of calcium chloride at room temperature. A sample of saturated calcium chloride solution was evaporated to dryness, and the mass of solid residue was measured.EvidenceVolume of solution (mL) = 15.0Mass of empty beaker (g) = 90.54Mass of beaker and residue (g) = 101.36The solubility of calcium chloride is g/100 mLA salt solution (30% Na2CO3) weighing 1ton iscooled to 20C where the salt crystallizes asdecahydrate. What will be the crystal yield ifthe solubility is 21.5 kg anhydrous Na2CO3/100kg water? (assume that 3% of the totalsolution is lost by evaporation)