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What structural feature(s) do ethanol and 1-decanol have in common? State a reason for the observed solubility patterns of ethanol and 1-decanol in water and hexane.
What structural feature(s) do toluene and naphthalene have in common? You can goggle the chemical structure. State a reason for the observed solubility patterns of toluene and naphthalene in water and hexane.
Solubility of organic compounds-
Organic compounds tend to dissolve well in solvents that have similar properties to themselves. This principle is often referred as "LIKE DISSOLVES LIKE".
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- Table 1. Solubility Tests. Functional Group Observations (specify type if any) Sample in concentrated (+/-) H2SO4 Color orange Hydroxyl group Hydroxyl group Hydroxyl group 1-butanol Color orange 2-butanol Color orange diisopropyl ether Look at the structures of compounds tested for solubility in concentrated H2SO4. What generalization can be made for a substance to be soluble in concentrated H2SO4 ?2. You have a solution that contains 4.0g of oxalic acid dissolved in 100 mL of water. This solution is placed in a separatory funnel, and then 100 mL of diethyl ether is added to the separatory funnel and an extraction is performed. (Diethyl ether and water are immiscible solvents.) Use the following constants to calculate how much oxalic acid is in each solvent after the extraction. Solubility of oxalic acid in water = 9.5 g / 100 mL Solubility of oxalic acid in ether = 16.9 g/100 mLThe mixture contains benzoic acid, 2-napthol, and naphthalene. Dissolve the mixture in the polar solvent ether. When you react the mixture with 10% NaHCO3(sodium bicarbonatea weak base in aqueous solution) reacts with benzoic acid and forms sodium benzoate an ionic compound (similar to NaCl) that dissolves in aqueous solution (heavier than ether in density) and goes to the bottom of the centrifuge tube or to the bottom of the separatory funnel forming two layers. Then remove the bottom aqueous layer and collect in a beaker labeled as bicarbonate extract. Acidify the bicarbonate extract in the beaker to give benzoic acid. The top ethereal layer contains in the centrifuge tube or separatory funnel 2-napthol and naphthalene. To this top layer add 10% NaOH (sodium hydroxideis a strong base in aqueous solution reacts with only 2-napthol, a weak acid forming 2-napthoxide an ionic compound soluble in aqueous solution (similar to NaCl) that goes to the bottom of the centrifuge tube or to…
- 24.9 g of an unknown molecular solute is dissolved in 5.01 moles of 1,2-ethanediol (C2H6O2), causing the freezing point of 1,2-ethanediol to decrease by 3.32 °C. Calculate the molar mass of the solute. For 1,2-ethanediol, the molar mass is 62.07 g/mol and Kf = 3.11 °C/m.Why is benzoic acid insoluble in water while sodium benzoate is soluble? How are their chemical structures related to their solubility? Which of them - benzoic acid or sodium benzoate - will be more soluble in CHCl3 and why?beer. A 2.39- mg sample of safrole was dissolved in 103.0 mg of diphenyl ether. The solution had a melting point of 25.70°C. Calculate the molecular weight of safrole. The freezing point of pure diphenyl ether is 26.84°C, and the freezing- point- depression constant, Kf, is 8.00°C/m.
- 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…The following questions all are based on the data in this table: Substance Solvent Temp.,oC Solubility, g per 100 mL X heptane 20 23.5 X heptane 80 27.0 X 1-propanol 20 0.6 X 1-propanol 80 8.7 Y heptane 20 4.0 Y heptane 80 4.0 Y 1-propanol 20 22.0 Y 1-propanol 80 31.0…Calculate the Ksp of a compound MX with a solubility of 3.85 × 10–4 g/L, and a molar mass of 146 g/mol. This is a fake compound; M represents some metal and X represents the anion in this ionic compound. Your answer must be consistent with the information given in this problem. Enter your answer in scientific notation, with two decimal places. Example: 1.22e-5 NOTE you must use the letter e and NOT 10.
- Suppose you wanted to prepare a eutectic mixture of naphthalene and diphenylamine.Determine the masses of each naphthalene and diphenylamine required to make 6.000 gof a mixture at the eutectic composition.Suppose that you have a 1:1 mixture of compounds that is comprised of compound X and compound Y. You desire pure compound X and are planning a recrystallization to enhance the purity. Which solvent below is optimal for your recrystallization? Ethanol (boiling point = 78 °C) Solubility At 0 °C 100 °C Compound X 0.05 g/mL 0.20 g/mL Compound Y 0.02 g/mL 0.40 g/mL Water (boiling point = 100 °C) Solubility At 0 °C 100 °C Compound X 0.02 g/mL 0.05 g/mL Compound Y 0.01 g/mL 0.10 g/mL Methanol (boiling point = 65 °C) Solubility At 0 °C 65 °C Compound X 0.04 g/mL 0.10 g/mL Compound Y 0.02 g/mL 0.30 g/mL Acetone (boiling point = 56 °C) Solubility At 0 °C 56 °C Compound X 0.10 g/mL 0.50 g/mL Compound Y 0.20 g/mL 0.50 g/mL Ethyl Acetate (boiling point = 77 °C) Solubility At 0 °C 77 °C Compound X 0.10 g/mL 0.60 g/mL Compound Y 0.30 g/mL 0.60…Part 1. One gram of caffeine dissolves in 55 ml of water; 7 ml of dichloromethane (DCM); 530 ml of diethyl ether; and 100 ml of benzene. Covert the solubility of caffeine in these four solvents into units of mg/ml. a) Solubility of caffeine in mg/ml in water: b) Solubility of caffeine in mg/ml in DCM: c) Solubility of caffeine in mg/ml in Diethyl Ether: d) Solubility of caffeine in mg/ml in Benzene: Which is the optimal solvent to extract caffeine from an aqueous solution? Why? Part 1 Continued: Use intermolecular force (IMF), provide a brief explanation on the solubility of caffeine in water, diethyl ether, observed above. (Hint: draw the skeletal structures for caffeine, DCM and diethyl ether)
