Suppose you want to determine the eutectic melting point of a eutectic mixture of adipic acid (literature MP 153 degree C) and salicylic acid (literature MP 158 degree C) .What would you do and what would expect to observe? Be sure to include a very specific detailed plan that any inexperienced organic chemistry lab student could follow if they were to use your procedure.

Suppose you want to determine the eutectic melting point of a eutectic mixture of adipic acid (literature MP 153 degree C) and salicylic acid (literature MP 158 degree C) .What would you do and what would expect to observe? Be sure to include a very specific detailed plan that any inexperienced organic chemistry lab student could follow if they were to use your procedure.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter10: Solutions

Section: Chapter Questions

Problem 24QAP

See similar textbooks

Similar questions

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…
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.
30 20 10 From the procedure 2. Assemble the simple distillation apparatus as generally shown in Figure SD.1 in the lab manual, ensuring that the thermometer bulb is aligned at, or slightly below, the Y in the distillation head. Each ground joint is greased by putting three or four stripes of grease lengthwise around the male joint and pressing the joint firmly into the other without twisting. 3. Attach a water condenser to the distillation head. 4. Remember, water goes in the bottom and out the top. Attach a clamp holder to the end of the drain tube to keep it weighted in the drain. Turn water to a trickle. If it is slowly draining, it is high enough. Begin a low flow of water through the condenser. 5. Place the set up on a heating/stir plate. 6. Turn on the hot plate to start heating the solution. Monitor the temperature and the boiling of the solution throughout the distillation process. 7. Record the temperature of the distillate when the first drops are recovered. 30.0 8. Adjust…
2. Questions: 1. CHM-202 Lab 2 Freezing Point Depression Rev2 G6-2022 10/14 From your understanding of colligative properties, how would you design an experiment to measure the freezing point of a material which freezes at -2 °C using the same apparatus used in this laboratory and any chemical reagents commonly found in a chemical laboratory. Ice is the only material you have available to cool the solutions. If you measured the boiling point of the solution used in Trial 4, would you predict it would have a boiling point equal to, higher than, or lower than the boiling point of pure cyclohexane? Explain your answer.
NO₂ 4 5 NH₂ NH HNO3 Isopropanol, NaOH reflux, 12 h 6 NO₂
explain solvent solvent interaction and solvent solute interaction in 10 pages
Which aqueous solution would you add to a mixture of aniline (structure on the left) and naphthalene to separate the compounds? NH2 O NAOH(aq) O HCI(aq) O NaBr(aq) О КОНaq)
You need to purify 0.8 grams of an impure sample of trans-cinnamic acid. After the purification is completed you isolate 0.57 grams of trans-cinnamic acid and record a melting point range of 129-132 °C. Cinnamic Acid has a solubility in ethanol of 13.9 g/100 ml at 10 °C and a solubility in water of 0.055 g/100 ml at 25 °C. (a) Explain why the recrystallization of trans-cinnamic acid must use a mixed solvent system. Please explain why the sample couldn't be successful recrystallized in ethanol alone. Calculations should be used to support your answer. (b) Calculate the % recovery and the % error for the melting point.
The position of the phases in the separatory funnel (whether the top or bottom phase) is dependent on the relative densities of the solvents. Complete table 1 to indicate whether each of the solvents will be on the top or bottom layer. Table 1. Solubility properties of common organic solvents. Solubility in H20 (g/L, 20-25°C) 9.5 x 10-3 1.79 8.09 17.5 Solubility of H20 (g/L, 20-25°C) 0.31 Phase layer Density (g/mL, 25°C) 0.661 Liquid hexane benzene chloroform 0.76 0.87 1.76 15 170 0.877 dichloromethane diethyl ether 1-butanol 60.5 73 0.3 1.489 1.327 0.713 0.81 0.83 1-octanol 49 ethyl acetate 83 33 0.902
Determine ΔT (T1 – T2), where T1 is the melting point of pure lauric acid and T2 is the melting point of the unknown & lauric acid mixture.
A student prepares a 0.71 Maqueous solution of trimethylacetic acid (C,H,CO,H). Calculate the fraction of trimethylacetic acid that is in the dissociated form in his solution. Express your answer as a percentage. You will probably find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits. Oxto ?
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 ?