When water is shaken with hexane, the two liquids separate into two phases. Which compound is present in the top phase, and which is present in the bottom phase? When water is shaken with chloroform, a similar two-phase system results. Again, which compound is present in each phase? Explain the difference between the two experiments. What do you expect to happen when water is shaken with ethanol (CH3CH2OH)?

When water is shaken with hexane, the two liquids separate into two phases. Which compound is present in the top phase, and which is present in the bottom phase? When water is shaken with chloroform, a similar two-phase system results. Again, which compound is present in each phase? Explain the difference between the two experiments. What do you expect to happen when water is shaken with ethanol (CH3CH2OH)?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter7: Molecular Structures

Section: Chapter Questions

Problem 88QRT

See similar textbooks

Similar questions

Explain the importance of using a thermometer in the simple distillation setup. Enumerate the characteristics of a substance for it to be separated from the heterogeneous mixture by steam distillation. How does steam facilitate the distillation of essential oils? Discuss some applications of simple distillation and steam distillation. Explain why you can use each method for the chosen application. What is the most dominant intermolecular forces of attraction that exist between: a. water and limonene, the major monoterpene component of lemon essential oil? b. water and constituent ions of sodium chloride? 6. Based on your answers in number 5, which pair (water-limonene or water-sodium chloride) exhibits a stronger attraction between their molecules/ions? 7. Describe what happens during the salting-out process in terms of the intermolecular forces of attraction involved as mentioned in your previous answers.
A student is about to dissolve 1.1 g of compound Z in solvent Y. Is 100 mL of solvent Y already enough to dissolve compound Z at a temperature of 25 ℃ or does the student need to get more solvent? If so, how much more? Note: The solubility of compound Z in solvent Y is 3.44 g/L at 25 ℃. *
Why is it necessary to dry the ice before adding it to the warm water?
No Plagiarism Please! Acrylonitrile and ethyl acetate have the same boiling point: 77.2ºC. In one to two sentences, explain what outcome you would expect if a mixture of these two substances were distilled.
1. Which is more efficient for separating the components of a liquid mixture of a liquid mixture, simple or fractional distillation? Why? 2. Explain (in 1 – 3 sentences) how distillation works in separating simple mixtures.
1. A 4 M acetic acid (CH3COOH) solution lowers the freezing point by -8oC; a 4 M KF solution yields a -15oC freezing point depression. What can account for this difference? 2. Based on what you have studied about intermolecular forces, predict which of the following liquid has the highest boiling point and why. All three compounds have comparable molecular weights. Butane, C4H10 b. Propanol, C3H7OH c. Acetone, CH3COCH3
You have two beakers. one contains pure water, the other contains pure methanol. The covalent bonds of methnol molecules are nonpolar. you pour crystals of stable salt into each beaker. Why will the table salt dissolve readily in water but will not dissolve in methanol?
A 10.00 mL sample of ethanol is added to 250.0 mL of water in order to observe the freezing point depression of the water. Consider the possible errors in this experiment, and determine whether each would cause the freezing point of the water to increase, decrease, or remain the same compared with the expected results. It is discovered that the 10.00 g ethanol sample is actually 95% ethanol and 5% water. The ethanol sample is left out for several minutes before being added to the water, allowing a significant amount to evaporate. Instead of starting the experiment with room temperature water, the experiment is started with cold water. Some of the water is splashed out of the container before the ethanol is added. Some of the ethanol and water solution is spilled out of the container during temperature measurement.
What specifically occurs when a liquid mixture is distilled? 1) Components of a solid mixture are separated by differences in boiling points 2) Components of a solid mixture are separated by differences in melting points 3) Components of a liquid mixture are separated by differences in boiling points 4) Components of a liquid mixture are separated by differences in melting points
2. a) How could you calculate a water pressure above a 1M NaCl solution (salt in water)? Could you explain what the meaning of your formula? What would be the boiling temperature of such solution at a normal external pressure? b) How could you separate components by distillation? Explain on a phase diagram.
A chemist is given a nonelectrolyte white powder for analysis. 38.7 g of this substance isdissolved in 100.0 g of water. It is determined that the resulting solution freezes at –4.0°C.Additionally, the elemental composition of the substance is identified and found to be 40.0%C, 6.7% H and 53.3 % O by mass. Find the molecular formula of this unknown white powderusing these experimental evidences (Kf of water: 1.86°C/m, C: 12 g/mol, H: 1 g/mol, O: 16g/mol)
A scientist is about to dissolve 0.9 g of compound U in solvent P. Is 100 mL of solvent P already enough to dissolve compound U at 25℃ or does the scientist need to get more solvent? If so, how much more is needed?Note: The solubility of compound U in solvent P is 3.62 g/L at 25 ℃.