the solubility of any organic material in a given solvent is due to the intermolecular forces present between the solvent and solute, hexanes (the alkanes isomers of C6H14) are rarely used for extraction purposes. What is a good reason for this experiment?

The solubility of nitrogen gas at 25.0°C and 6.17 atm is 0.00000960 mol/L. Calculate the concentration (in molarity) of nitrogen dissolved in water under atmospheric conditions. The partial pressure of nitrogen gas in the atmosphere is 7.08 atm. a. 6.73×10^5 b. 1.10×10^5 c. 7.80×10^5 d. 3.60×10^5 e. 6.80×10^5

The vapor pressure of pure acetone is 185 torr. When 90.1 g of glucose (MW 180.2) dissolves in 7.5 mol of pure acetone, what will be the vapor pressure of the solution (in torr)? 148 torr 173 torr 197 torr 189 torr

the separation of a mixture into pure substance 3. If a solution is made up by mixing 6.0 g of benzoic acid in 1.00 L of water at 42 °C, would the solution be saturated? Would you expect to see solid on the bottom of the container?

A solution is prepared by adding 425g of AgNO3 to 0.150L of water at 40.0∘C. The solubility of AgNO3 at 40.0∘C is 311g100.mL. How many grams of AgNO3 are expected to precipitate if the temperature is dropped to 0.00∘C where the solubility of AgNO3 is only 122g100.mL? Give the answer with three significant figures.

The diving atmosphere used by the U.S. Navy in its undersea Sea-Lab experiments consisted of 0.036 mole fraction O2 and 0.056 mole fraction N2, with helium (He) making up the remainder. What are the masses of nitrogen, oxygen, and helium in a 8.47 g sample of this atmosphere? Mass of oxygen = Mass of nitrogen = Mass of helium =

Calculating molality.

The presence of a nonvolatile solute causes the freezing point of a solution to be lower than that of the pure solvent. Because freezing point depression depends only on solute concentration and not on the identity of the solute, freezing point depression can be used to determine the molar mass of a solute.   The freezing point of a solution prepared by dissolving 127.3 mg of caffeine in 10.0 g of camphor is lower than that of pure camphor (Kf = 39.7°C/m) by 2.61°C. What is the molar mass of caffeine?   Elemental analysis of caffeine yields the following results: 49.49% C, 5.15% H, 28.87% N, and the remainder O. What is the molecular formula of caffeine? List the elements in the order given by the elemental analysis.

7. Carbon monoxide gas is found to be more soluble in water than hydrogen gas, even though carbon monoxide and hydrogen gas have very similar Lewis structures. Why? What does have similar Lewis structures have to do with the solubility if any between carbon monoxide and nitrogen? 8. What accounts for a meniscus when measuring liquids in the lab? Explain. Chemical Phases and Vapor Pressure: 9. If the temperature of a liquid is increased, what is the effect on the vapor pressure? 10. The vapor pressure of molecule X at 21.7 °C is 35 mmHg. Find the vapor pressure of this molecule at 68°C. AHvap= 26 kJ/mol, R = 8.314 J/mol*K. Chemical Phases and Heat: 11. How does the heat of fusion of chloroform and the heat of fusion of ethane compare? Why? 130

Will the solubility of CaCO3 in water increase or decrease if the pressure of CO2 gas above the saturated solution is increased? Note that CO2 gas reacts with water to produce a weak diprotic acid H2CO3. This acid can undergo the loss of one or two protons to form HCO3- and CO32- ions (these are bicarbonate and carbonate).