CHEM-1602 Chapter Notes -Aqueous Solution, Intermolecular Force, Colligative Properties

What best explains why dissolving a gas in water is always exothermic? A) There are no solute-solute interactions to break up B) There are no solvent-solvent interactions to break up C) The resulting solute-solvent interactions are especially powerful D) The solubility of gases in water is higher in temperature E) Water is a polar solvent Given the solubility graph below determine which statement is correct. A) Both substance X and Y represent gaseous substances. B) Substance Y is more soluble for a given temperature and quantity of solvent than substance X. C) Substance Y is unsaturated at 30 g/100mL water and a temperature of 100 degree C. D) At 0 degree C substance X is more soluble than substance Y. E) An increase in pressure would cause an increase in solubility for both substance X and Y. Which of the following properties are not considered to be colligative properties? A) Vapor-pressure lowering B) Boiling-point elevation C) Freezing-point depression D)

An ionic compound. is more likely to dissolve in a polar solvent, such as water, than a non-polar solvent, such as hexane. always has a pH greater than 7 generates excess OH^- when dissolved in water. cannot be separated from another ionic compound in a mixture Chromatography techniques can be used for separation and absolute identification of substances when combined with the proper detector. True False pH is a measure of the acidity of an aqueous solution. True False In HPLC, the mobile phase is always a gas. True False