The fact that the oceans contain salt water shows that polar solvents dissolve ionic solutes.
Answer: TRUE
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Chemistry Chapter 13
- Which one of the following substances is more likely to dissolve in CCl4?
- Formation of solutions where the process is endothermic can be spontaneously provided that
- Two solutions that are isotonic have the same __.
- As the temperature of a solution increases, the solubility of a gaseous solute ____.
- The molality of a solution is defined as the amount of moles of solute divided by what?
- Which substance below is NOT a colloid?
- A sample of 2.05 g of polystyrene of uniform polymer chain length was dissolved in enough toluene to form 0.100 L of solution. The osmotic pressure of this solution was found to be 1.21 kPa at 25 C. Calculate the molar mass of the polystyrene.
- The osmotic pressure of an aqueous solution of a certain protein was measured to determine the protein's molar mass. The solution contained 3.50 mg of protein dissolved insufficient water to form 5.00 mL of solution. The osmotic pressure of the solution at 25 C was found to be 1.54 torr. Treating the protein as a nonelectrolyte, calculate its molar mass.
- If the pure water in the left arm of the U-tube is replaced by a solution more concentrated than the one in the right arm, what will happen?
- In osmosis, there is the net movement of solvent from the area of ____ solvent concentration to the area of ___ solvent concentration.
- Calculate the freezing point of a solution containing 0.600 kg of CHCl3 and 42.0 g of eucalyptol (C10H18O), a fragrant substance found in the leaves of eucalyptus trees.
- Automotive antifreeze consists of ethylene glycol, CH2(OH)CH2(OH), a nonvolatile nonelectrolyte. Calculate the boiling point and freezing point of a 25.0 mass % solution of ethylene glycol in water.
- A 0.100 molal solution of which compound below will have the lowest freezing point?
- Nonvolatile solute-solvent interactions also cause solutions to have ____boiling points and ____freezing points than the pure solvent.
- The vapour pressure of a solution is ___ than that of the pure solvent.
- Changes in colligative properties depend only on ___.
- A solution with a density of 0.876 g/mL contains 5.0 g of toluene (C7H8) and 225 g of benzene. Calculate the molarity of the solution.
- What is the molarity of a solution made by dissolving 36.5 g of naphthalene (C10H8) in 425 g of toluene (C7H8)?
- If an aqueous solution is very dilute, will its molality be?
- A solution is made by dissolving 4.35 g glucose (C6H12O6) in 25.0 mL of water at 25 C. Calculate the molality of glucose in the solution. Water has a density of 1.00 g/mL.
- The solubility of solid solutes in liquid solvents increases with increasing ____.
- The solubility of liquids and solids ____appreciably with pressure.
- The solubility of a gas in a liquid is ____ to its pressure.
- In general, the solubility of gases in water ____ with increasing mass.
- Arrange the following substances in order of increasing solubility in water: