Introductory Chemistry Study Set 7

Solutions have a higher boiling point than pure solvents.

Solutions exist in all phases of matter.

Solutions have a lower vapor pressure than the pure solvent.

The freezing point of a 0.5 m solution of NaCl is water is less than 0°C.

CH₃OH is not soluble in water

Solutions have a higher freezing point than their pure solvents.

A solution is made by mixing 2.00 mol of solute and 15.0 mol of solvent. The mole fraction of the solute is 0.133

Molarity of a solution is the number of moles of solute divided by the milliliters of the solution.

NaOH will be more soluble in CCl₄ than H₂O.

The boiling point of a 5.00 m solution of C₆H₄Cl₂ in CCl₄ is 101.6°C. Assume that C₆H₄Cl₂ is not volatile and K_b = 4.95°C/m.

The freezing point of a 1.9 m solution of NaCl in H₂O is -3.5°C if K_f = 1.86°C/m.

Molality refers to the number of moles of solute per gram of solvent.

Which of the following terms refer to the major component of a solution?

The van't Hoff factor for CaCO₃ is 2.

The van't Hoff factor for CCl₄ is 5.

For ionic solutions, the total ion concentration is the sum of the individual ion concentrations.

In both dilution and concentration, the amount of solute stays the same.

The molarity of a solution is 25 M if 5.0 moles of the solute is present in 5.0. liters of the solution.

Osmotic pressure is the tendency of a solution to pass solution through a semipermeable membrane due to concentration differences.

If 25.0 mL of a 1.0 M solution is diluted to 50.0 mL, the concentration becomes 0.50 M.