Colligative Properties

When CH₃OH is dissolved in water, how many particles are in solution for each unit?

• 1

• 3

• 4

• 5

• 6

The graph above is a heating curve of water. Which number in the graph represents the process of freezing?

• 1

• 2

• 3

• 4

• 5

The freezing point of a solution is ____ the freezing point of the pure solvent.

• the same as
• lower than
• higher than
• no relation to

The van't Hoff factor measures the number of particles formed in solution. What is the van't Hoff factor for the compound Na₂SO₄?

• 1

• 3

• 5

• 7

Electrolytes have a greater effect on colligative properties than nonelectrolytes do because electrolytes

• are volatile

• have higher boiling points

• produce fewer moles of solute particles per mole of solvent

• produce more moles of solute particles per mole of solvent

When 26.0 g of NaCl, are dissolved in 0.5 kg of water, what is the freezing point of this solution? (K_f = 1.86 ^oC/m)

• -3.3

• 103.3

• -1.7

• -0.8

A solution contains 15.5 g of a nonelectrolyte and 200 g of water. The water freezes at -4.5° C and K_f = 1.86° C/m. What is the molar mass of the nonelectrolyte?

• 18g/mol

• 32g/mol

• 16g/mol

• 46g/mol

• 53g/mol

Molality is measured in

• mols per kg
• mols per L
• mols per kJ
• mols per mL

What is the freezing point of a 1.5 m solution of sucrose in water? (K_f = 1.86°C/m)

• -2.8°C
• -1.2°C
• -0.81°C
• 0.81°C

How many moles of HCl (molar mass = 36.46g/mol) are present in .70L of a .33M HCl solution. $\ Molarity=\ \frac{moles\ ofsolute}{L\ of\ solution}$  

• .23 mol

• .28 mol

• .38 mol

• .47 mol