Properties of Solutions _II

Front

What is the molarity of a solution that contains 0.154 moles of Na+ in 1.00 L?

Back

The molarity (M) is calculated as moles of solute per liter of solution. Therefore, M = 0.154 moles / 1.00 L = 0.154 M.

Front

What is the freezing point depression formula?

Back

Front

Define the van't Hoff factor (i).

Back

The van't Hoff factor (i) is the number of particles into which a solute dissociates in solution. For example, NaCl dissociates into two ions (Na+ and Cl-), so i = 2.

Front

What is the effect of adding a solute on the boiling point of a solution?

Back

Adding a solute to a solvent increases the boiling point of the solution, a phenomenon known as boiling point elevation.

Front

What is the freezing point of pure water?

Back

The freezing point of pure water is 0.0 °C.

Front

How do you calculate the molality of a solution?

Back

Front

What is the boiling point elevation formula?

Back

Front

What happens to the freezing point of a solution when more solute is added?

Back

The freezing point of the solution decreases as more solute is added.

Front

What is the molecular weight of ethylene glycol (C2H6O2)?

Back

The molecular weight of ethylene glycol (C2H6O2) is 62.07 g/mol.

Front

What is the significance of the freezing point depression constant (kf)?

Back

The freezing point depression constant (kf) is a property of the solvent that indicates how much the freezing point will decrease per molal concentration of solute.