Chapter 16 - Solutions

Question 0

Describe the state of equilibrium in a saturated solution that contains undissolved solute

Answer 0

A state of dynamic equilibrium exists between the saturated solution and any undissolved solute.

Question 1

What determines how fast a substance will dissolve?

Answer 1

• Agitation
• Temperature
• Particle size of solute

Question 2

What conditions determine the solubilities of solid, liquid, and gaseous solutes in a solvent?

Answer 2

Temperature for all. Both temperature and pressure for gaseous solutes.

Question 3

What determines whether or not a substance will dissolve?

Answer 3

A substance will dissolve if it has a compatible chemical composition to the solvent.

Question 4

Name three colligative properties of solutions.

Answer 4

• Vapor pressure lowering
• Freezing point depression
• Boiling point elevation

Question 5

1) Why does a solution have a depressed freezing point compared with the pure solvent?
2) Why does a soliton have an elevated boiling point compared with the pure solvent?

Answer 5

1) The presence of solute in water disrupts the formation of the orderly pattern particles of solids take on. As a result, more kinetic energy must be withdrawn from the solution than from the pure solution to solidify.
2) In order for a solution to boil, we must add more kinetic energy to raise the vapor pressure to atmospheric pressure. The presence of solute elevated the boiling point of the solution.

Question 6

Would a dilute or a concentrated sodium fluoride solution have a higher boiling point?

Answer 6

The more concentrated the solution, the most colligative properties change.

Question 7

How do you calculate the molarity (M) of a solution?

Answer 7

Molarity (M) = moles of solute/liters of solvent.

Question 8

How does the # of moles of solute before a dilution compare with the # of moles of solute after the dilution?

Answer 8

Moles of solute does no change.

Question 9

Practice #22 pg. 531

Answer 9

Okay.