chapter 11

Question 1

Entropy changes are usually what for a solution?

Answer 1

Positive

Question 2

What are enthalpies values for a solution?

Answer 2

Positive or Negative

Question 3

Which two of the 3 interactions in a solution are endothermic?

Answer 3

Solvent-Solvent, Solute-Solute

Question 4

What is the equation for mole fraction?

Answer 4

(X)=Moles of component/ Total moles of solution

Question 5

What is the equation for mass percent?

Answer 5

Mass %= (X)*100%

Question 6

What is the equation for molality?

Answer 6

m=moles of solute/kg of solvent

Question 7

What is henry’s law and what is it used for?

Answer 7

Solubility=k*p It is used to calculate the solubility of a gas . Solubility is in mol/liter.

Question 8

What is raoult’s law, and what is it used for?

Answer 8

Psolution=Psolvent*Xsolvent. It used to find the vapor pressure of a solution depending on the mole fraction of the solvent.

Question 9

What is i for NaCl?

Answer 9

2 Na and Cl

Question 10

What is I for NaCl2

Answer 10

3 Na and 2 Cls

Question 11

If a solution has a lower vapor pressure, what happens to the boiling point, when compared to a pure solvent?

Answer 11

The boiling point rises.

Question 12

If a boiling point for a solution is higher, than a pure solvent, on the phase diagram where will the liquid to gas line for the solution be, when compared to the line for the solvent?

Answer 12

It will be lower on the graph, meaning that to achieve boiling at the same pressure the solution has to reach a higher temperature. (Look at figure 11.12 if confused)

Question 13

what is the equation for osmotic pressure?

Answer 13

OP=MRT