Question

Which of the following solutions will behave closest to an ideal solution?

Answer 1

\[0.01 M CaCl _{2}\]
\[0.01 M NaCl \]
\[0.01 M Na _{2}SO _{3} \]
\[0.01M Al _{2}(SO4)_{3}\]

Answer 2

Not that sure with this one

Answer 3

@sweetburger

Answer 4

is it 2?

Answer 5

@Rushwr That's correct

Answer 6

how did you come to that answer? just curious

Answer 7

Least attraction forces. What I thought was in an solution it breaks in to ions ? @ !

Answer 8

yeah NaOH --> Na+ Cl-

Answer 9

yeah apply raoult's law and see. deviatinos

Answer 10

This is the explanation from none other than (wikipedia)

"Ideality of solutions is analogous to ideality for gases, with the important difference that intermolecular interactions in liquids are strong and cannot simply be neglected as they can for ideal gases. Instead we assume that the mean strength of the interactions are the same between all the molecules of the solution.

More formally, for a mix of molecules of A and B, the interactions between unlike neighbors (UAB) and like neighbors UAA and UBB must be of the same average strength, i.e., 2 UAB = UAA + UBB and the longer-range interactions must be nil (or at least indistinguishable). If the molecular forces are the same between AA, AB and BB, i.e., UAB = UAA = UBB, then the solution is automatically ideal.

If the molecules are almost identical chemically, e.g., 1-butanol and 2-butanol, then the solution will be almost ideal. Since the interaction energies between A and B are almost equal, it follows that there is a very small overall energy (enthalpy) change when the substances are mixed. The more dissimilar the nature of A and B, the more strongly the solution is expected to deviate from ideality."

Answer 11

like paragraph one is saying that the ideal solutions are kind of like ideal gases. but it's like you can't ignore that in solution there are going to be some intermolecular forces of attraction.

Answer 12

the "mean strength of interactions are the same" across the board.

Answer 13

Also the molecular forces between the molecules must be the same too

Answer 14

They are arguing that

those two molecules if mixed would be ideal they are saying because the interactions between them would be similar.

Answer 15

Since they are asking Ideal behaviour !

Answer 16

Let's apply this to the answer choices.

Answer 17

Not really sure but I feel that for NaCl the interactions would be the same? if they are in water. (not sure about this)