Photon336
  • Photon336
Which of the following solutions will behave closest to an ideal solution?
Chemistry
  • Stacey Warren - Expert brainly.com
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SOLVED
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jamiebookeater
  • jamiebookeater
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Photon336
  • Photon336
\[0.01 M CaCl _{2}\] \[0.01 M NaCl \] \[0.01 M Na _{2}SO _{3} \] \[0.01M Al _{2}(SO4)_{3}\]
Photon336
  • Photon336
Not that sure with this one
Photon336
  • Photon336
@sweetburger

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Rushwr
  • Rushwr
is it 2?
Photon336
  • Photon336
@Rushwr That's correct
Photon336
  • Photon336
how did you come to that answer? just curious
Rushwr
  • Rushwr
Least attraction forces. What I thought was in an solution it breaks in to ions ? @ !
Photon336
  • Photon336
yeah NaOH --> Na+ Cl-
Rushwr
  • Rushwr
yeah apply raoult's law and see. deviatinos
Photon336
  • Photon336
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."
Photon336
  • Photon336
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.
Photon336
  • Photon336
the "mean strength of interactions are the same" across the board.
Photon336
  • Photon336
Also the molecular forces between the molecules must be the same too
Photon336
  • Photon336
They are arguing that |dw:1438974657573:dw| those two molecules if mixed would be ideal they are saying because the interactions between them would be similar.
Rushwr
  • Rushwr
Since they are asking Ideal behaviour !
Photon336
  • Photon336
Let's apply this to the answer choices.
Photon336
  • Photon336
|dw:1438974760572:dw| Not really sure but I feel that for NaCl the interactions would be the same? if they are in water. (not sure about this)
Photon336
  • Photon336
@Woodward do you know why NaCl would be the most ideal, and not the other three. I'm kind of stuck explaining the answer.
Photon336
  • Photon336
I'm going to keep this question open. (I don't think this has to do clearly with the number of ions in solution)
Photon336
  • Photon336
@abb0t thoughts? why would NaCl be the most ideal out out of the other three?
Rushwr
  • Rushwr
Even I am stucked in explaning part
Rushwr
  • Rushwr
I'm not pretty sure but how I took this was taking the solution which had equal like attraction intensities !
Rushwr
  • Rushwr
Like in other cases they weren't equal right
Rushwr
  • Rushwr
|dw:1438975975370:dw|
Rushwr
  • Rushwr
So ithought that would show the least deviation !
Photon336
  • Photon336
makes sense @Rushwr least deviation because of fewest attractions?
Rushwr
  • Rushwr
yeah !
Photon336
  • Photon336
I was basing my interpretation off what wikipedia said.
Photon336
  • Photon336
said like the type of attractions are the same throughout.
Photon336
  • Photon336
really not sure
Rushwr
  • Rushwr
I'm not sure if I am correct but that's how I thought. I think we better solve this @taramgrant0543664
Photon336
  • Photon336
@Bozhena
taramgrant0543664
  • taramgrant0543664
So Im assuming that it's the enthalpy of mixing meaning the more ideal the closer to zero (Delta Hmix). Enthalpy depends on the number of bonds broken in the reactants and the bonds formed in the products, seeing as there is only one option with the 1:1 ratio that would be it
Photon336
  • Photon336
@taramgrant0543664 that's Enthalpy = \[\Sigma bonds broken - \Sigma Bonds formed \] NaCl--> Na+ Cl- One bond broken; what bond is formed?
Photon336
  • Photon336
I'll read up more on this
taramgrant0543664
  • taramgrant0543664
Well there isn't really a bond on the one side there's just the electrostatic attraction between the two ions and eventually they combine due to the force of attraction

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