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Photon336
 one year ago
Which of the following solutions will behave closest to an ideal solution?
Photon336
 one year ago
Which of the following solutions will behave closest to an ideal solution?

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Photon336
 one year ago
Best ResponseYou've already chosen the best response.0\[0.01 M CaCl _{2}\] \[0.01 M NaCl \] \[0.01 M Na _{2}SO _{3} \] \[0.01M Al _{2}(SO4)_{3}\]

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0Not that sure with this one

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0@Rushwr That's correct

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0how did you come to that answer? just curious

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.1Least attraction forces. What I thought was in an solution it breaks in to ions ? @ !

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0yeah NaOH > Na+ Cl

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.1yeah apply raoult's law and see. deviatinos

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0This 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 longerrange 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., 1butanol and 2butanol, 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
 one year ago
Best ResponseYou've already chosen the best response.0like 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
 one year ago
Best ResponseYou've already chosen the best response.0the "mean strength of interactions are the same" across the board.

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0Also the molecular forces between the molecules must be the same too

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0They 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
 one year ago
Best ResponseYou've already chosen the best response.1Since they are asking Ideal behaviour !

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0Let's apply this to the answer choices.

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0dw: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
 one year ago
Best ResponseYou've already chosen the best response.0@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
 one year ago
Best ResponseYou've already chosen the best response.0I'm going to keep this question open. (I don't think this has to do clearly with the number of ions in solution)

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0@abb0t thoughts? why would NaCl be the most ideal out out of the other three?

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.1Even I am stucked in explaning part

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.1I'm not pretty sure but how I took this was taking the solution which had equal like attraction intensities !

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.1Like in other cases they weren't equal right

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.1So ithought that would show the least deviation !

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0makes sense @Rushwr least deviation because of fewest attractions?

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0I was basing my interpretation off what wikipedia said.

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0said like the type of attractions are the same throughout.

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.1I'm not sure if I am correct but that's how I thought. I think we better solve this @taramgrant0543664

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.1So 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
 one year ago
Best ResponseYou've already chosen the best response.0@taramgrant0543664 that's Enthalpy = \[\Sigma bonds broken  \Sigma Bonds formed \] NaCl> Na+ Cl One bond broken; what bond is formed?

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0I'll read up more on this

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.1Well 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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