[baby]

hi everybody.
explain me, pls


i understand this:  if solubility product (Ksp) is less than Ksp_saturated, than particles will dissolve;
is Ksp is higher than Ksp saturated, particles will precipitate until Ksp_saturated is reached.

But how to estimate this:

1. the lower Ksp , the more (or less ) soluble the compound is ?

thanx

[UG]

But how to estimate this:

1. the lower Ksp , the more (or less ) soluble the compound is ?

The lower the K_sp the less soluble the compound is

[baby]

one more question, pls

how to relate the sizes of particles and Ksp? 


smaller particles can be easier dissolved (are more soluble), so the smaller sizes the higher Ksp ??  is that correct?

 thanks

[Borek]

No relation between size of "particles" (whatever they are meant to be) and Ksp.

[baby]

I am just trying to understand it logically, not necessary quantitatively,


Just to know if the way I think is right or not:

smaller particles can be easier dissolved => they are more  soluble than larger particles.  The more soluble they are=> higher Ksp for them =>  for smaller particles the Ksp is higher.

it should be related with the surface energy needed to overcome when particles need too be dissolved. for smaller particles such energy is lower=> we can easier overcome this energetic barrier from which I assume that smaller particles can be easier dissolved and hence are more soluble and have higher Ksp

Correct me please if the way i think is wrong

 

[baby]

please have a look,  is there anything wrong in the way I posted above .

[Borek]

As I told you - there is no such relation, so your thinking must be wrong.

[MrTeo]

I think that the size of particles only affects the solvation speed: being smaller they are dissolved quickly but we can't say that the solubility increase... trying to explain that easily we could say that, once solvated, larger or smaller crystals (an example could be salt if you want to think at it concretely) are equally dispersed in water and there's no difference between their saturated solutions: in both systems there's a dynamic equilibrium between the ions in solution and the undissolved compound. This equilibrium is in fact linked to the value of K_sp.

I'd say that you could also try to verify this wheighing the amount of salt you're able to dissolve in a fixed amount of water using both larger and smaller crystals. You'll see that solubility doesn't increase.