Solubility

[rainashley]

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Which is more soluble? A1B1 with a Ksp of 10^-6 OR A1B3 with a Ksp of 10^-6? Why?
What do we know about a solution from its Ksp? What does the Ksp tell us exactly?
Thanks

 

[loveoforganic]

Ksp1 = [A]

[A] =

Solubility is a measure of number of particles in solution.

So, 10^-6 = (X)(X) = (X)^2

solubility = (10^-6)^(1/2)


Ksp2 = [A]^3

(X)(3X)^3 = 10^-6

27X^4 = 10^-6

solubility = [(10^-6)/(27)]^(1/4)

 

[rainashley]

Which is more soluble?

 

[RogueUnicorn]

🤣

 

[loveoforganic]

🤣

@OP: You can do the math.

 

[RogueUnicorn]

@OP: You can do the math.

what's left of it, anyway

 

[JFK90787]

Ksp is equilibirum expression for solids. Since the starting solute is solid, it doesn't get included in the equilibirum expression with the products.

And yeah, loveoforganic did the messy part for you. If you can't figure out solubility from that then

 

[Econ2MD]

To be fair to the OP, showing the math equations doesn't exactly explain the concept, which is what the MCAT is in theory testing. Maybe you could explain the concept in words...might be more helpful than ridicule?

 

[loveoforganic]

Maybe if his followup question had anything to do with the concepts 😉

 

[HopefulOncoDoc]

OP, since solubility is a measure of the number of particles in solution, the greater x value between the two will be more soluble. Comparing the two;

A1B1 has a solubility or x-value = (10^-6)^(1/2) = 10^-3

A1B3 has a solubility or x-value = (10^-6)/(27)]^(1/4) = 10^-2

Thus A1B3 is more soluble.

 

[Econ2MD]

Maybe if his followup question had anything to do with the concepts 😉

Agreed. Just thought it was a little harsh, that's all.

 

[Insulinshock]

Why are you guys being such d*cks? Sorry not everyone is as smart as you, you don't have to treat the OP like a *****. Calculations don't mean **** unless you understand what its saying.

 

[loveoforganic]

solubility1 = (10^-6)^(1/2)
solubility2 = [(10^-6)/(27)]^(1/4)

followup question

Which is more soluble?

The only unanswered part to his followup question takes algebra I. Maybe you should drop a little bit of the condescension yourself and help the OP work through his problem describing what it is he's still confused about.

 

[rainashley]

I basically wanted to ask TWO questions

Which is more soluble: A1B1 with a Ksp of 10^-6 OR A1B3 with a Ksp of 10^-6? Why?


What do we know about a solution from its Ksp? What does the Ksp tell us exactly?

thanks

 

[loveoforganic]

Do you still have issues with your first question? What specifically is it you don't understand?

For your second question - AFAIK, ksp doesn't tell you a whole lot, unless you're comparing compounds that dissociate into an equal number of ions. You can use the ksp expression to solve for solubility however.

 

[rainashley]

OP, since solubility is a measure of the number of particles in solution, the greater x value between the two will be more soluble. Comparing the two;

A1B1 has a solubility or x-value = (10^-6)^(1/2) = 10^-3

A1B3 has a solubility or x-value = (10^-6)/(27)]^(1/4) = 10^-2

Thus A1B3 is more soluble.

What do the numbers mean though... Just because 10-2 is a bigger number... its more soluble? why?
So A1B3 is more soluble because its molarity is greater?
As molarity increases... solubility increases?

 

[RogueUnicorn]

🤣

 

[Eye Cue]

I hope this helps:

http://en.wikipedia.org/wiki/Solubility

 

[rainashley]

can you just answer my question?
thanks

 

[lDanny]

can you just answer my question?
thanks

really?

 

[rainashley]

yes

 

[disarticulate]

🤣

Do you have to make fun because you're a miserable reapplicant stuck in an SMP? Are you that insecure? pfff... 🤣

 

[disarticulate]

Ashley, first off, ignore the losers who waste their time and your time by posting ridicule. The psychological basis behind their actions is to combat insecurity by trying to convince themselves that they're intelligent. Similar to the reason why they play world of war craft all day to give themselves a sense of accomplishment, as it is absent in their real life.

Moving on... Remember that the solubility constant (Ksp) is a measurement of how well a substance dissolves in a specific amount of solvent. Since these two molecules have the same Ksp, yet one has more dissolvable components (A1B3), it must be more soluble. No need to do risky calculations as they waste your time on the test and can lead you down the wrong path.

All the best.

 

[loveoforganic]

oh lord

 

[seep]

Remember that the solubility constant (Ksp) is a measurement of how well a substance dissolves in a specific amount of solvent. Since these two molecules have the same Ksp, yet one has more dissolvable components (A1B3), it must be more soluble.

No offense to anyone here, but this question is immediately answerable using this line of reasoning.

 

[rainashley]

Ashley, first off, ignore the losers who waste their time and your time by posting ridicule. The psychological basis behind their actions is to combat insecurity by trying to convince themselves that they're intelligent. Similar to the reason why they play world of war craft all day to give themselves a sense of accomplishment, as it is absent in their real life.

Moving on... Remember that the solubility constant (Ksp) is a measurement of how well a substance dissolves in a specific amount of solvent. Since these two molecules have the same Ksp, yet one has more dissolvable components (A1B3), it must be more soluble. No need to do risky calculations as they waste your time on the test and can lead you down the wrong path.

All the best.

it took 2 weeks to finally get the reasonable right answer
i sincerely appreciate it

 

[RogueUnicorn]

Do you have to make fun because you're a miserable reapplicant stuck in an SMP? Are you that insecure? pfff... 🤣

🤣