URGENT: Solubility of KCl, KBr and Saturation Point

M.A.H

Im stuck on this Q:

From the graph I can see that KBr is more soluble than KCl, so how does that answer the Q of which crystals will form when its cooled?

(The MS said its KBr)

Also am i rigth in assuming that the saturation point say for water depends on the solute being dissolved?

Because my friend said that the saturation point of a solvent is the same for ANY solute.

Thanks

Reply 1

icapturethecastle

this is a complete guess...

is it anything to do with bond lengths?
longer bond, therefore weaker, and so more soluble :s-smilie:

is this unit 3 (edexcel)?

i am not good at chemistry...

Reply 2

M.A.H

tami*

this is a complete guess...

is it anything to do with bond lengths?
longer bond, therefore weaker, and so more soluble :s-smilie:

is this unit 3 (edexcel)?

i am not good at chemistry...

Erm KBr would have a longer bond length coz Cl is mroe elctronegative than Br, but dont see how thats affects which crystallizes first. :s-smilie:

Its U2 Edexcel (Nuffield) :mad:

Reply 3

icapturethecastle

i'm completely clueless then...
i don't even know about the crystallisation thing...i don't think i've done it

if i have i'm screwed cos my chemistry exams on thursday...eeek!!

Reply 4

charco

Study Forum Helper

There are NO bond lengths involved because they are ionic salts.

Use the graph to find the solubility at a given temperature. If the temperature is lowered then use the graph again to see the solubility at the new temperature. If the two solutions are saturated then the difference will be the mass deposited