The new design of chemspider is horrrrrrible....

omg, it's back chemistry.stackexchange.com/questions/32015/…

What's this all of a sudden now

not a clue, it's cros posted on ELL - really do not know what's going on with this guy.

If it is him, it is almost as if he is trying to make out that someone else is targetting him

That's a possibility

it's certainly not me, or anyone of us

Hopefully mods will sort this mess out again

yup, have flagged and are walking away from it (again)

Let's all be Rilakkumas here...

Egg's act Lee!

ʕっ•ᴥ•ʔっ

( ͡° ͜ʖ ͡°)

That's no Rirakkuma!

　　　　　　　　　　　　　　,. ―‐ ､　　　　　　　　　,. ―‐　､
　　　　　　　 　 　 　 　 /　　　 　ヽ. -―――‐-'　　　　　ヽ
　　　　 　 　 　 　 　 ／￣｀ヽ　　´　　 　 　 　 　 ｀ 　 ／￣｀ヽ
　　　　　　　　　 　　{　/⌒)　}　 ／￣￣￣￣￣＼　 {　(⌒'.　}
　　　　　　　　　　　 ,ゝヽ＿ノ　/　　　 　 　 　 　 　 '　ヽ.＿ﾉ く
　　　 　 　 　 　 　 / 　　 /　 /　　　　　　　　　 　 　 ',　ヽ.　　 ヽ
　　　　　　　　　　 ヽ.＿,ｲ 　 ｉ　　●　　　　　　● 　　i 　 ｉヽ＿_ﾉ
　　　　　　　　　　　　 　 !　　|　　　　　 ●　　　　　　 l 　 |
　　　　　　　　　　　　　　',　　ヽ 　　　　人　　　 　　 /　 /
　　　　　　 　　　　　 　 　ヽ 　　`ー―――――一'´　　＼＿＿__
.　　　　　　　 　 　 　 　 ／　　　　　　（　　）　　　　 (＾ヽ'"´ ヽ　 　 ｀ヽ
　　　　　　　　 　 　 　 （＿__,.ィ 　 　　　　　 　 　 ／　　ｌ　ｌ　 ｉ　　 　　i

Okay then, that works

Is anyone over here keen about moderator elections?

No one :/

It'll happen when it happens.

@LordStryker A question on solubility of salts. Can I ask?

Go for it

@LordStryker Is there a way of comparing which salt is more soluble between Hg2Cl2 and Cr2(SO4)3 without knowing their Ksp's?

Well lets see. Is the chromium complex anhydrous?

@LordStryker complex?

Cr3+(xH2O) type of complex?

well it isn't a molecule so I called it a complex.

Something like that

Its chromium sulphate in crystal form. So, ya... anhydrous.

Okay so I'm not exactly sure how to go about comparing relative solubilities here but I would take a gander that one could consider the intermolecular interactions that would be taking place for these types of salts.

Something like comparing lattice and hydration energy relatively

Perhaps

I hate saying this sometimes but I really don't know the answer to your question at the moment.

You could look these things up in solubility tables I suppose (no Ksp's needed there) but I assume that isn't the kind of answer you're looking for.

You could try and make solutions of these things yourself and compare relative solubilities that way but again I don't think that is the answer you're looking for.

I think the answer to my original question is : NO

Well it may not be.

There's no real reliable way to compare solubilities just by looking at the formulas, I'm pretty sure

Since the carions and anions are different.

@NicolauSakerNeto So the only reliable way to compare relative solubilities of salts (in non extreme cases) is experiment?

@NicolauSakerNeto formulas and relative size of the ions. But even that info wont help.

User, it might help but it's not reliable, especially not quantitatively, and if you're looking up data, why not look up the Ksp in the first place!

@NicolauSakerNeto No. I am not looking up any data.

LordStryker, I'm not sure if there's any other way to do it

As far as I understand solvation is an extremely difficult problem even with molecular modelling methods

So I don't really see how some sort of qualitative extrapolation can have a good chance except in some relatively trivial cases

Of course some ions have a tendency to make more soluble or more insoluble salts, but quantification of this may be quite difficult

And this question doesn't look fit for the main site too.

Solvation certainly is a problem to model but I don't think that necessarily translates into predicting the solubility of something.

But I think it makes for a good question @user223679

@NicolauSakerNeto Can you give some examples of those ions?

Too broad? @LordStryker

The solubility of anything would be dependent on the strength of the solvent-solute interactions minus the solute-solute interactions

Solute-solute is easier assuming a perfect crystal

I don't see how it would be too broad. The question directly focuses on an alternative process for determining relative solubilities if Ksps were not available.

Solvent-solute is hard

Of course you may want to state that conducting the experiment or looking these things up in tables is not really what you are looking for as an answer.

And what examples of ions do you mean, User?

this probably

Well, I mean if you were to compare, say Ca^{2+} to Hg^{2+}, you'd expect the calcium salts to be generally more soluble than the mercury salts

Though that is a very extreme comparison, which makes it comparatively simple

If you were to ask between Fe^{3+} and Cr^{3+}, it would pretty much be guesswork

@NicolauSakerNeto Whats the logic behind this?

If you look at several calcium and mercury salts on a Ksp table, you'll find that mercury salts tend to be more insoluble

If you want to take a large Ksp table and calculate the solubilities for each ion, go ahead, that could be quite an interesting job

Probably not too hard with a spreadsheet program

Great, now I'm doing it myself

Damned curiosity

har

Can someone suggest me a good title for this question?

Is there a way of comparing which salt is more soluble without knowing their Ksp data or performing experiments? this looks too long.

@NicolauSakerNeto Haha

"Determining relative solubilities of salts without Ksp values?"

or "predicting" may be more precise

@LordStryker should I add that I cant experiment in the title? Or in the body?

"Predicting relative solubilites of salts without Ksp values?" - In the body of your question make clear that you are aware of experimental based procedures but you are curious to know if any (semi-)reliable methods exist to predict these types of things.

Done. Hope you all don't mind if the question is linked to this chat.

@NicolauSakerNeto @LordStryker @Gowtham Any corrections?

Looks fine to me

hello!

@Apoorv Hello

Great, I was supposed to rest and get some things done, and now I've been crunching numbers and plotting graphs for an hour

I am a slave to my curiosity

@NicolauSakerNeto like a true scientist

Like an addict!

Hah now my rep is 6626, Planck's constant yay!

First pople's split valence basis now Planck's constant. humph showoff.

:P

Maybe I should go into numerology, Eddington's got nothing on me

This is very good - the member mentioned from before has written a good homework question and there has been a constructive comment discussion, good to see him participate properly chemistry.stackexchange.com/questions/32029/…

Yeah that turned out a lot better