The Street > The Lounge
New Random Thoughts Thread
Prodigal Son:
I don't think the entirety of bg believes Carlos reads books.
Cole:
--- Quote from: Prodigal Son on December 12, 2015, 11:36:29 PM ---
--- Quote from: Cole on December 11, 2015, 02:45:49 AM ---
--- Quote from: Prodigal Son on December 10, 2015, 11:28:20 PM ---Ginger, after minimal reflection, it is my professional advice you try a super saturated NaCl and water solution to clean you water pipe.
--- End quote ---
I've never understood the "super saturated" thing. I use Cu(CuSo4) reference cells for work, and the CuSo4 we put into the halfcell needs to be super saturated. But really, how saturated can something get? You can only put in so much before it doesn't get dissolved by the water.
--- End quote ---
In the example you used, the CuSO4 is a ligand to the Cu. That's not an ionic or covalent type bonding. It's a complex ion most of the time. The CuSO4 groups around the Cu as much as possible.
In terms of a saturated solution you can alter it through thermodynamic changes. If you increase the energy to the system the solute will dissolve more as most solutions will become more soluble as heat increases. If you had it under an activation energy graph you could see the amplitude and relate that to how much of the solute is in solution.
This followed by rapid cooling to put it in a thermodynamic hole where the energy decrease is faster than it can precipitate out the system can have the same dissolved material at 25°c.
--- End quote ---
Thanks nerd. But that doesn't explain super saturated vs saturated.
Prodigal Son:
Saturation you can think of as the amount of whatever at equilibrium in a solvent. That solution can become super saturated by using the method I was just talking about. Solutes can be more soluble by temperature. If get as much of your chemical to dissolve at a temperature but expect it will go back to a state of equilibrium were the solution can only have so much of the solute at 25°c. Instead you do a rapid cooling to go past the energy value to precipitate out, the solute can stay in solution instead of being in saturation it would normally be at in standard conditions.
Cole:
Maybe I just don't know the actual definitions of either.
Prodigal Son:
Maybe this will help you visualize it.
Do you remember making rock candy? So you take your sugar (solute) and add it to boiling water (solvent). If you don't use boiling water, there is only so much sugar that will dissolve into solution. By boiling it, the solubility (how well it dissolves) increases. This greater solubility means there is a saturated solution at 100°c. As the solution cools slowly the crystals (precipitate) form large and classical crystal shape. Sometimes crystals won't form, this is what you would find as a super saturated solution in standard conditions.
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