Hey guys whats up?
I have been a long time lurker and I'm sorry for not joining years ago to contribute to this great community! I don't really join forums much....
Anyway here I am. The main reason I joined is to add to the conversations going on in the STB section about the adding of salts and Ionic strengths of the Aquarius solutions. I have a back ground in chemistry and wanted to add me 0.02c. As I am a new member I cant post in the extractions forum yet. Firstly ChemisTryptaMan is a genius for thinking of it. I probably never would have. Secondly he is right (obviously) with the salt thing the more ionic the solution the more "push" it has against the non polar molecules.
NaCl is great, everyone has it and it works well. The thing is, is it the best?? Maybe.. I did some thinking over the past day on the subject and this is what I came up with.
This was my thought process as it went along
I thought about trying Na2CO3 as the CO3 is minus 2 charge. It should work well... I'm not sure if it will work as well as salt though as it doesn't completely ionize like NaCl does. If Na2CO3 ionizes > 50% in water than it should be more effective (at total negative ionization) than NaCl at equal solubility.... Of course solubility comes into play! I was thinking probably a mixture of the two in some kind of ratio would yield better results than just either on their own...
Enter Na3PO4 (Trisodium Phosphate) as the PO4 has a charge of -3.
When this came into my head I had thought I hit the joke pot. Not only is it a strong base (fully ionizes) but it has minus three charges!! Then I checked it solubility.. Only 88grams per liter.
Then I hit myself in the face because I had totally forgotten about moles...and it gets even worse when you actually check the amount of moles possible to dissolve in solutions...
Solubility are
NaCl - 359g/L = 6.143mol/L
Na2CO3 - 215g/L = 2.023mol/L
*2 for the charge = 4.046mol/L worth of NaCl (But it doesn't fully ionize)
Na3PO4 - 88g/L = 0.53mol/L
*3 for the charge = 1.59mol/L
So even though the last 2 have double and triple charges you can't physically get them into the water as well.
Conclusion
Salt would seem to be the best bet so far. I'm not counting out other things as of yet. Simply basing H2SO4 or H3PO4 with NaOH should yield good results. As the H will just bond to the OH making more water therefore making the SO4/PO4 ions even more soluble.... Might get a massive excess of Na cations though... Needs more thinking and definitely needs more experimenting!
Anyway I have always loved these forums and I am glad I have finally decided to join.
(Sorry if this is the COMPLETE wrong place to write all this it's just I have been thinking about it non stop for 2 days and had to get it out of my brain)
I have been a long time lurker and I'm sorry for not joining years ago to contribute to this great community! I don't really join forums much....
Anyway here I am. The main reason I joined is to add to the conversations going on in the STB section about the adding of salts and Ionic strengths of the Aquarius solutions. I have a back ground in chemistry and wanted to add me 0.02c. As I am a new member I cant post in the extractions forum yet. Firstly ChemisTryptaMan is a genius for thinking of it. I probably never would have. Secondly he is right (obviously) with the salt thing the more ionic the solution the more "push" it has against the non polar molecules.
NaCl is great, everyone has it and it works well. The thing is, is it the best?? Maybe.. I did some thinking over the past day on the subject and this is what I came up with.
This was my thought process as it went along
I thought about trying Na2CO3 as the CO3 is minus 2 charge. It should work well... I'm not sure if it will work as well as salt though as it doesn't completely ionize like NaCl does. If Na2CO3 ionizes > 50% in water than it should be more effective (at total negative ionization) than NaCl at equal solubility.... Of course solubility comes into play! I was thinking probably a mixture of the two in some kind of ratio would yield better results than just either on their own...
Enter Na3PO4 (Trisodium Phosphate) as the PO4 has a charge of -3.
When this came into my head I had thought I hit the joke pot. Not only is it a strong base (fully ionizes) but it has minus three charges!! Then I checked it solubility.. Only 88grams per liter.
Then I hit myself in the face because I had totally forgotten about moles...and it gets even worse when you actually check the amount of moles possible to dissolve in solutions...
Solubility are
NaCl - 359g/L = 6.143mol/L
Na2CO3 - 215g/L = 2.023mol/L
*2 for the charge = 4.046mol/L worth of NaCl (But it doesn't fully ionize)
Na3PO4 - 88g/L = 0.53mol/L
*3 for the charge = 1.59mol/L
So even though the last 2 have double and triple charges you can't physically get them into the water as well.
Conclusion
Salt would seem to be the best bet so far. I'm not counting out other things as of yet. Simply basing H2SO4 or H3PO4 with NaOH should yield good results. As the H will just bond to the OH making more water therefore making the SO4/PO4 ions even more soluble.... Might get a massive excess of Na cations though... Needs more thinking and definitely needs more experimenting!
Anyway I have always loved these forums and I am glad I have finally decided to join.
(Sorry if this is the COMPLETE wrong place to write all this it's just I have been thinking about it non stop for 2 days and had to get it out of my brain)