dale_wilson69
Harmless
Posts: 12
Registered: 1-12-2007
Member Is Offline
Mood: No Mood
|
|
Copper in grams per liter
I do not have the equipment to test the amount of copper in grams per liter. Can anyone tell me from experience approx. how much copper is in my
solution in grams per liter? See image posted
Can anyone email me a pictures of what H2SO4 leached solution looks like with 40 gpl (grams per liter) of copper.
Thanks
Dale
dale_wilson69@hotmail.com
|
|
|
evil_lurker
National Hazard
Posts: 767
Registered: 12-3-2005
Location: United States of Elbonia
Member Is Offline
Mood: On the wagon again.
|
|
Dump solution out of flask. Dry and weigh empty flask. Fill up flask back to the ring with solution. Weigh flask again, subract the weight of the
flask from the total weight of flask+solution. This gives the total weight for 100mls of solution.
Now subtract another 100g from that weight (100ml of water weighs in at 100g or so depending on temp). The remainder should give you a rough idea of
how much copper sulfate is in 100mls of solution (provided most of the H2SO4 has reacted).
To calculate grams of copper in solution, take the total molar weight copper sulfate and figure what percent per mole is copper, then multiply that by
the grams of copper sulfate in solution.
Another possible way would might be to add a non-soap coated brillo type scrubbie to 100mls of solution and precipitate all the copper out, filter and
weigh.
Not all chemicals are bad. Without chemicals such as hydrogen and oxygen, for example, there would be no way to make water, a vital ingredient in
beer.
|
|
|
12AX7
Post Harlot
Posts: 4803
Registered: 8-3-2005
Location: oscillating
Member Is Offline
Mood: informative
|
|
Damnit Jim, I'm a doctor, not a spectrophotometer! 
I would guess somewhere under 0.2M. Why don't you, oh Idunno, test it? They make spectrophotometers for this.
Tim
|
|
|
not_important
International Hazard
Posts: 3873
Registered: 21-7-2006
Member Is Offline
Mood: No Mood
|
|
Photographs are not very reliable ways of matching colours and intensities. Too much depends on the lighting used and the film + scanner or CCD in
digital cameras.
Is sulfate the only anion in the solution? Are there other coloured cations?
If copper is the only strongly coloured cation, and sulfate the only anion except for traces of others, then there is a simple procedure to determine
the concentration of copper.
You need two long transparent tubes. Test tubes will work if long enough or the solution is concentrated enough, plastic tubes will work because your
solution does sound particularly reactive.
Make up a solution with a known concentration of CuSO4, better if it's in about the same concentration of acid. Also better if it is within a factor
of 3 or 4 of the concentration of the solution you want to gage - a simple "eyeballing" of a small amount of water and CuSO4 will get you within that
range.
Set up the tubes in the vertical position, with an diffused white light source under them; a piece of white paper lit with a strong light works well.
Wrap paper or foil around the outsides of the tubes, leaving just the bottom and opening at top uncovered (keeping out side illumination)
Add whichever solution seems the most concentrated to one tube, filling it 1/5 to 1/4 of the way. Now add the more dilute solution to the other tube,
looking down into both tubes to compare the tint and brightness of transmitted light, until they look the same. If the fuller tube is much less that
3/4 full, add more of the concentrated solution to its tube and continue adding the more dilute solution to its tube until the match again. Stop when
the fuller tube is roughly 75 to 90 percent full.
Measure the depth of solution in both tubes by removing the wrappings and using a ruler. The ration of the fluid levels and the concentration of the
known solution will let you calculate the unknown's concentration to 5% or better.
This works for compounds that do not change too much in amount of ionization or complex formation as you change the concentration.
|
|
|
chemoleo
Biochemicus Energeticus
Posts: 3005
Registered: 23-7-2003
Location: England Germany
Member Is Offline
Mood: crystalline
|
|
Take i.e. 10 ml of that, and heat in a beaker to dryness, then roast it in a crucible of known weight under a flame until it turns all white
(anhydrous CuSO4). Weigh the crucible again. There you have your concentration, i.e. 0.5 g/10 ml, or 50g/l or x mole/l.
Never Stop to Begin, and Never Begin to Stop...
Tolerance is good. But not with the intolerant! (Wilhelm Busch)
|
|
|
chloric1
International Hazard
Posts: 1147
Registered: 8-10-2003
Location: GroupVII of the periodic table
Member Is Offline
Mood: Stoichiometrically Balanced
|
|
| Quote: | Originally posted by 12AX7
Damnit Jim, I'm a doctor, not a spectrophotometer!
Tim |
Tim you so silly!
When you figure that one out I got some nickel nitrate solution I forgot to measure out the dissolved solids. I will post a picture of that tomorrow
if anyone wants to take a guess.
Fellow molecular manipulator
|
|
|
not_important
International Hazard
Posts: 3873
Registered: 21-7-2006
Member Is Offline
Mood: No Mood
|
|
| Quote: |
Take i.e. 10 ml of that, and heat in a beaker to dryness, then roast it in a crucible of known weight under a flame until it turns all white
(anhydrous CuSO4). Weigh the crucible again. There you have your concentration, i.e. 0.5 g/10 ml, or 50g/l or x mole/l. |
Works if it's only copper sulfate in the solution, and there's not too much free sulphuric acid. As it was called "H2SO4 leached solution", and the
previous thread dealt with extracting metals from a complex mix of metals concentrates, I'd not bet on it being clean CuO4 until told otherwise.
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
