Re: Alternative sources for isotopes
AdeebR wrote:Hi Jahangir,
Most lanthanide salts are pretty water soluble. I've typically dissolved lanthanide salts in either H20 or 0.01M HCL to prepare a 2M stock solution, and then dilute this to 50mM working solution in L buffer.
Adeeb
Hi Adeeb et al.,
Sorry to bother you with this but I was just thinking of what you wrote above and I have a few questions.
I intend to order 100mg of the following metals from Trace Sciences:
- 113-InCl3
- 115-InCl3
- 157-GdCl3.6H2O
Now, my questions are, why do you make specifically a 2M stock solution? I mean, why not 3M or 1M or even 500mM? Is there an optimal concentration at which your stock solutions should be? And do you know what the shelf-life is for those stock solutions?
Also, would it not be better to use the 0.01M HCl solution rather than the dH2O? As this would prevent the formation of metal oxides? Also, does the pH increase (i.e. become more alkaline) over time? Would 0.01M HNO3 also do the job?
Lastly, with all those metals that I intend to purchase above, to make a 2M stock solution of, lets say, the 157-GdCl3.6H2O, I would need to add the entire 100mg of the metal into approximately 135ul (microlitres) of 0.01M HCl or HNO3 solution. Can I just confirm if my maths is correct? (knowing that I'm going to look like an idiot for even asking such a basic question) but the reason I ask is to confirm if it's actually possible to dissolve such a (relatively) large amount of metal into such a (relatively) small amount of solution?
Many many thanks for help and looking forward to your response!
Jahangir