Can someone help me with the preparation if this complex. I found few threads here which are pretty old. I saw a post in woelen's site. I wish I could
know the stoichiometry of how much of Cscl and CuCl to use?
Hoping you guys would help.. I will definetly be performing this as a video in my channel . Thanks in advanceMaurice VD 37 - 16-9-2021 at 06:28
Don't use CuCl ! You should start from CuCl2 !!
What do you want to do with this compound ? Cesium compounds are rather expensive.vibbzlab - 16-9-2021 at 07:56
I just wanted to make this compound just to see that vibrant colors. I already have around 25 g of cesium carbonate with me. And I have Copper II
Chloride too . Can you help me outfredsci93 - 16-9-2021 at 13:04
The potassium salt is prepared by slow evaporation of 2mol potassium chloride to 1mol copper chloride in water, I figure that should work for the
cesium salt as well.Bedlasky - 16-9-2021 at 14:23
I just wanted to make this compound just to see that vibrant colors. I already have around 25 g of cesium carbonate with me. And I have Copper II
Chloride too . Can you help me out
Convert the carbonate to CsCl by adding HCl. Evaporate to a small volume, no need to make dry CsCl. Next, follow the instructions on my page, taking
into account that you have a solution of CsCl instead of the solid.
The reaction is not critical at all, you really should get some of the complex salt. it is important though that you use concentrated HCl. With dilute
HCl it will not work and then you just get green solutions.vibbzlab - 17-9-2021 at 03:14
Is there any mole ratio or stoichiometry to how much Cs salt required and The Copper Chloride. woelen - 17-9-2021 at 04:12
It is very simple. Just drop solution of CuCl2 in conc. HCl into a concentrated solution of CsCl and observe the formation of the yellow and red
complexes. If you start with two concentrated solutions, then the experiment simply cannot fail.
If you really want to be precise, then you can compute the mole ratio of CuCl2 and CsCl easily. These complexes simply are additions of CuCl2 and
CsCl, no redox, no exchange with other compounds.vibbzlab - 17-9-2021 at 04:24
Thanks woelen. I will definitely do the work and post in my channel. I'll definitely credit you in the video as well Bezaleel - 22-9-2021 at 12:53
vibbzlab, I would really find it a pity if you would use your Cs2CO3 to make CsCl. Cs-carbonate is usually much more expensive and much harder to get
than Cs-chloride, so I would by some CsCl and work from there.
The carbonate is the ideal starting point if you want to make Cs salts with less common anions, so my advice would be to keep it for such reactions.vibbzlab - 23-9-2021 at 22:54
Thanks in advance