Sciencemadness Discussion Board - Sulfamates

Sulfamates

samarium14 - 22-3-2021 at 05:38

Hi today i made copper sulfamate dihydrate. Also I will make Ni and Co sulfamates. It has beautiful deep blue colour. I used basic copper carbonate and sulfamic acid, next i evaporated solution.

[Edited on 22-3-2021 by vano]

[Edited on 22-3-2021 by vano]

itsallgoodjames - 22-3-2021 at 06:09

You should make chromium sulfamate

samarium14 - 22-3-2021 at 06:34

Quote: Originally posted by itsallgoodjames

You should make chromium sulfamate

Do you have? Or do you know colour?

itsallgoodjames - 22-3-2021 at 06:36

I have no clue about the color. Chromium tends to make nice colors though

samarium14 - 22-3-2021 at 07:05

I will make

Bedlasky - 22-3-2021 at 08:34

You read my mind, Vano

. I also plan to make copper amidosulfate

samarium14 - 22-3-2021 at 09:24

Oh its good

. Good luck in your plan. Today i made some copper salts, also CuSiO3.

[Edited on 22-3-2021 by vano]

DraconicAcid - 22-3-2021 at 10:25

Nice! The first time I tried making copper sulphamate, I accidentally heated it, so it hydrolyzed and the only precipitate I got was ammonium bisulphate.

WGTR - 22-3-2021 at 10:55

If you ever want to electroplate lead, its sulphamate is very water soluble. I have used a lead anode in sulphamic acid for this purpose. The color of that salt isn’t particularly interesting though.

samarium14 - 22-3-2021 at 11:09

Quote: Originally posted by DraconicAcid

Nice!

Thanks!

samarium14 - 22-3-2021 at 11:11

Quote: Originally posted by WGTR

If you ever want to electroplate lead, its sulphamate is very water soluble. I have used a lead anode in sulphamic acid for this purpose. The color of that salt isn’t particularly interesting though.

I have heard of nickel being actively used, but I have not heard of lead. thanks.

DraconicAcid - 22-3-2021 at 11:25

Quote: Originally posted by vano

Quote: Originally posted by DraconicAcid

Nice!

Thanks!

You're welcome! For a chemist should give all for another chemist's sake- he should give flask for flask- love as a road and a bridge!

samarium14 - 22-3-2021 at 12:04

Quote: Originally posted by DraconicAcid

Quote: Originally posted by vano

Quote: Originally posted by DraconicAcid

Nice!

Thanks!

You're welcome! For a chemist should give all for another chemist's sake- he should give flask for flask- love as a road and a bridge!

True words!

Lion850 - 22-3-2021 at 12:46

Nice blue Vano. Sulfamates are also on my list to make one day.

samarium14 - 22-3-2021 at 12:48

Quote: Originally posted by Lion850

Nice blue Vano. Sulfamates are also on my list to make one day.

Thanks. Good luck!

valeg96 - 23-3-2021 at 00:36

I made a bunch of sulfamates in the past. The Ni salt is extremely hygroscopic and you will get a viscous oil that takes a lot to dry. The Co salt gives a very hard crust. The Mn(II) salt is a dirty white solid.

samarium14 - 23-3-2021 at 01:06

Thanks for sharing your experience. Did you ever tried chromium salt?

samarium14 - 26-3-2021 at 23:22

Hi, today i made cobalt sulfamate hydrate, thats is why it has light pink colour. I made it from cobalt carbonate and sulfamic acid.

When the water evaporated from the solution to the end, it had exactly the same color as Valleg sulfamate, it was also really hard to crust. So I redissolved it in water, then heated it, when some of the water had evaporated and left a pink solid that looked wet, I removed the bottom of the flask and transferred it to its walls. After a few minutes it dried with the help of hot air and got a similar color, unfortunately I do not know the formula of hydrate.

It contains some anhydrous blue particles, i will be made better powder.

ChemTalk - 27-3-2021 at 07:11

Thanks Vano, that's a nice cobalt sulfamate
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ChemTalk
Standard Reduction Potentials

samarium14 - 27-3-2021 at 07:13

Quote: Originally posted by ChemTalk

Thanks Vano, that's a nice cobalt sulfamate
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ChemTalk
Standard Reduction Potentials

Thank you