Muhammad Zarrar Khan

I believe using SnCl2.2H2O should be fine for your case, as your ammonia hydroxide solution should contain water. The color change after heating might be due to thermal decomposition of tin oxyhydroxide. Please refer to this paper to see if it might be helpful:

Article Thermal Decomposition of Tin(II) Oxyhydroxide and Subsequent...

Thanks for your kind response @Tianyu Liu

Actually i had a batch of anhydrous SnCl2 and it was just lying there.I thought i should use it for some research purpose.My aim is to add CNTs and then coat the whole thing with conductive polymer for electrochemical measurements.So i can use only anhydrous SnCl2.I,ll characterize them via Xrd+FTIR to see if its working or not. Will share the results.

Just in case you are still interested in this: In my opinion it doesn't make a difference if you use anhydrous or SnCl2 or the dihydrate, because you dissolve the precursors in water anyway. It might just be necessary to adjust the stoichiometry, i.e. the amount of the respective tin(II) precursor. The fact the the initially white solid turns black is indicative for the formation of the desired tin(II) oxide.

Frank T. Edelmann

Yes , it didnt matter .. i successfully synthesized via adjusting the stoichiometery accordingly.Actually i am working on the synthesis of ternary TinOxide/MWCNTs/Conductive Polymer (PANI,PTh,PPy etc) to study their cyclic voltametery .The literature showed every one using hydrous rather than anhydrous precursor of tin chloride.

Thanks for your response ..

Cheers :)