Dissolving titanium metal/dioxide

Yesterday I went to lab and I was supposed to prepare titanium nitrate for synthesis. I said - no problem - we will just dissolve titanium dioxide in hot concentrated nitric acid. It failed. OK. Then we tried titanium metal. It only dissolved in hot concentrated hydrochloric acid. I thought that oxidizing chloride with HNO3 would replace anions. It worked partially and I got almost clear solution but on heating - titanium dioxide formed.

Any ideas how to prepared titanium nitrate?

Quote: Originally posted by clearly_not_atara

No titanium (IV) binary salts can be obtained from aqueous solution. The lattice enthalpy of TiO2 is much too strong. Anhydrous titanium nitrate is prepared by reacting titanium tetrachloride with dinitrogen pentoxide. It is a volatile, potentially explosive compound. Titanium (III) nitrate can be prepared in an aqueous solution by salt metathesis, but an inert atmosphere is ideal to prevent oxidation of Ti3+ by oxygen forming TiO2.

Quote: Originally posted by clearly_not_atara

Practically all Ti3+ salts are soluble. Even TiPO4 is soluble IIRC. So any salt can be used, but it must precipitate with the cation of nitrate. Titanium (III) sulfate is a strong contender, undergoing metathesis with calcium nitrate efficiently. If sulfate is also a problem, maybe better luck with titanium (III) bitartrate and potassium nitrate. Although I don't know how to make the bitartrate...

Thanks for another answer... I do not understand clearly your sentence i... it must precipitate with the cation of nitrate? That the product of reaction is the soluble nitrate of titanium and the other salt should be precipitated? If so, I see no problem in CaSO4 formation, I can filter insoluble salt... basically I need to get titanium ion in my Li-Fe-Ti nitrate-glycine oxide synthesis method (if you heard about it). But I dont know how to maintain titanium in Ti3+ state while evaporating water from the mixture. I will have toi take closer look on papers that have been published since date.

Quote: Originally posted by WangleSpong5000

Titanium dioxide is an adulterant in many hardware store HCl solutions. Fuck knows why... but yeah I spose it must be soluble in 30 + HCl

I might or might not be able to answer that, i will explain how i got the information, it may or may not matter but i am pretty sure it only applies to hardware type grade.

I have a new contact for some chemicals, they are a kind of waste center of sorts. recycle place might be a better description, they take large amounts of industrial used solvents and clean them up.

This is all part of the Scottish zero waste policy thing we have. Anyway I asked why this guys HCl was 1 very cheap, and 2 why was it sometimes pretty crap.

He said it depended on the source for it, he wouldnt say where but he mentioned a place in Newcastle that uses alot of metal. They often get a large amount of HCl off them thats been used as a metal pre wash, it comes in fairly clean compared to what they normally deal with.

They give it a quick clean up and bottle it up and sell on. I am the exception for them, they dont normally deal with the 5ltr guy. But I happen to know him and he dosnt live that far from me...

Only met him a couple of weeks ago, i didnt know the company existed! They called me thinking i was some SME that had started up in the area (my business), and tried selling me solvents by the tanker load!!!

Anyway we had a laugh on the phone and i now have a good source of extremely cheap and contaminated HCl .

Quote: Originally posted by NEMO-Chemistry

Quote: Originally posted by WangleSpong5000   Titanium dioxide is an adulterant in many hardware store HCl solutions. Fuck knows why... but yeah I spose it must be soluble in 30 + HCl I might or might not be able to answer that, i will explain how i got the information, it may or may not matter but i am pretty sure it only applies to hardware type grade. I have a new contact for some chemicals, they are a kind of waste center of sorts. recycle place might be a better description, they take large amounts of industrial used solvents and clean them up. This is all part of the Scottish zero waste policy thing we have. Anyway I asked why this guys HCl was 1 very cheap, and 2 why was it sometimes pretty crap. He said it depended on the source for it, he wouldnt say where but he mentioned a place in Newcastle that uses alot of metal. They often get a large amount of HCl off them thats been used as a metal pre wash, it comes in fairly clean compared to what they normally deal with. They give it a quick clean up and bottle it up and sell on. I am the exception for them, they dont normally deal with the 5ltr guy. But I happen to know him and he dosnt live that far from me... Only met him a couple of weeks ago, i didnt know the company existed! They called me thinking i was some SME that had started up in the area (my business), and tried selling me solvents by the tanker load!!! Anyway we had a laugh on the phone and i now have a good source of extremely cheap and contaminated HCl .