Teen Chemist
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Strontium chloride
I recently bought some strontium chloride for flame test purposes and I want to know some other uses for it.
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Adas
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Eat it  I heard it is good for your bones - it makes them harder (I wouldn't
eat it, though)
Rest In Pieces!
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Hexavalent
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You could have a go at making some other strontium compounds from it, such as the nitrate, sulfate, other halides, oxide, etc. and maybe look into
what kind of organic compounds you could make from it.
"Success is going from failure to failure without loss of enthusiasm." Winston Churchill
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Teen Chemist
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Thanks for the sugestions
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Polverone
Now celebrating 21 years of madness
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Thread Moved
28-4-2012 at 15:42 |
Hexavalent
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What have you decided to do with your SrCl2?
You could also try and find a way to make strontium metal from it . . .that'd be cool
"Success is going from failure to failure without loss of enthusiasm." Winston Churchill
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Teen Chemist
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Quote: Originally posted by Hexavalent  | What have you decided to do with your SrCl2?
You could also try and find a way to make strontium metal from it . . .that'd be cool |
Nothing yet but i will look into some of these things.
Maybe I could make some toothpaste.
[Edited on 29-4-2012 by Teen Chemist]
[Edited on 29-4-2012 by Teen Chemist]
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Teen Chemist
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I read that you could take an aqueous solution of strontium chloride and an aqueous solution of copper sulfate and mix them to get a precipitate of
strontium sulfate and an aqueous solution of copper chloride. Is that correct.
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Hexavalent
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I can't see why not - it would simply be a double-displacement reaction. All the other Group II sulfates are almost insoluble, so I fail to see a
reason why Sr would be any different.
You would get; [Cu2+](aq) + [SO42-](aq) + [Sr2+](aq) + 2[Cl-](aq) ------> SrSO4 (s) + [Cu2+](aq) + 2[Cl-](aq)
Just mix stoichiometric amounts of the reagents dissolved in water, filter off the SrSO4 and wash several times with cold water to purify it. Allow it
to dry and you should have some nice strontium sulfate.
Another idea I've just thought of is for pyrotechnics . . .are you into that kinda stuff? Sr gives a reall nice red colour IIRC when included in such
mixtures.
P.S. Please use the 'edit' feature on the top right hand of your post to include extra information, as opposed to posting twice sequentially.
[Edited on 29-4-2012 by Hexavalent]
"Success is going from failure to failure without loss of enthusiasm." Winston Churchill
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Teen Chemist
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I have used it to color the flame in a potassium nitrate sugar mix
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Hexavalent
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Nice, perhaps you could use what you learnt from that and what you gan gather on the internet and in books to devise a thermite composition or similar
to try and obtain strontium . . .I've never really heard of anyone doing that before.
"Success is going from failure to failure without loss of enthusiasm." Winston Churchill
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Teen Chemist
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That would be interesting. I wonder if I would have to convert it to an oxide first.
I just reacted a solution of strontium chloride and one of copper sulfate to get a precipitate of strontium sulfate.
[Edited on 29-4-2012 by Teen Chemist]
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Hexavalent
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Nice, what mole scale did you run the reaction at?
"Success is going from failure to failure without loss of enthusiasm." Winston Churchill
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Teen Chemist
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Im sad to say i dont know i havent learned to calculate that yet but i have been looking into it
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barley81
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Make some strontium nitrate and use it in pyrotechnic compositions! I haven't done this, but the nitrate is frequently used in pyrotechnics (for
coloring the flame red).
Strontium salts and barium salts are useful for replacing the sulfate ion with another ion. For example, chloric acid can be prepared by reacting
barium chlorate with sulfuric acid.
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Hexavalent
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Kinda mentioned that upthread . . .
TeenChemist, did you weigh out your reagents or just use a few spoonfulls of this and a bit of that?
"Success is going from failure to failure without loss of enthusiasm." Winston Churchill
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barley81
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D'oh. Thanks for pointing that out.
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Teen Chemist
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I used 5 grams of each in 50 mls of water each.
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Hexavalent
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That's a good start, but remember - just because one *part* CuSO4 reacts with one *part* SrCl2, it doesn't mean that requires equal GRAM quantities of
each. It's the moles that count, and here's how to calculate it;
1. Look at how many moles you need for the reaction. Here, 1 mole of CuSO4 and 1 mole of SrCl2 are needed.
2. Look up the formula masses/weights/Mr for each compound.
3. Multiply the mole amounts you require by the formula weight. This is one mole of that compound in grams.
4. If this number gives, say, 245g and you don't want to use that much chemical, you can do a half-mole reaction (245/2 = 122.5g), a tenth mole
reaction (245/10=24.5g) etc.
Let's look at another example; 2AgNO3 + CaCl2 ---> 2AgCl + Ca(NO3)2
SILVER NITRATE
1. Here, two moles of silver nitrate are needed per mole of calcium chloride.
This means that, saying we want to run a 1/2 mole reaction, we need;
2. Formula weight of Silver Nitrate = 169.87g/mol, x2=339.74
3. 339.74/2 = 169.87
Calcium chloride, anhydrous
1. 1 mole of CaCl2 is needed per two moles of AgNO3.
2. Formula weight of CaCl2 = 110.98g/mol, *1= 110.98
3. 110.98/2 = 55.49g
***
So, to run the above reaction at 1/2 mole scale, you would need to use 169.87g of silver nitrate and 55.49g of anhydrous calcium chloride.
[Edited on 30-4-2012 by Hexavalent]
"Success is going from failure to failure without loss of enthusiasm." Winston Churchill
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Eddygp
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Reducing the strontium chloride with sodium? (Maybe the sodium should be liquid in order to react...)
SrCl2 + 2Na = 2NaCl + Sr
Seems a possible choice.
there may be bugs in gfind
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Teen Chemist
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Hexavalent I will try to do that next time. Could you contact me via U2U so I could learn more about calculating these things.
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Hexavalent
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U2U'd you, always happy to help another amateur scientist wherever I can
[Edited on 30-4-2012 by Hexavalent]
"Success is going from failure to failure without loss of enthusiasm." Winston Churchill
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MrHomeScientist
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Some time ago I wanted to try the thermite method of producing strontium metal, but never got very far. The idea was to take SrCO3, heat it
to decompose it to SrO, then 'thermite' that with aluminum powder. I don't think I ever got it hot enough to become the oxide, though. Wikipedia cites
its decomposition temperature as 1494C.
The reduction with sodium mentioned above also sounds interesting (and potentially dangerous). Can anyone elaborate on the conditions you'd need for
such a reaction?
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