Hi all, could someone that knows help me out please....I am wanting to make
some Strontium Sulphate, and I read that I can use Potassium Sulphate and Sr
Nitrate?  What would be be the best concentrations of solutions to use if
the goal was 100 gms of the Strontium Sulphate.  Would I be correct in
thinking that the reulting solution after precipitation of the Sr sulphate
would be potassium nitrate? How do I make sure that I am not wasting any of
my starting reagents??

On Sep 6, 10:43 pm, "Jane" <jan... at (no spam) bigpond.net.au> wrote:

Hi all, could someone that knows help me out please....I am wanting to make
some Strontium Sulphate, and I read that I can use Potassium Sulphate and Sr
Nitrate? What would be be the best concentrations of solutions to use if
the goal was 100 gms of the Strontium Sulphate. Would I be correct in
thinking that the reulting solution after precipitation of the Sr sulphate
would be potassium nitrate? How do I make sure that I am not wasting any of
my starting reagents??

Without looking up solubilities, I'll just remark generally something
you may already know. Usually in a situation like this one reagent is
expendable and would be used in excess to avoid wasting another. In
this case you may have to use an excess of K2SO4 to maximize recovery
of SrSO4 without wasting Sr(NO3)2, and don't try to recover KNO3.

If, however, SrSO4 is for practical purposes insoluble,

shoot for a stoichiometric ratio of the starting materials.

Bob wrote:
On Sep 6, 10:43 pm, "Jane" <jan... at (no spam) bigpond.net.au> wrote:

Hi all, could someone that knows help me out please....I am wanting to make
some Strontium Sulphate, and I read that I can use Potassium Sulphate and Sr
Nitrate?  What would be be the best concentrations of solutions to use if
the goal was 100 gms of the Strontium Sulphate.  Would I be correct in
thinking that the reulting solution after precipitation of the Sr sulphate
would be potassium nitrate? How do I make sure that I am not wasting any of
my starting reagents??

Without looking up solubilities, I'll just remark generally something
you may already know.  Usually in a situation like this one reagent is
expendable and would be used in excess to avoid wasting another.  In
this case you may have to use an excess of K2SO4 to maximize recovery
of SrSO4 without wasting Sr(NO3)2, and don't try to recover KNO3.

If, however, SrSO4 is for practical purposes insoluble,

It is, highly insoluble. Which makes this an easy one to do -

Dissolve both separately in water, filter, mix the solutions, filter,
wash filtrand with purified water, dry in oven - that's it.

The first filtrations removes any insoluble impurities, the last any
soluble impurities (which don't react to form solid products).

I made a couple of pounds of strontium carbonate in an almost identical
reaction last week, took about 15 minutes, apart from drying time.

then you would

shoot for a stoichiometric ratio of the starting materials.

Indeed.

If you want this for pyro purposes then just be sure to use pyro grade
ingredients, otherwise you may get traces of sodium salts, which will
make the flame yellow.

-- Peter Fairbrother