[Spectrum]

Al + 3KOH + H₂O + 3C₂H₂O₄.H₂O --> K₃[Al(C₂O₄)₃].H₂O + 4.5H₂ + 5H₂O


Hmmm, that's what I get when I balance it.

[Borek]

What gas is produced when dissolving Al in strong base? Move water to products as well - although what will really happen depends on the crystallic form of your product.

[Spectrum]

Al + 3KOH + H₂O + 3C₂H₂O₄.H₂O --> K₃[Al(C₂O₄)₃].H₂O + 4.5H₂ + 5H₂O


Hmmm, that's what I get when I balance it.

[Borek]

4.5H₂?

Water on both sides? Some coefficients are OK, but in general equation is still not balanced.

[Spectrum]

After working on this a bit today and yesterday. I have come up with K₃[Al(C₂O₄)₃] as my product that I made.

Now, after I made this product. I took some of it and dissovled it in dilute sulphuric acid (50cm³) and then 100cm3 of water. I then titrated it with potassium permanganate (0.01979mol l-1)

The only problem I have now is that I don't understand how this helps me to find the %ethanedioate in my product and then elps me estimate a value for x in the formula for the complex, K₃[Al(C₂O₄)₃] xH₂O

[Borek]

Titration should give information about number of moles - as you have (hopefully) weigthed your sample before titration, you know mass and number of moles - that gives molar mass. And molar mass is a simple function of x.

[Spectrum]

So if I had 0.1504g of product and that took around 21cm3 to titrate.

So number of moles = 0.01979 x 21cm3 = 0.0004moles

That would mean a molar mass = 0.1504/0.0004 = 361.895.

So if the Mr of my product is 411.3348. I then subtract them to get 50. then if i divide this by the mr of water, which is roughly 18, i get 2.78, which is closer to 3 i guess, so the number for X, is 3?

[Borek]

Reasoning seems to be correct.

But then, without knowing your numbers, experimental procedure, blah blah and blah blah, you can be wrong. I can't tell, I just don't know enough.