Hello, I've hit a road block with this question and I'm hoping someone can point me in the right direction.
The problem states that a 5.30-g sample containing only Mn2(SO4)3(s) and Al2(SO4)3(s) is dissolved in aqueous solution. The metal ions are precipitated as hydroxides, which are pyrolyzed in air to produce 1.85 g of a mixture of Mn2O3(s) and Al2O3(s). What was the percent Mn in the original sample?
I've designated x = mass of Mn2O3 and with that, I found that the moles of Mn would be = 2x/157.87
What is the next step? Or, am I completely mistaken?
Thx in advance