I've been trying to work out how much H2O2 there is per gram of sodium percarbonate. Basically if I were to dissolve 1g into 10 or 100ml of water, what percent concentration of H2O2 would I have?
I've found the molecular weight of 2Na2CO3 * 3H@O@ is 313.96g or Na2CO3 * 1.5H2O2 156.98g. If the carbonate is anhydrous (which I would think it would have to be having the peroxide attached..??) it has a mass of 106g leaving 51g for the H2O2 at 32.5% of the molecular weight.
H2O2 has a molar mass of 34.0147 g/mol, IDK if that is needed or not. It has a density of 1.450 at 100% and decreases as the percentage to water decreases. 35% is 1.13g/ml and 3% is 1.0095g/ml.
If 1g NaCO3*1.5H2O2 is added to 99.5ml of H2O (the percarb is 2.1g/cc, so I subtracted /5ml or water) the .325g of H2O2 will dissolve into solution giving an unknown concentration. IDK if I'm making this too complicated or what.
100ml/.325 = .325% IDK if that gives the correct percentage of H2O2 so that is why I am asking.