How to make 2 moles of a 35% by weight hydrogen peroxide solution from 30% hydrogen peroxide solution?
If the procedure asks for 2 mole of H2O2. Then can we calculate the weight of that much amount of H2O2 from any % solution of H2O2 or do we strictly need to use the same weight %.
Your quetion is not clear. However, one mole (i.e. Avagadro number) of any molecule will be present in its molecular weight (in grams). For instance molecular weight of hydrogen peroxide is 34 and hence 34 g of hydrogen peroxide will contain one mole.
Moreover, you can not prepare 35% solution from 30% solution (until and unless you look for a means to concentrate it, which to the best of my knowledge will be tough for hydrogen peroxide). You seem to have typed wrongly.
Please calculate molarity of commercial hydrogen peroxided solution you are using (the bottle must be having information about specific gravity besides molecular weight and percentage).
Exactly. The usual methods (distillation, rotary evaporation and freeze-drying) would result in the H2O2 either evaporating or being degraded. The major method, dialysis, would just result in a dilute solution of H2O2 distributed between the inside and outside of the membrane.
I guess P. Pardha-Saradhi is right. I have not framed the questions right. It went all wrong. Its not what I want to know. It is obvious that if I were to prepare 35% solution from 30% solution, I have to concentrate it.
The research articles I'm following says use 2 moles of a 35% by weight hydrogen peroxide solution.
But I have 30% by weight hydrogen peroxide available.
Now the reframed question is:
Ques 1: Can I use 30% by weight hydrogen peroxide instead of 35% by weight hydrogen peroxide for peroxidation reaction.
Ques 2: if the paper says 2 moles of a 35% by weight hydrogen peroxide. How much amount (quantity) of 30% hydrogen peroxide, I should use.
You can use H2O2 30% by weight hydrogen peroxyde instead of 35%.
I have not read the paper but you have to verify if this paper advises to add 2 moles of a H2O2 or if you have to work with a 2mol/l H2O2 solution.
If you had to add 2 moles of a H2O2 35% solution, it correspond to add194g or 175 ml of a solution H2O2 35% by weight hydrogen peroxyde. If you want to use a 30% H2O2 solution, 2 moles of H2O2 correspond to 227g or 201 ml of a solution H2O2 30% by weight hydrogen peroxyde.
If the paper deals with a concentration of 2mol/l of H2O2, you have to dilute your initial solution of H2O2.
A H2O2 30% by weight hydrogen peroxyde has a concentration of 9,79 mol/l of H2O2
A H2O2 35% by weight hydrogen peroxyde has a concentration of 10,63 mol/l of H2O2
I agree with Jerome.
It looks you want to prepare 2 M hydrogen peroxide from 30% (i.e. ~9.79 M) hydrogen peroxide.
If you still want 35%, have a bunch of 30% you want to use, and a lot of time on your hands, you could probably enrich it by controlled freezing, since it forms a (admittedly complex) eutectic. Possibly the safest way to manipulate concentrated H2O2 solutions. But then you'd have to filter off the slush (not through cellulosic paper, please!) and titrate each phase to see if you've gotten anywhere. What a bother.
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