I have calculated the molarity of 30% H2O2 solution as follows. Is this correct?
It means 30 g of H2O2 in 100 g of solution
MW of H2O2 = 34.01 g/mol
The Volume of 100 g of solution = weight/density
Density of 30% H2O2 solution = 1.11 g/cc
So, volume of solution = 100/1.11 = 90.09 mL
Amount in 90.09 mL of solution = 30 g
Amount in 100 mL of solution = (30/90.09)x 100 = 33.3 g
No of moles = 33.3/34.01 = 0.979 moles
Molarity = no of moles in one litter of solution = 0.979/0.1 = 9.79 molar [100mL = 0.1L]
Molarity is the molar concentration, which refers to the number of moles per 1 litre.
You have a 30% solution of H2O2, with a density of 1.45 g/cm3. It is important to note that we are considering the density of the solute, not the solution.
Therefore, the molarity or molar concentration of the 30% H2O2 solution is 12.79 M/dm3.
Consequently, in 100 mL of the solution, you have 1.279 moles of H2O2.
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