For "16.8 V" H2O2 solution ( density = 0.95 g/ml), calculate :- 1. Molarity 2. Molality 3. % w/w 4. % w/v 5. ppm of solute 6. mole fraction of solute
Answers
A sample of H2O2 solution lebelled as 16.8 volume has density 0.95 g/ml.
To find :
- Molarity
- Molality
- percentage w/w
- percentage w/v
- ppm of solute
- mole fraction
solution : Molarity = volume strength/11.2
= 16.8/11.2
= 1.5
Molarity of H2O2 solution is 1.5 M, it means 1.5 moles of H2O2 present in 1000 ml of solution.
so, mass of solvent = volume of solution × density of solution
= 1000 ml × 0.95 g/ml
= 950 g
now Molality = no of moles of solute/mass of solvent in kg
= 1.5 × 1000/950
= 150/95
= 1.58 molal
percentage w/w = mass of solute/mass of solution × 100
mass of solute = 1.5 × 34 = 51 g
mass of solution = 950g + 51 g = 1001g
now percentage w/w = 51/1001 × 100
= 5.0949 %
percentage w/v = mass of solute/volume of solution × 100
51/1000 × 100
= 5.1 %
ppm of solute = mass of solute/mass of solution × 10⁶
= 51/1001 × 10⁶
= 0.050949 × 10⁶
= 5.0949 × 10⁴
mole fraction of solute = 1.5/(1.5 + 950/18) [ mole of solvent = 950/18 ]
= 1.5/(1.5 + 52.78)
= 1.5/54.28
= 0.02763