Question

Ozzie wanted to do another experiment using 10.8% (by mass) H₂O₂. What is the molarity of this H₂O₂ solution?

Answer 1

unsolvable

Step-by-step explanation:

Molarity is defined by the equation:

`M=(n)/(v)`

where
`n` is the number of moles of solute and
`v` is the total volume of the solution (in liters).

We are given that 10.8% of the weight of an H₂O₂ solution is H₂O₂ (and the rest is water, H₂O).

To figure out how many moles of H₂O₂ there would be in a 1kg solution, we can first find the molar mass of H₂O₂.

H₂O₂ ⇒ 2(1.008) + 2(15.999) = 34.014 g/mole

We know that there should be 108g of H₂O₂ in a 1kg solution, and we can convert this mass to moles using the molar mass we just solved for:

`\frac{108\!\\ot\!\text{g}}{1} \cdot \frac{1\text{ mole}}{34.014\!\\ot\!\text{g}} = 3.175\text{ mole } \text{H}_2\text{O}_2`

However, since the density of the solution is not given, we cannot accurately calculate the molarity.