Question

Suppose now that you wanted to determine the den-sity of a small yellow crystal to confirm that it is sulfur. From the literature, you know that sulfur has a density . of 2.07 g/cm. 3. How would you prepare 20.0 mL of the liquid mixture having that density from pure sam-ples of CHCl3and CHBr3? (Note:1 mL = 1 cm. 3.)

Answer 1

Answer : The volume of liquid mixture
`CHCl_3` and
`CHBr_3` are, 11.73 ml and 8.27 ml respectively.

Explanation : Given,

The overall density of mixture =
`2.07g/cm^3=2.07g/ml`

The density of
`CHCl_3` = 1.492 g/ml

The density of
`CHBr_3` = 2.890 g/ml

Total volume of liquid mixture = 20 ml

Let us assumed that the volume of
`CHCl_3` = X ml and the volume of
`CHBr_3` = Y ml

So, the sum of volumes is equal to the total volume of mixture required.

`Xml+Yml=20ml` ...............(1)

As we have to determine the density of the liquid mixture. So, the mass would be,

`Density* Volume=Mass`

The equation will be :

`\text{Density of }CHCl_3* \text{Volume of }CHCl_3+\text{Density of }CHBr_3* \text{Volume of }CHBr_3=\text{Density of mixture}* \text{Volume of mixture}`

`1.492g/ml* (Xml)+2.890g/ml* (Yml)=2.07g/ml* (20ml)` ........(2)

Now equating both the equation 1 and 2, we get the

X = 11.73 ml

Y = 8.27 ml

Therefore, the volume of liquid mixture
`CHCl_3` and
`CHBr_3` are, 11.73 ml and 8.27 ml respectively.

Answer 2

So the question ask that how to prepare 20ml of the liquid mixture having a denstiy of 2.7 g/cm and the best answer, base on the data you have given and further formulation of a solution, the answer would be CHCL3=11.73ml and CHBr3 = 8.268 ml. I hope you are satisfied with my answer