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.)

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

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BarrettArcher BarrettArcher · Answer 2 · 2019-05-29T11:25:05+02:00

Answer : The volume of liquid mixture [tex]CHCl_3[/tex] and [tex]CHBr_3[/tex] are, 11.73 ml and 8.27 ml respectively.

Explanation : Given,

The overall density of mixture = [tex]2.07g/cm^3=2.07g/ml[/tex]

The density of [tex]CHCl_3[/tex] = 1.492 g/ml

The density of [tex]CHBr_3[/tex] = 2.890 g/ml

Total volume of liquid mixture = 20 ml

Let us assumed that the volume of [tex]CHCl_3[/tex] = X ml and the volume of [tex]CHBr_3[/tex] = Y ml

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

[tex]Xml+Yml=20ml[/tex] ...............(1)

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

[tex]Density\times Volume=Mass[/tex]

The equation will be :

[tex]\text{Density of }CHCl_3\times \text{Volume of }CHCl_3+\text{Density of }CHBr_3\times \text{Volume of }CHBr_3=\text{Density of mixture}\times \text{Volume of mixture}[/tex]

[tex]1.492g/ml\times (Xml)+2.890g/ml\times (Yml)=2.07g/ml\times (20ml)[/tex] ........(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 [tex]CHCl_3[/tex] and [tex]CHBr_3[/tex] are, 11.73 ml and 8.27 ml respectively.