a) You use 100 ml ethylchloride (density 0.92 g/ml) to extract 25 ml ethylene bromohydrin (density 2.41 g/ml) mixed with 100 ml. Is the aqueous layer the lower or the upper layer. How could you easily test this.
----- Ethylchloride is less dense so it is the top layer
Ethylene Bromohydrin is more dense so it is the bottom layer
b) You dissolve sodium chloride 40g. in the above mixture. Assuming the aqueous layer will have a volume of 112 ml, will the aqueous phase be the lower or the upper layer? Explain.
I am having problem with this question.
To determine whether the aqueous phase will be the lower or upper layer after dissolving sodium chloride, we need to consider the density of the resulting solution.
First, let's calculate the density of the sodium chloride solution. We know the mass of sodium chloride (40g) and the volume of the aqueous phase (112ml). Density is calculated by dividing the mass by the volume:
Density = mass / volume
Density = 40g / 112ml ≈ 0.357 g/ml
Now, we need to compare the density of the sodium chloride solution (0.357 g/ml) with the densities of the ethyl chloride (0.92 g/ml) and ethylene bromohydrin (2.41 g/ml).
Since the density of the sodium chloride solution (0.357 g/ml) is less than both the density of ethyl chloride (0.92 g/ml) and ethylene bromohydrin (2.41 g/ml), it will be the upper layer.
The reason for this is that when two immiscible liquids are mixed, the less dense liquid forms the top layer, while the more dense liquid forms the bottom layer. In this case, ethyl chloride, being less dense than both the sodium chloride solution and ethylene bromohydrin, forms the top layer, while ethylene bromohydrin forms the bottom layer.
Therefore, the aqueous phase (sodium chloride solution) would be the upper layer in this case.