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 of water. Is the aqueous layer the lower or the upper layer. How could you easily test this.
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 went through this last night and you've corrected at least one of the problems. What is your trouble now? Explain in detail.
Based on my calculations I would think the aqueous layer would be on the bottom for a. How can you test it. You have the mixture in a sep funnal, add a drop or two or water and see if it sinks through the upper layer to the bottom layer or mixers with the upper layer.
The second part of the question I found that aqueous phase is still the bottom layer based on the density of each.
I just want to make sure I'm on the right track.
Thanks!
I think you're ok if the assumption that the volumes are additive is ok but I don't know about that. Having said that, I don't know of any other way of approaching the problem. If I were making up the problem I would have made the aq layer the top on a and the bottom after adding the NaCl in b but the calculations don't show that.
To determine whether the aqueous layer is the lower or the upper layer in the given mixture, we can use the concept of density. Since ethylene bromohydrin has a higher density than water, it would be expected to sink to the bottom of the mixture and become the lower layer. On the other hand, ethylchloride has a lower density than water, so it would be expected to float on top and become the upper layer.
To test this, you can simply observe the separation of the layers after the mixture has been allowed to settle. When the density of two immiscible liquids is different, they will naturally separate into layers based on their densities. The denser liquid will settle at the bottom, while the less dense liquid will float on top.
Now, let's move to the second part of the question. When you dissolve sodium chloride (NaCl) in the mixture, it will increase the density of the aqueous layer as sodium chloride is a dense compound. This increase in density of the aqueous layer could affect its position in the mixture.
To determine whether the aqueous phase will be the lower or the upper layer after dissolving sodium chloride, we need to consider the change in density caused by the addition of the salt. Since sodium chloride is a dense compound, its addition will increase the overall density of the aqueous layer.
If the density of the aqueous layer becomes higher than that of the ethylene bromohydrin, it will sink to the bottom and become the lower layer. However, if the density of the aqueous layer remains lower than that of the ethylene bromohydrin, it will continue to float on top and be the upper layer.
To calculate the volume of the aqueous layer, we first need to determine the mass of the solution, which is the sum of the mass of ethylene bromohydrin (density 2.41 g/ml) and water (density 1 g/ml). Given that the volume of ethylene bromohydrin is 25 ml and the volume of water is 100 ml, we can find their respective masses using their densities.
Mass of ethylene bromohydrin = Volume × Density = 25 ml × 2.41 g/ml
Mass of water = Volume × Density = 100 ml × 1 g/ml
Once you have the mass of the solution, you can add the mass of sodium chloride (40 g) to the total mass. From this, you can calculate the resulting density of the aqueous layer.
If the density of the aqueous layer with dissolved sodium chloride is greater than the density of ethylene bromohydrin, the aqueous layer will be the lower layer. Otherwise, if the density is lower, the aqueous layer will remain the upper layer.
By considering the densities and using basic calculations, you can determine whether the aqueous layer will be the lower or the upper layer in the given mixture.