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
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.
Thank you!
To determine whether the aqueous phase will be the lower or upper layer after dissolving sodium chloride in the mixture, you need to consider the density of the resulting solution.
To begin, let's calculate the mass of the aqueous layer after dissolving sodium chloride.
Given:
- Volume of the aqueous solution: 112 ml
- Sodium chloride mass: 40 g
First, convert the volume of the aqueous solution from milliliters to grams using the density of water. The density of water is approximately 1 g/ml.
Mass of the aqueous solution = Volume of the aqueous solution x Density of water
Mass of the aqueous solution = 112 ml x 1 g/ml = 112 g
Next, calculate the total mass of the solution after dissolving sodium chloride.
Total mass of the solution = Mass of the ethylene bromohydrin + Mass of the ethylchloride + Mass of the aqueous solution
Total mass of the solution = Volume of ethylene bromohydrin x Density of ethylene bromohydrin + Volume of ethylchloride x Density of ethylchloride + Mass of the aqueous solution
Given:
- Volume of ethylene bromohydrin: 25 ml
- Density of ethylene bromohydrin: 2.41 g/ml
- Volume of ethylchloride: 100 ml
- Density of ethylchloride: 0.92 g/ml
Total mass of the solution = 25 ml x 2.41 g/ml + 100 ml x 0.92 g/ml + 112 g
Total mass of the solution = 60.25 g + 92 g + 112 g
Total mass of the solution = 264.25 g
Now we can compare the density of the aqueous solution (mass/volume) with the density of the ethylene bromohydrin and ethylchloride. The layer with the higher density will be at the bottom.
Density of the ethylene bromohydrin = Mass of the ethylene bromohydrin / Volume of the ethylene bromohydrin
Density of the ethylchloride = Mass of the ethylchloride / Volume of the ethylchloride
Density of the aqueous solution = Mass of the aqueous solution / Volume of the aqueous solution
Comparing these values, if the density of the aqueous solution is higher than both the ethylene bromohydrin and ethylchloride, the aqueous phase will be the lower layer in the solution. However, if the density is lower than both, the aqueous phase will be the upper layer.
Additionally, you can confirm this by conducting a simple experiment. Take a small volume of the solution and add a few drops of a water-soluble colored dye (e.g., food coloring) to it. Observe where the dye settles to determine the layering of the solution. If the dye sinks to the bottom, it indicates that the aqueous solution is the lower layer. If the dye remains at the top, it indicates that the aqueous solution is the upper layer.