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Organic liquids A, B, and C have densities of 0.690, 0.955 and 1.126 g/mL, respectively. A and C are low polarity solvents, while B is a highly polar solvent. If each were added to water separately, how would you expect them to behave? (address solubility and density)

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closed as off-topic by Klaus Warzecha, Philipp, Satwik Pasani, Amaterasu, tschoppi Mar 1 '14 at 13:50

This question appears to be off-topic. The users who voted to close gave this specific reason:

If this question can be reworded to fit the rules in the help center, please edit the question.

How about you have a go at the question first? – Richard Terrett Nov 8 '12 at 3:29
I agree with Richard. The object of the question seems to be that YOU think and discuss various possibilities – Epicentre Nov 8 '12 at 5:21
I agree with @RichardTerrett. Tell us what you have tried and what you do and don't understand about this problem. Doing so will get you a much better answer that will be useful to more people than just you. – Ben Norris Nov 8 '12 at 12:04
@Epicentre Thanks for your input. Answers are reserved for actual answers to the question. I have moved this up to a comment for now. – jonsca Nov 8 '12 at 22:10

The first thing to do is determine the polarity and density of water. The density of water is 1.00 g/mL. Because the electronegativities of hydrogen and oxygen are not close at all (2.2 for hydrogen and 3.44 for oxygen), water is definitely polar. With this information, we can compare it with the given information to determine what will happen.

Adding Solvent A to Water:

Solvent A is lowly-polar and less-dense than water. Because solvent A is less-dense, it will float on or just below the surface of the water. Because 'like dissolves like', solvent will not dissociate in water a large amount.

Adding Solvent B to Water:

Solvent B is very polar and about the same density of water. Because the densities are very similar, you would expect solvent B to be distributed evenly throughout solution. Going back to 'like dissolves like', because solvent B is very polar, you can expect to dissociate very well in water.

Adding Solvent C to Water:

Solvent C is lowly-polar and more-dense than water. Because solvent C is more-dense than water, it will sink to the bottom. Solvent C behaves similar to solvent A in terms of dissociation because they have the same polarities.

Just a note: the question mentioned solvents A and C have low polarities. When put in water, they will dissociate a little, but in general won't do much.

'Like Dissolves Like'

The phrase 'like dissolves like' is a common term in solubility chemistry to explain that molecules of the same polarities will dissolve each other. Polar molecules will generally dissolve other polar molecules, while non-polar will dissolve non-polar. (That's a really simplified explanation of solubility; it can get complicated.)

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Welcome to Chemsitry.SE @Peter. This is a nice answer. However, the question is tagged "Homework". In our homework policy, we encourage the OP to show us what they have been able to accomplish before we answer, and even then we should not provide the complete answer. – Ben Norris Nov 12 '12 at 11:40

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