Explain the water solubilities in different compounds?

Question

Please explain the order of water solubilities for the compounds in each of the following groups:

a) Ethanol>Choloroethane>Ethane

b) Methanol>Ethanol>1-propanol

Answer 1

There is the broad statement of "like dissolves like"

Since water is very polar, it will have a hgher solubility with very polar compounds.

In your group a, only ethanol is polar. The others will have low or no solubility in water

In group b, the sequence again follows the amount of polarity. Methanol, ethanol and propanol have the same OH group, but as the carbon chain gets bigger, the percentage of the polarity in the molecule goes down

Answer 2

Hydrogen Bonding will probable be the biggest impact. besides the undeniable fact that, CO2 isn't very soluble in water (that's why sodas flow flat once you go away them open. the extra beneficial tension that's utilized while canned keeps it in). CO2 is a without delay formed molecule with carbon interior the middle and oxygen on the exterior. there'll be a extra unfavourable average charge around the oxygen, yet no longer as a lot because of fact the water (in different words, there is not any dipole 2nd). London dispersion forces are hapening yet they are so vulnerable that they have got not got an excellent impression here. Water has a dipole 2nd, so the helpful end could be interested in the somewhat unfavourable components of the CO2. This appeal is in basic terms very vulnerable. Ionic bonding is an extremely good bond and is quite a chemical bond (think of salt). you may warmth it with a torch and it won't ruin. Covalent bonding is what holds oxygen and carbon jointly in CO2. wish that helps with this question and any others you have have been given.