Question

Which of the following is most soluble in water?

Answer 1

answers>>>>>>>>>?

Answer 2

Here it is

Answer 3

Three of those compounds can H-Bond. let's also try to rank them in terms of solubility in water.

Answer 4

carboxylic acid is the most water suitable

Answer 5

I got this wrong too, the first time I did it.

Answer 6

It said... lol it's the Na2SO4 is the most water soluble out of all of them

Answer 7

I knew it
I was having a doubt between those 2

Answer 8

yeah.. like I guess it makes sense because ionic compounds dissolve completely, in water.. but as for the order I think it would be the compound with the nitrogen<oxygen<carboxylic acid then< the ionic compound

Answer 9

I agree wit you though the carboxylic acid would be the most out of the three b.c it has an additional LP to act as a hydrogen bond acceptor i think.

Answer 10

let me post another here

Answer 11

What about this one?

Answer 12

Question is: which of the following gases is most likely to be ideal.

Answer 13

He

Answer 14

Yeah He

Answer 15

You can eliminate right away two of the choices, the HF cuz of H bonding, and the alkene forgot what it was vanderwaals or something.

Answer 16

For the first one, you can actually directly consider \(Na_2 SO_4\) to be the conjugate base of the very very strong acid \(H_2SO_4\), which according to wikipedia has -3 pka for the first hydrogen and 1.99 pka for the second hydrogen.

Butanoic acid (which smells like puke, it's the stuff in rotten milk, and has a common name of butyric acid, it's gross) has a pka of about 4 since it's a caboxylic acid (you should or will eventually end up remembering this).

The point of all this is Butanoic acid might lose its hydrogen because it's acidic, however you should think of the ionic compound as an acid that already lost its hydrogen because it's even more acidic. When it comes down to it, a "strong" acid is just really "weak" at holding onto Hydrogen atoms, which is kind of backwards haha.

For the second one, like you said, just have to figure out which atom is smaller, He or Xe since the ideal gas approximation neglects particle-particle interactions. :P

Answer 17

Yeah it was Helium guys!

Answer 18

and yeah I never thought about it that way! at least wit the ionic compound(s). -3 pKa wow lol basically a ka >>>>>>1 lol

Answer 19

the problem said something about Xe having more electrons so greater chance of interaction as opposed to Helium

Answer 20

agree @Photon336

Answer 21

going to close this out and post another one