Comments on: 3 Trends That Affect Boiling Points

By: Surendra kumar

Surendra kumar — Thu, 06 May 2021 14:20:22 +0000

As the number of carbon Atoms increases their molecular mass increases and their vanderwalls force of attraction increases and this leads to increases in boiling points of higher hydrocarbon chains

By: YISHA

YISHA — Tue, 23 Feb 2021 18:14:58 +0000

What causes the boiling point of higher hydrocarbons to be high?

By: James Ashenhurst

James Ashenhurst — Tue, 23 Feb 2021 17:59:24 +0000

In reply to YISHA. That's something you can easily look up!

By: YISHA

YISHA — Sun, 21 Feb 2021 08:42:14 +0000

Which one has higher boiling point CH3OH or CH3CH2OH

By: James Ashenhurst

James Ashenhurst — Wed, 30 Sep 2020 02:54:45 +0000

In reply to Andre. Is your compound water soluble or organic soluble? Because if it's soluble in organic solvent, you can avoid worrying about this by just extracting with something like ethyl acetate. If your compound is water soluble and you are drying it through rotary evaporation / distillation, the acetic acid and water will evaporate at similar rates. At the end you will have NaOH / NaOAc salts however.

By: Andre

Andre — Tue, 29 Sep 2020 10:09:04 +0000

I am trying to figure out if acetic acid will evaporate or not in the drying step of my compound after treating the solution with NaOH to a pH around 8

By: James Ashenhurst

James Ashenhurst — Mon, 28 Sep 2020 16:34:50 +0000

In reply to Andre. Are you trying to purify acetic acid?

By: Andre

Andre — Mon, 28 Sep 2020 07:04:30 +0000

Thank you James.
Remaining with the same example (in the extremes as you said), if I make the solution of diluted acetic acid completely boil in a beaker as to remove water, what will remain in the beaker? Acetate salts?

By: James Ashenhurst

James Ashenhurst — Fri, 25 Sep 2020 16:15:10 +0000

In reply to Andre.

It’s hard to answer this question without more specific detail.

In the extremes, it’s easy to answer. For instance if H2O is protonated *completely* with a strong acid, it becomes H3O+ . Being a charged compound it therefore has a very low volatility (this is why H2SO4 is often used to remove water). The same is true when H2O is completely deprotonated to NaOH.

The same would hold for acetic acid if it was either protonated completely or deprotonated completely. Salts are not volatile.

By: Andre

Andre — Mon, 14 Sep 2020 10:06:49 +0000

Take for example a diluted solution of acetic acid in water. Will the bp of acetic acid change at acidic pH or basic pH?