Recent content by MermaidWonders

Hey! Thought I'd drop by and ask. Something strange happened this morning. I turned on my iPod because I was going to listen to a lecture recording for a class. I could get the voice memo to "play", but absolutely no sound is coming out. I tried it with and without headphones, but no luck at...

Hi, Sorry for the super late reply. Just saw this. When I first came across that question, I was very confused as to why my professor had put "6 H, t" and "4 H, quintet" for the splitting patterns and peak integrations for the red and blue set of protons, respectively (as in the screenshot)...

Never mind. I see why.

For the colourfully-annotated compound above, why aren't the splitting patterns and integrations for the red and blue set of protons "pentet, 6 H" and "octet, 4 H", respectively?

Alrighty, thank you so much!

So is soap just not the appropriate surfactant to make a hexane in water emulsion? Also, is it true that we can essentially make almost any emulsion by choosing the right surfactants?

Hey, just another question pertaining to the same lab from last week... since soap can make oil/grease soluble in water, why is hexane immiscible in soap solution?

So they essentially solubilize everything?

Hi, sorry if this is a really dumb question, but since soaps have both a polar and a non-polar component to them, does it mean that they can actually dissolve all substances (polar and non-polar)?

Ah, makes sense now. Thank you so much! :)

Sorry, I didn't clarify. "Strength" as in whether the acid/base is strong or weak. So should I consult the table of relative strengths of acids and bases, or is it already obvious to say that all of them would burn the skin?

Which of the following will burn your skin if you get it on you? a. concentrated sulfuric acid b. concentrated nitric acid c. concentrated potassium hydroxide d. concentrated hydrochloric acidMy first instinct was that all of them would since they are either concentrated acids or bases. I then...

Yeah, OK, got it. Thanks!

Ah, I see now. :) So if the whole molecule is an electrophile overall, is there a case where the Cl atom serves as the electrophilic site? It's just that with the problems I've encountered so far, I'm used to seeing the C atom acting as the electrophilic site and Cl the nucleophilic site but...

Wait... doesn't the polar bond between C and Cl result in Cl being negatively-polarized?