rank strongest acid to weakest acid?

rank strongest acid to weakest acid

H3CNH2
CH3C (triple bond) CH
CH2=CHCH3
H20
CH4

i tried to rank them using the Pka values but I couldn't find the pKa value of the alkyne and I thought the H3CNH2 was the strongest but it's not?

wow.....not even close to the answer....

it was H2O first and then the triple bond, the amine, double bond, and CH4....
:/

I did this same problem on Sapling Learning and I can confirm Anonymous's answer is correct. Now, if only someone can explain why it makes sense. Is it just comparing pKa values?

The strongest is the triple bond with terminal H. You had that ranked correctly yesterday when you first posted this problem.

Next is double bond with terminal H.
CH3NH2 is an amine and is basic. That will be the weakest acid listed.
You place H2O and CH4. Can you find the pKa values for CH4 and H2O? I think H2O is 16 but I'm not sure my memory is that good and I don't know pKa for CH4. However, the two go between the amine and the double bond with terminal H.

What is the name to h2c

sp C is more acidic than sp2 C which is more acidic than sp3 C because it is more electronegative relatively. Thus, alkene (triple bond) acidity > alkene > alkane

Well, let me break it down for you in a way that hopefully won't make your head spin like a triple bond!

First off, when it comes to acids, we usually look at their ability to donate protons (H+ ions). The stronger the acid, the more eager it is to let go of those protons like a clingy ex.

Now, from the list you've given, let's put on our acrobatic gloves and start with the strongest acid around town: H3CNH2!

H3CNH2 might seem innocent with all those nitrogen and hydrogen buddies, but don't be fooled. It's actually an extremely strong base called methylamine. And as we all know, acids and bases don't play well together, so that's why H3CNH2 has some serious acid game!

Next up, we have CH3C (triple bond) CH, or acetylene. Although I couldn't find its exact pKa value either (it's a sneaky one!), it is known to be fairly acidic due to the presence of the triple bond. So, let's give it a spot in the middle of the acid hierarchy.

Now, let's move on to CH2=CHCH3, or good ol' propene. While propene does have some acidic character, it's not as strong as our previous contenders. So, we'll slide it down the list a bit.

Now, prepare yourself for a splash of disappointment because H2O (water) is actually a pretty weak acid. Don't get me wrong, it sure makes up for it in other areas (like putting out fires and keeping you hydrated), but when it comes to acidity, it's not as strong as the others.

And finally, we have CH4, aka methane. Methane, my friends, is like a teddy bear at a grizzly bear convention when it comes to acidity. It just can't compete with the others and is the weakest acid in this lineup.

So, to summarize (drumroll, please!):

1. H3CNH2 (Methylamine)
2. CH3C (triple bond) CH (Acetylene)
3. CH2=CHCH3 (Propene)
4. H2O (Water)
5. CH4 (Methane)

I hope that clears things up for you, and may the acids be with you!

To rank the acids from strongest to weakest, you can consider their acidity based on their conjugate bases' stability. The stronger an acid, the weaker its conjugate base.

Let's compare the given compounds and determine their relative acidity:

1. H3CNH2 (Methylamine): In this compound, the nitrogen atom (N) can donate its lone pair of electrons, making it a weak base. Therefore, H3CNH2 can be considered a weak acid.

2. CH3C (triple bond) CH (Propyne): The acidity of alkynes generally increases with the number of acetylenic hydrogen atoms (terminal hydrogen atoms directly bonded to the carbon triple bond). The acidity is influenced by the stability of the resulting acetylide ion. Since you couldn't find the pKa value, we can assume that the acidity of propyne (CH3C≡CH) is relatively higher than that of methylamine.

3. CH2=CHCH3 (Propene): Unlike alkynes, alkenes do not have acidic properties because there are no acidic protons directly bonded to the double bond.

4. H2O (Water): Water is a weak acid because it can donate a proton, forming a hydroxide ion (OH-) as its conjugate base.

5. CH4 (Methane): Methane is not an acid because it does not have any acidic protons.

Based on this analysis, we can rank the compounds from strongest to weakest acid as follows:
1. CH3C (triple bond) CH (Propyne)
2. H3CNH2 (Methylamine)
3. H2O (Water)
4. CH2=CHCH3 (Propene)
5. CH4 (Methane)

Please note that this ranking is based on the general trends in acidity for similar compounds. Actual pKa values might vary depending on specific conditions and experimental data.