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I have two compounds with two hydrogens namely (a),(b),(c) and (d). I have to compare the acidity of the following hydrogens.

My approach:

I removed the hydrogen atoms one by one and compared the stabilities, as there are most resonating structures for (a) it will be most stable (most acidic too). Then followed by (b), (c) and (d).

But the answer is given different without any further explanation. Does anybody have the right approach to tackle these type of questions?

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  • $\begingroup$ b and d should be many orders of magnitude weaker then a and c BTW both compounds are probably as acidic as typical carboxylic acid. $\endgroup$
    – Mithoron
    Commented Mar 11, 2019 at 0:29
  • $\begingroup$ en.wikipedia.org/wiki/Chemistry_of_ascorbic_acid#Acidity $\endgroup$
    – Mithoron
    Commented Mar 11, 2019 at 0:31
  • $\begingroup$ Order is different from what you're saying. $\endgroup$
    – Sahil Silare
    Commented Mar 11, 2019 at 2:42
  • $\begingroup$ c must be more acidic than a, for sure. does that go well with your textbook's answers? $\endgroup$
    – William R. Ebenezer
    Commented Mar 11, 2019 at 8:51
  • $\begingroup$ And you should get better textbook. $\endgroup$
    – Mithoron
    Commented Mar 11, 2019 at 18:53

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