H2SO4 vs H2CO3

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Joussie Camacho 4I
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Joined: Tue Oct 02, 2018 12:16 am

H2SO4 vs H2CO3

Postby Joussie Camacho 4I » Sat Dec 08, 2018 12:25 am

If both H2SO4 and H2CO3 are polyprotic acids, why is sulfuric acid a strong acid but carbonic acid is not? Is it because although carbonic acid CAN donate its 2 H+s, it's very unlikely to? Why then does sulfuric readily donate one H+ to make HSO4- ?

Posts: 31
Joined: Fri Sep 28, 2018 12:25 am

Re: H2SO4 vs H2CO3

Postby sameeksha_panda_3h » Sat Dec 08, 2018 3:11 am

I'm not completely sure, but HSO4- is probably a more stable conjugate bas than HCO3-! In addition to other factors, the stability of the conjugate can contribute to concentration of H+ in a solution.

Ahmed Mahmood 4D
Posts: 72
Joined: Fri Sep 28, 2018 12:28 am

Re: H2SO4 vs H2CO3

Postby Ahmed Mahmood 4D » Sat Dec 08, 2018 10:58 pm

Because HSO4- has sulfur, which has a greater electronegativity than carbon, the anion is more stable (Due to electron delocalization) and thus its acid is stronger.

Nicole Elhosni 2I
Posts: 62
Joined: Fri Sep 28, 2018 12:28 am

Re: H2SO4 vs H2CO3

Postby Nicole Elhosni 2I » Sun Dec 09, 2018 7:40 am

In class, Dr. Lavelle pointed out though that both SO4 2- and CO3 2- have resonance, which means their electrons are delocalized and the anion will be stable. Doesn't this make the acid a strong acid then?

Shutong Hou_1F
Posts: 117
Joined: Sat Sep 14, 2019 12:17 am

Re: H2SO4 vs H2CO3

Postby Shutong Hou_1F » Sun Dec 01, 2019 4:11 pm

H2SO4 is more readily to donate H atoms than H2CO3 because S is more electronegative by having more protons (in 4th period, while C is in 3rd period) and thus have more electron density withdrawing power.

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