Which is the weaker acid h2so3 or h2seo3?
Answers
Answered by
1
◇hy user◇
Here's ur answer 》》》》》
There are two basic classes of acids: binary acids and oxyacids. Binary acids are molecules like HCl, HBr, HI, etc. We’re not interested in them.
Oxyacids (sometimes written as oxoacids) are acids that contain hydrogen, oxygen, and one other element. The strength of an oxyacid depends on two things:
The electronegativity of the central atom, and…The number of oxygen atoms bonded to the central atom.
Both of these factors affect the strength of the oxyacid in the same way: by drawing electron density away from the O-H bonds.
You see, a strong acid is one that ionizes completely, or nearly completely. In oxyacids, the ionizable hydrogen is bonded to an oxygen atom rather than to the central atom; hence, the ionization of an oxyacid involves severing an O-H bond. This is easier in acids where electron density is drawn away from the O-H bond by highly electronegative atoms elsewhere in the molecule.
In the case of H2CO3 and H2SO4, there are two things that make H2SO4 a stronger acid than H2CO3. For one, the central atom in H2SO4, sulfur, is more electronegative than the central atom in H2CO3, carbon, and therefore draws more electron density away from the two O-H bonds. Also, H2SO4 has four oxygen atoms, two of which are not bonded to hydrogen atoms and therefore capable of drawing electron density away from O-H bonds. Carbonic acid, on the other hand, has only three oxygen atoms, only one of which is not bonded to hydrogen. Ergo, there is more electron density around the O-H bonds in carbonic acid than there is in sulfuric acid, which means the bonds are stronger, the hydrogen atoms more difficult to remove, and the acid weaker.
Keep in mind that H2SO4 is a strong acid, but HSO4- isn’t. When the second H+ ion is removed, a highly-negative SO4(2-) ion is left behind, which quickly reclaims hydrogen ions from the surrounding H3O+ and H2O molecules, reforming HSO4- relatively quickly.
Hope it helps ☺⚡✌
Here's ur answer 》》》》》
There are two basic classes of acids: binary acids and oxyacids. Binary acids are molecules like HCl, HBr, HI, etc. We’re not interested in them.
Oxyacids (sometimes written as oxoacids) are acids that contain hydrogen, oxygen, and one other element. The strength of an oxyacid depends on two things:
The electronegativity of the central atom, and…The number of oxygen atoms bonded to the central atom.
Both of these factors affect the strength of the oxyacid in the same way: by drawing electron density away from the O-H bonds.
You see, a strong acid is one that ionizes completely, or nearly completely. In oxyacids, the ionizable hydrogen is bonded to an oxygen atom rather than to the central atom; hence, the ionization of an oxyacid involves severing an O-H bond. This is easier in acids where electron density is drawn away from the O-H bond by highly electronegative atoms elsewhere in the molecule.
In the case of H2CO3 and H2SO4, there are two things that make H2SO4 a stronger acid than H2CO3. For one, the central atom in H2SO4, sulfur, is more electronegative than the central atom in H2CO3, carbon, and therefore draws more electron density away from the two O-H bonds. Also, H2SO4 has four oxygen atoms, two of which are not bonded to hydrogen atoms and therefore capable of drawing electron density away from O-H bonds. Carbonic acid, on the other hand, has only three oxygen atoms, only one of which is not bonded to hydrogen. Ergo, there is more electron density around the O-H bonds in carbonic acid than there is in sulfuric acid, which means the bonds are stronger, the hydrogen atoms more difficult to remove, and the acid weaker.
Keep in mind that H2SO4 is a strong acid, but HSO4- isn’t. When the second H+ ion is removed, a highly-negative SO4(2-) ion is left behind, which quickly reclaims hydrogen ions from the surrounding H3O+ and H2O molecules, reforming HSO4- relatively quickly.
Hope it helps ☺⚡✌
Similar questions