What would be more acidic? SO2 or SO3?
Does this have to do something with the higher oxidation state? And why is that?
Or can we say SO3 is more acidic by,
SO2+H2O--->H2SO3
SO3+H2O--->H2SO4
as H2SO4 is more acidic?
Yes that is what I meant! :-)
Your second thought is right on. H2SO4 is a stronger acid than H2SO3. However, a clarification needs to be made. I don't think it's proper t ask if SO2 or SO3 is more acidic. I think what you means is "is an aqueous SOLUTION of SO2 or an aqueous SOLUTION of SO3 more acidic?"
SO3 is more acidic compared to SO2. This is because the oxidation state of sulfur in SO3 is +6, while in SO2 it is +4. Higher oxidation states often result in more acidic compounds.
The acidity of oxides is determined by their ability to donate protons (H+ ions) when dissolved in water. In this case, when SO2 reacts with water, it forms sulfurous acid, H2SO3, while SO3 reacts with water to form sulfuric acid, H2SO4. Sulfuric acid (H2SO4) is a stronger acid compared to sulfurous acid (H2SO3).
Therefore, based on the reaction equations you provided, we can conclude that SO3 is more acidic than SO2.
To determine which compound, SO2 or SO3, is more acidic, we need to consider their chemical properties and structure.
Firstly, the acidity of an oxide is related to its ability to donate a proton (H+ ion) when it interacts with water. In general, the more electronegative elements have a higher tendency to donate a proton, making oxides of more electronegative elements more acidic.
In the case of SO2 and SO3, the electronegativity of sulfur increases with the higher oxidation state. This means that SO3, with a higher oxidation state of sulfur compared to SO2, is expected to be more acidic.
Now, let's focus on why the higher oxidation state leads to increased acidity. In the process of oxidation, sulfur gains oxygen atoms. These additional oxygen atoms increase the electron-withdrawing effect on the central sulfur atom in the molecule. As a result, the sulfur becomes more electron deficient, making it more willing to donate a proton.
Additionally, your second approach to compare the acidity by looking at the product of their reaction with water is correct. When both SO2 and SO3 react with water, they form sulfurous acid (H2SO3) and sulfuric acid (H2SO4), respectively. Sulfuric acid (H2SO4) is a strong acid, while sulfurous acid (H2SO3) is a weak acid. Therefore, based on the products, we can conclude that SO3 is more acidic than SO2.
In summary, you can determine that SO3 is more acidic than SO2 by considering the higher oxidation state of sulfur in SO3 and its ability to form a stronger acid when reacting with water.