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Metal and non-metal oxides and water reaction?

  1. Jan 21, 2013 #1
    1. The problem statement, all variables and given/known data
    I understand how metallic oxide dissolve in water to produce OH- ion due to high electronegativity of oxygen. But I am having trouble understanding how non-metallic oxide dissolve in water to form acid?
    For Homework I have to explain the reaction of Sulfur trioxide in water and how that produces H+ and sulfate ions.But I have no idea how to go on about this

    2. Relevant equations3. The attempt at a solution

    SO3 + H2O=> H2SO4
    and H2SO4=> H+ +HSO4-
    HSO4-=>H+ +SO4-

    I have no idea if these are correct or not? Also what makes the H2SO4 in the first reaction disassociate to ions?
     
  2. jcsd
  3. Jan 21, 2013 #2

    Borek

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    Staff: Mentor

    First and second equations are OK, the last one is not (charge is not balanced).
     
  4. Jan 21, 2013 #3
    So h+ so4-==> h+ + so4-2?
     
  5. Jan 21, 2013 #4
    I was also wondering when sulfur trioxide dissolves in water why does only one of the oxygen atoms in sulfur trioxide attaches to a hydrogen atom? why not the other 2
     
  6. Jan 21, 2013 #5

    Borek

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    Staff: Mentor

    Can't say it is much better. Please pay attention to how you format these things - some letters have to be capitalized, some characters should be made subscripts/supperscripts and so on.

    If you don't know how - [noparse]H3O+[/noparse] is displayed as H3O+.

    H2SO4 is most stable for energetic reasons. Both HSO4- and H3SO4+ exist, although the latter is observed only in pure sulfuric acid, never in water solutions.
     
  7. Jan 21, 2013 #6
    Okay thanks. Also do all non-metallic oxides have to be polar molecules in order to form an acid within water?
     
  8. Jan 21, 2013 #7

    Borek

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    Staff: Mentor

    I wouldn't call CO2 polar.
     
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