posted by Darrin on .
Write the equation for the reaction associated with the Ka2 of sulfuric acid, H2SO4.
Write the equation for the reaction associated with the Kb2 of carbonate, CO32–.
1 H2SO4 ==> H^+ + HSO4^-
2 HSO4^ ==> H^+ + SO4^2-
1 is 100 ionized; therefore, there is no k1.
k2 = (H^+)(SO4^2-)/HSO4^-)
Do the same kind of thing with the hydrolysis of CO3^2-
1 CO3^2- + HOH ==> HCO3^- + OH^-
k1 = ....
2 HCO3^- + HOH ==> H2CO3 + OH^-
k2 = (H2CO3)(OH^-)/(HCO3^-) = ?
bob you are literally always wrong
DrBob222 is 100% correct. The acid will lose hydronium ions in water, whereas a base will gain hydronium ions in water; remember that the arrows must be pointing in both directions when writing these chemical equations due to equilibrium (strong acids and bases completely dissociate in water). It's actually not all that simple but best way to put it for those having difficulty understanding.
We Love you Bob, let the haters hate, they don't know what they're talking about
My Sapling grade is suffering, thanks Bob
I think Bob just put the equation in a different format than Sapling is asking for. I got
HSO4^- <--> SO4^2-(aq) + H^+(aq)
HCO3^-(aq) + H2O(l) <--> H2CO3(aq) + OH-(aq)
soooo he is kinda wrong?