easy acid-base question?
As we all know H2(SO4) completely dissociates to HSO4- + H+ and then HSO4- goes to equilibrium through the equation HSO4- <-----> H+ + SO42-
But how come Sr(OH)2 which is a strong base when dissociates doesnt completely dissociates to SrOH+ and OH- and instead completely dissociates to Sr2+ and 2(OH)-? Is it because SrOH+ a strong base or something?? please help me so confused
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Because Sr(OH)2 is an ionic compound and ionic compounds completely dissociate when they dissolve in water. Acids are not ionic compounds but are molecules that have an extremely polar bond. In H2SO4, SO4 group really attracts electrons, so the covalent bond with hydrogen essentially gets ripped off the hydrogen. But after it takes the electrons from the first H+, the SO4 group becomes negative, making it difficult to attract electrons with the same strength (electrons are negatively charged), so the second bond with H doesn't get "ripped off' the H with the same strength, making it a weak acid.
Very rudimentary answer, but hope it helps. The key difference is that Strontium Hydroxide is a soluble ionic compound whereas sulfuric acid is a molecule.
Why do you have to know? Can't you just accept that it does?