Chemistry 12

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define the term strong bronsted lowry acid

it is 100% ionized in solution? is that it?

  • Chemistry 12 -

    Strong bronsted lowry acids are H+ donors, bases are proton acceptors. Lewis acids are electron pair acceptors, and Lewis bases are electron pair donors.

  • Chemistry 12 -

    Thank you soo much, that makes so much sense :)

  • Chemistry 12 -

    But saying completely ionized is not necessarily correct. A strong acid such as HCl will be completely ionized in the presence of a weak or a strong base, but a strong acid like H3PO4 will give up the its first proton readily in a solution with a weak or strong base, but its conjugate acid will not readily due so with the weak base. So, saying completely ionized isn't necessarily correct, but saying readily able to give up A proton with a weak base such as H20, which can act as an acid or a base, is better. I could be wrong, but this is the way I understand it.

  • Chemistry 12 -

    Thank you soo much :) I can totally see you as a smart Chemist in the future :)

  • Chemistry 12 -

    I'm actually a biochemist, I just haven't been immersed in some of this stuff in a while. My last post should read conjugate base not acid. Sorry for that, I'm a little prone to typos and brain farts when I'm a little tired.

  • Chemistry 12 -

    Although all of H3PO4 is completely ionized (i.e, -H2PO4,) it can not give up the rest of its H+ readily.

  • Chemistry 12 -

    and when you think of strong bronsted lowry acid you think of strong proton donors.

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