Acids and Bases

Acids and Bases

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  • Hey bro since we are sitting here waiting for our food, let me ask you a question. Do you know what a Bronsted-Lowry and Arrhenius acid and bases are?
  • Hmm... I think so. Arrhenius acid and bases Arrhenius acids contain hydrogen and ionize hydrogen ions.
  • Correct now give me some examples.
  • Uhhh I think HCl is an example of acids and NaOH is a base. Ooo I think I know the formulas too. Its HCl(g)->H+(aq)+Cl-(aq).
  • Yes. The equation for bases is NaOH(s)->Na+(aq)+OH-(aq). Do you know what Bronsted-Lowry acid an bases are?
  • Nope. I have no clue.
  • A Bronsted base is an expansion of Arrhenius acids and bases. The acids are hydrogen donors and the bases are hydrogen acceptors.
  • So one gives and one takes. Hm ok I'm getting the hang of it.
  • H-B+ is the conjugate acid and A- is the conjugate base.
  • HNO3 and H2O are examples. The set equation for Bronsted-Lowry is H-A + B->H-B+ + A-. H-A is the acid and B is the base.
  • Yes, or [H+]=10^-pH. Well our food is here. We can continue this later. Enjoy your "Bronsted" stew.
  • Time to get into pH. pH measures acidity/basicity as a function of the hydrogen ion in solution. It is the negative log of the concentration of H+ ions.
  • So... the formula would be... pH= -log[H+].
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