Chapter 15 Flashcards
T/F: In any substance, an Arrhenius acid produces H+, while and Arrhenius base either accepts an H+ or produces an OH-.
F. The Arrhenius model works only in aqueous solutions.
T/F: An acid-base reaction uses double harpoons, not one-way arrows.
F. Any reaction that involves a strong acid or base will proceed to completion, so those use one-way arrows. Any reaction that is in equilibrium, though, will use the double harpoons.
List the strong six.
HBr HCl HI H2SO4 "sulfuric" HClO4 "perchloric" HNO3 "nitric"
Invent at least three strong bases.
Any group 1A or 2A hydroxides will work!
T/F: A Brønsted-Lowry acid can donate H+, while a Brønsted-Lowry base can accept an H+.
T. Keep in mind that once a Brønsted-Lowry base accepts an H+, it becomes an acid, because it can now donate it back (and vice-versa).
T/F: The Brønsted-Lowry acid-base model is not limited to aqueous solutions.
T.
T/F: A conjugate acid-base pair differs only by an H+.
T.
T/F: K_a is only used for reactions involving weak acids.
T. It doesn’t involve any bases, that would be K_b. Also, since K_a is an equilibrium constant, it can’t involve strong acids, since those go to completion and not equilibrium.
T/F: A strong acid can never be a conjugate with a strong base, and a weak acid can never be a conjugate with a weak base.
T.
EQUATION K_a and K_b
([products]^coefficient) / ([reactants]^coefficient)
T/F: A substance that can act as both an acid and a base is said to be an amphitheater.
F: It is said to be amphiprotic.
Why does an acid-base equilibrium favor the side with weaker acids and bases?
Because those weak acids and bases are too lazy to accept/donate H+, so they rarely move to the other side.
What are the three equations that relate pH and POH?
(1) -log[H3O+] = pH ; 10^-pH = [H3O+]
(2) [H3O+] x [OH-] = K_w
(3) -log[OH-] = pOH ; 10^-pOH = [OH-]
K_w is always equal to
1.0 x 10^-14
