Acids and Bases Part 1 - Tri
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Transcript Acids and Bases Part 1 - Tri
Jackson Bettis
Michael Martzahn
Definitions
Acids are H+ donors. They give up H+ ions (protons)
Bases are H+ acceptors. They are compounds that
snatch up H+ ions.
Conjugate Acids donate protons in the forward
chemical reaction
Conjugate Bases accept protons in the forward
chemical reaction
Identification
Acids have an H in front usually
Acids have a pH of less than 7
Bases have an OH sometimes
Bases have a pH of more than 7
Conjugate Bases of strong acids are terrible bases that
have no effect on pH
Conjugate Bases of weak acids are weak bases and thus
do affect pH
Identification, cont.
Conjugate acids of weak bases are weak acids and do
affect pH
What it means to be a strong acid
Strong Acids dissociate completely in water
Therefore, they give up more protons than weak acids
The Six Strong Acids
HCl
HNO3
H2SO4
HClO4
HI
HBr
Acid dissociation reaction in water
H2O <-> H+ + OH Therefore, water can act as a base or an acid
Kw
Kw = 1.0 * 10-14
Kw / [OH-] = [H+]
Kw / [H+] = [OH-]
-log[H+] = pH
-log[OH-] = pOH
pH + pOH = 14
Writing Ka expressions
Ka = [H+][A-] / [HA]
Kb = [OH-][HB+] / [B]
Ka * Kb = Kw
Calculating pH
For strong acids: -log[H+]
For strong bases: -log[OH-]
For weak acids or bases: ICE table
Calculating pH, cont.
1.) determine major species in solution
2.) Decide which species in the reaction will control
[H+]
3.) Set up an ICE table for the reaction to determine
[H+]
Calculating pH of buffers
Ex.) We add 0.05 mols of NaOH to a 500 mL solution
of 0.25 M HOCl and 0.20 M NaOCl. Assume no
volume change.
Sample problem :D
Calculate the pH of a 0.20 M solution of HF (Ka = 7.2 *
10-4)
Another Sample Problem
20. The ionization constant for acetic acid is 1.8 × 10–5; that
for hydrocyanic acid is 4 × 10–10. In 0.1 M solutions of
sodium acetate and sodium cyanide, it is true that
(a) [H+] equals [OH–] in each solution
(b) [H+] exceeds [OH–] in each solution
(c) [H+] of the sodium acetate solution is less than that of
the sodium cyanide solution
(d) [OH–] of the sodium acetate solution is less than that
of the sodium cyanide solution
(e) [OH–] for the two solutions is the same
Yet another sample problem
12. A solution prepared by mixing 10 mL of 1 M HCl
and 10 mL of 1.2 M NaOH has a pH of
(a) 0
(b) 1
(c) 7
(d) 13
(e) 14