ACID-BASE REVIEW 2014
1. Define Arrhenius Acid and Base
Acid:
Base:
2. Define Bronsted-Lowry Acid and Base
Acid:
Base:
3. Define a Lewis Acid and Base
Acid:
Base:
4. Give some properties of an acid, and some of a base
Acid:
Base:
5. H3O+ is called:
6. OH- is called:
7. [OH-] = 3x10-3. Is it an acid, base or neutral solution?
8. [H]+= 6x 10-12. Is it an acid, base or neutral solution?
9. Give the pH of (use practice sheet to review; pH + pOH = 14)
a.
[H+] = .0001
b.
[OH-] = .001
c.
[H+] = 5.3 x 10-5
d.
[OH-] =3 x 10-4
10. Give an example of a monoprotic acid, diprotic acid and triprotic acid. (practice nomenclature of acids &
bases)
11. What does amphoprotic mean? To what type of materials does it apply?
12. Write the equation for the self-ionization of water.
13. Write the equation for the ionization of HCl in water.
14. Label conjugate acid-base pairs.
NH3 + H2O  NH4+ + OH15. Write the dissociation equation for KOH in water.(what ions form? Is the solution acidic or basic (alkaline))
16. Which is the strongest acid (same Molarity)?
Oxalic acid
[H+] = 9.5 x 10-3
Carbonic acid
[H+] = 2.24 x 10-6
17. Which is the strongest base (same Molarity)?
Ammonia
[H+] = 2.0 x 10-12
Ethylamine
[H+] = 4.47 x 10-13
18. Which is the color you would expect litmus paper to turn when exposed to an acid like orange juice?
19. In the following equation which is the conjugate base?
C2H3O2-1 + H2S  HC2H3O2 + HS-1
20. What role does H2O play in the following reaction?
H2O + H3PO4  H2PO4-1 + H3O+1
21. In the following equation which is the conjugate acid?
HNO3 + NH3  NH4+ + NO3-1
22. Underline the acids and cross out the bases:
NaCl
CH4
H3PO4
LiOH
H2O
HI
Cu(OH)2
LiBr
NH4NO3
Mg(OH)2
H2S
AgCl
ACID-BASE REVIEW 2014
1. Define Arrhenius Acid and Base
Acid: formula begins with “H” and produce hydrogen ions in solution
Base: formula ends with “OH” and produce hydroxide ions in solution
2. Define Bronsted-Lowry Acid and Base
Acid: proton donor
Base: proton acceptor
3. Define a Lewis acid and base: Lewis acid is an electron pair acceptor, Lewis base an electron pair donor
4. Give some properties of an acid, and some of a base
Acid: turn litmus red, taste sour, low pH, neutralize bases, react with metals to make H2 gas,
react with carbonates to produce carbon dioxide, a metal salt and water
Base: turn litmus blue, taste bitter, high pH, neutralize acids, turn phenolphthalein from clear to
pink
5. H3O is called: hydromium ion or a hydrated hydrogen ion
6. OH- is called: hydroxide ion
7. (OH-) = 3x10-3. Is it an acid, base or neutral solution? pOH about 3; pH about 11 so … BASIC
8. (H)+= 6x 10-12. Is it an acid, base or neutral solution? pH about 12; pH = 11.22
so … BASIC
9. Give the pH of (use practice sheet to review; pH + pOH = 14)
a. [H+] = .0001
pH = 4
b.
[OH ] = .001
pH = 11
pOH = 3
c.
[H+] = 5.3 x 10-5 pH = 2.28
pOH = 3.52
d.
[OH-] =3 x 10-4
pH = 10.48
10. Give example of monoprotic acid, diprotic acid. (practice nomemclature of acids & b ases)
Monoprotic = HCl, HNO3, Diprotic = H2SO4, H2CO3
11. What does amphoprotic mean?
Can act as both a proton donor and a proton acceptor (L-B Theory) ex: HS-, H2O, H2PO412. Write the equation for the ionization of water.
HOH(l)   H+(aq) + OH-(aq)
13. Write the equation for the ionization of HCl in water.
HCl(aq)   H+(aq) + Cl-(aq)
14. Label conjugate acid-base pairs.
NH3 + H2O  NH4+ + OHbase acid
C acid
C base
15. Write the dissociation equation for KOH in water. KOH(s)  K+(aq) + OH-(aq) ; the solution is basic
since there are more hydroxide ions
16. Which is the strongest acid (same Molarity)?
Oxalic acid
[H+] = 9.5 x 10-3
Carbonic acid
[H+] = 2.24 x 10-6
Oxalic it has the lower pH
23. Which is the strongest base (same Molarity)?
Ammonia
[H+] = 2.0 x 10-12
Ethylamine
[H+] = 4.47 x 10-13
Ethylamine since it has the lower pH
24. Which is the color you would expect litmus paper to turn when exposed to an acid like orange juice?
Red
25. In the following equation which is the conjugate base?
C2H3O2-1 + H2S  HC2H3O2 + HS-1
HS-1 is the conjugate base
26. What role does H2O play in the following reaction?
H2O + H3PO4  H2PO4-1 + H3O+1
H2O acts as the base; H3O+ is the conjugate acid
27. In the following equation which is the conjugate acid?
HNO3 + NH3  NH4+ + NO3-1
NH4+ is the conjugate acid
28. Underline the acids and cross out the bases:
NaCl
CH4
H3PO4
LiOH
H2O
HI
Cu(OH)2
LiBr
NH4NO3
Mg(OH)2
H2S
AgCl