ACID-BASE TITRATIONS pH REVIEW 2014
1. Define Arrhenius Acid and Base
Acid:
Base:
2. Define Bronsted-Lowry Acid and Base
Acid:
Base:
3. Give several properties of an acid, and a base (which one is “alkali”)
Acid:
Base:
4. H3O+ is called ___________ is what forms when __________ ions combine with a water molecules
5. OH- is called:
6. [OH-] = 3x10-3. Is it an acid, base or neutral solution?
7. [H]+= 6 x 10-12. Is it an acid, base or neutral solution?
Calculate the pH
Calculate the pH
8. 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
9. Give example of monoprotic acid, diprotic acid. (practice nomemclature of acids & b ases)
10. What does amphoteric mean? (give an example of an amphoteric species (molecule or ion)
11. Write the equation for the ionization of water.
What is the equilibrium constant for water ( kw = ? )
12. Write the equation for the ionization of HCl in water.
13. Label conjugate acid-base pairs.
NH3 + H2O  NH4+ + OH14. Write the dissociation equation for KOH in water ?.
15. Which is the strongest acid?
Oxalic acid Ka = 5.6 x 10-2
Carbonic acid Ka = 4.3 x 10-7
16. Be able to identify the parent acid and base of a salt. Know the short list of strong acids and bases.
What is the difference between a “strong” acid and a concentrated acid?
If CuSO4 is dissolved in water, is the solution acid, basic or neutral?
17. If NaCl is dissolved in water, is the solution acid, basic or neutral?
18. What is the Molarity of HCl if 40 ml of HCl neutralizes 120 ml of 3 M NaOH?
More titration practices:
Remember: volume times concentration of acid = volume times concentration of base
Or milliliters time Molarity = milliliters times Molarity
mlA MA = mlB MB
19. How many ml of .25 M HCl would be needed to neutralize 30.0 ml of .15 M NaOH?
20. If 45.4 ml of 0.5 M NaOH is used to neutralize 10.0 ml of acetic acid solution; what is the
molarity of the acetic acid?
Vinegar from the store is 5% acetic acid (.83 M); HAS THIS “VINEGAR” BEEN WATER DOWN OR
CONCENTRATED?
21.
25.0 ml of 0.25 M H2SO4 is to be titrated with a mono hydroxyl base of about 0.05 M
concentration. How much base should we expect to use? (remember what kind of acid is sulfuric acid)
22. Review rules of Nomenclature (when to use roman numerals, when to use “hydro”, when
to use a prefix (like mono, di , tri, tetra ) Name the following:
H3P
Na2SO4
Li2S
CO2
NHO3
Cu(OH)2
FeBr3
MgO
Ba(OH)2
CS2
HClO3
CoCl2
K3PO4
FeCl3
NaCl
AgNO3
(Now go back and circle the acidic salts, and underline the basic salts)
23. Review the notes and practice sheet on predicting and balancing reactions
Acids and bases neutralize to produce a __________ and __________.
Acids and a metal react to produce __________ gas and a _______________.
Acids and a carbonate react to produce _______ , _________ gas and a ________.
Predict and balance the following:
___ H3P + ___ Li2CO3 
___ H2O
+
___ _____ +
___ ________
ACID-BASE TITRATIONS pH REVIEW 2014 ANSWERS
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. Give several properties of an acid, and a base (which one is “alkali”)
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 phenolpthalien from clear to pink
4. H3O+ is called _ hydromium ion _ is what forms when _ hydrogen _ ions combine with a water
molecules aka a hydrated hydrogen ion
5. OH- is called: hydroxide ion
6. [OH-] = 3x10-3. Is it an acid, base or neutral solution? pOH about 3; pH = 11.48 so … BASIC
7. [H]+= 6 x 10-12. Is it an acid, base or neutral solution? pH about 12; pH = 11.22
so … BASIC
8. 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
9. Give example of monoprotic acid, diprotic acid. (practice nomemclature of acids & bases)
Monoprotic = HCl, HNO3, Diprotic = H2SO4, H2CO3
10. What does amphoteric mean? (give an example of an amphoteric species (molecule or ion)
Can act as both a proton donor and a proton acceptor (L-B Theory) ex: HS-, H2O, H2PO411. Write the equation for the ionization of water. What is the equilibrium constant for water ( kw = ? )
HOH(l)   H+(aq) + OH-(aq)
12. Write the equation for the ionization of HCl in water.
HCl(aq)   H+(aq) + Cl-(aq)
13. Label conjugate acid-base pairs.
NH3 + H2O  NH4+ + OHbase acid
acid
base
14. Write the dissociation equation for KOH in water ?. KOH  K+ + OH15. Which is the strongest acid?
Oxalic acid Ka = 5.6 x 10-2
Carbonic acid Ka = 4.3 x 10-7 Oxalic acid because it has a higher dissociation constant; it will
form more ions in solution and not stay together in the molecular form
16. Be able to identify the parent acid and base of a salt. Know the short list of strong acids and bases.
What is the difference between a “strong” acid and a concentrated acid?
A “strong” acid or base completely dissociated to form ions, a weak one stays in its molecular form until called
upon. Concentrated is a measure of how many moles per volume)
If CuSO4 is dissolved in water, is the solution acid, basic or neutral? Acidic; its parent acid is strong
17. If NaCl is dissolved in water, is the solution acid, basic or neutral? Neutral both parents are strong
18. What is the Molarity of HCl if 40 ml of HCl neutralizes 120 ml of 3 M NaOH? 9 M HCl; use 1/3 as
much so 3 times more concentrated
More titration practices:
Remember: volume times concentration of acid = volume times concentration of base
Or milliliters time Molarity = milliliters times Molarity
mlA MA = mlB MB
19. How many ml of .25 M HCl would be needed to neutralize 30.0 ml of .15 M NaOH?
mlA MA = mlB MB
mlA (.25M) = 30 ml (.15M)
mlA = 18 ml
If 45.4 ml of 0.5 M NaOH is used to neutralize 10.0 ml of acetic acid solution;
20.
mlA MA = mlB MB
10ml (MA) = 45.4 ml (.5M)
MA = 2.27 M
what is the molarity of the acetic acid?
Vinegar from the store is 5% acetic acid (.83 M); HAS THIS “VINEGAR” BEEN WATER DOWN OR
CONCENTRATED? Concentrated; from the store it’s only 5% or .83 Molar
21.
25.0 ml of 0.25 M H2SO4 is to be titrated with a mono hydroxyl base of about 0.05 M
concentration. How much base should we expect to use? (remember what kind of acid is sulfuric acid)
The H2SO4 acts like it’s double the concentration, .25 moles makes .5 moles of H+ ions
mlA “effective”MA = mlB MB
25.0 ml (0.50 M) = ? ml (. 05M)
mlB = 250 mL
22. Review rules of Nomenclature (when to use roman numerals, when to use “hydro”,
when to use a prefix (like mono, di , tri, tetra ) Name the following:
H3P hydro phosphoric acid
Na2SO4
HNO3 Nitric acid
Cu(OH)2 copper hydroxide
FeBr3 iron (III) bromide MgO
magnesium oxide
Ba(OH)2
CS2
HClO3
cobalt (II) chloride
K3PO4
barium hydroxide
potassium phosphate
Li2S
sodium sulfate
carbon di sulfide
FeCl3
NaCl
iron (III) chloride
lithium sulfide
chloric acid
sodium chloride
CO2
carbon di oxide
CoCl2
AgNO3
silver (I) nitrate
(Now go back and circle the acidic salts, and underline the basic salts)
23. Review the notes and practice sheet on predicting and balancing reactions
Acids and bases neutralize to produce a __salt____ and ___water_____.
Acids and a metal react to produce ____hydrogen___ gas and a ____ salt _____.
Acids and a carbonate react to produce _ water __ , _carbon di oxide_ gas and a __salt__.
Predict and balance the following:
_2_ H3P + _3_ Li2CO3 
_3_ H2O
+
_3_ _CO2____ +
_2_ ___Li3P_____