Titration Problems
1. In a titration, 27.4 ml of 0.0154 M Ba(OH)2 is added to a 20.0 ml sample of HCl
solution of unknown concentration. What is the molarity of the acid solution?
Ba(OH)2
+
HCl 
H2O +
BaCl2
2. A 15.5 ml sample of 0.215 M KOH solution required 21.2 ml of aqueous acetic
acid solution in a titration experiment. Calculate the molarity of the acetic acid
solution.
KOH +
CH3COOH 
H2O +
KC2H3O2
3. By titration, 17.6 ml of aqueous H2SO4 neutralized 27.4 ml of 0.0165 M LiOH
solution. What was the molarity of the aqueous acid solution?
LiOH +
H2SO4 
Li2SO4 +
H2O
4. If 20.0 ml of 0.0100 M aqueous HCl is required to neutralize 30.0 ml of an
aqueous solution of NaOH, determine the molarity of the NaOH solution.
HCl +
NaOH 
H2O +
NaCl
5. Suppose that 20.0 ml of 0.10 M Ca(OH)2 is required to neutralize 12.0 ml of
aqueous HCl solution. What is the molarity of the HCl solution?
Ca(OH)2
+
HCl 
H2O +
CaCl2
6. Suppose that 15.0 ml of 2.50 x 10-2 M aqueous H2SO4 is required to neutralize
10.0 ml of an aqueous solution of KOH. What is the molarity of the KOH
solution?
H2SO4 +
KOH 
H2O +
K2SO4
7. In a titration experiment, a 12.5 ml sample of 1.75 x 10-2 M Ba(OH)2 just
neutralized 14.5 ml of HNO3 solution. Calculate the molarity of the HNO3
solution.
Ba(OH)2
+
HNO3 
Ba(NO3)2
+
H2 O
8. If 20.0 ml of a 0.300 M solution of NaOH is required to neutralize 30.0 ml of a
sulfuric acid solution, what is the molarity of the H2SO4 solution?
NaOH +
H2SO4 
Na2SO4
+
H2O
9. What volume in milliliters of 0.500 M HNO3 is required to neutralize 25.0 ml of a
0.200 M NaOH solution?
HNO3 +
NaOH 
NaNO3
+
H2O
10. In a laboratory experiment, 20.0 ml of NH3 solution is titrated to the methyl
orange endpoint using 15.65 ml of a 0.200 M HCl solution. What is the
concentration of the aqueous ammonia solution?
NH3 +
HCl 
NH4Cl
11. How many grams of KOH are required to neutralize 200.0 ml of a 4.00 M
solution of HNO3?
KOH +
HNO3 
KNO3 +
H2O
12. How many liters of a 1.500 M sulfuric acid solution are needed to completely
neutralize 220 ml of a 6.5 M solution of NaOH?
NaOH +
H2SO4 
H2O +
Na2SO4
13. In a laboratory experiment, a student neutralizes a 15.00 ml sample of vinegar
with 31.85 ml of a 0.400 M NaOH solution. Calculate the molarity of the
solution.
CH3COOH +
NaOH 
H2O +
NaCH3COO
14. What mass of barium chloride, BaCl2, is required to completely precipitate the
barium sulfate from 35.0 ml of 0.200 M H2SO4?
BaCl2 +
H2SO4 
BaSO4 +
HCl
15. What is the molarity of NaOH solution if 25.0 ml is required to completely
neutralize 40.0 ml of a 1.50 M solution of H2SO4?
NaOH +
H2SO4 
H2O +
Na2SO4
16. Calculate the milliliters of a 0.600 M solution of HNO3 necessary to neutralize
28.55 ml of a 0.450 M solution of KOH.
HNO3 +
KOH 
KNO3 +
H2O
17. How many grams of calcium hydroxide (Ca(OH)2) are required to neutralize
52.68 ml of a 0.750 M H2SO4 solution?
Ca(OH)2
+
H2SO4 
H2O +
CaSO4
18. In the titration of 25.0 ml of 0.1000 M HCl with 0.100 M NaOH, what is the pH
after 15.0 ml of the NaOH solution has been added?
HCl +
NaOH 
H2O +
NaCl
19. In the titration of 25.00 ml of 0.1000 M HCl with 0.1000 M NaOH, what is the
pH after 20.0 ml of the standard NaOH has been added?
HCl +
NaOH 
H2O +
NaCl
20. In the titration of 25.0 ml of 0.100 M HCl with 0.25 M NaOH, what is the pH
after 35 ml of NaOH solution has been added?
HCl +
NaOH 
H2O +
NaCl