Chapter 10 and 11 Review
1. According the Arrhenius’s view of acids a bases
a. An acid was what?
b. A base was what?
2. According to Bronsted- Lowry,
a. An acid was what?
b. A base was what?
3. Put in order of increasing Conjugate Base strength, the following acids:
a. H2SO3, H2SO4
b. HNO2, HNO3
c. HClO2, HClO4, HClO, HClO3
4. Write a Bronsted Lowry for each species in the following equations. Label the acids and
bases using Bronsted Lowry theory terminology.
a. H2O + H2O  H3O+ + OH-
b. HCl + H2O  H3O+ + Cl-
c. NH3 + H2O  NH4+ + OH-
d. NH3 + HCl  NH4Cl
5. Calculate the molarity of the following aqueous solutions.
a. 10.5 g KCl in 250.0 ml of solution
b. 30.7 g LiClO4 x 3 H2O in 125 ml of solution
c. 25.0 ml of 1.50 M HNO3 diluted to 0.500 L
d. 15.0 g CaCl2 in 0.350 L solution
e. 4.66 g Mn(NO3)2 x 2 H2O in 185 ml of solution
f.
35.0 ml of 6.00 M H2SO4 diluted to 250. ml
6. How many milliliters of 0.250 M NaCl solution must be measured to obtain 0.100 mol of
NaCl?
7. A student needs to prepare 250. ml of 0.100 M Cd(NO3)2 solution. How many grams of
cadmium nitrate are required?
8. How many grams of CaCl2 are needed to prepare 250. ml of 0.125 M CaCl2 solution?
9. How can we prepare 100. ml of 0.0400 M K2Cr2O7 from 0.200 M K2Cr2O7?
10. How could 100. ml of 0.125 M H2SO4 solution be made from 0.500 M solution?
11. How many milliliters of 0.124 M NaOH are required to react with H2SO4 if you have 15.4
ml of 0.108 M H2SO4?
12. How many milliliters of 0.100 M AgNO3 solution are needed to react completely with
25.0 ml of 0.400 M CaCl2 solution?
13. How many milliliters of 0.500 M KOH are needed to react completely with 60.0 ml of
0.250 M FeCl2 solution to precipitate Fe(OH)2?
14. A 25.00 ml portion of an HCl solution is transferred to a flask, and after a few drops of
indicator are added, the HCl solution is titrated with 0.0775M NaOH solution. The
titration requires exactly 37.46 ml of the standard NaOH solution. What is the molarity
of the HCl solution?
15. In a titration, a sample of H2SO4 solution having a volume of 15.00 ml required 36.42 ml
of 0.147 M NaOH solution for complete neutralization. What is the molarity of the
H2SO4 solution?
16. Stomach acid is hydrochloric acid. A sample of gastric juice having a volume of 5.00 ml
required 11.00 ml of 0.0100 M KOH solution for neutralization in a titration. What was
the molar concentration of HCl in this fluid?
17. In a titration, 23.25 ml of 0.105 M NaOH was needed to react with 21.45 ml of HCl
solution. What is the molarity of the acid?
18. Suppose you have 1.034 g of clover leaves and you extract the oxalic acid from them into
a small amount of water. This solution of oxalic acid is found to require 34.47 ml of
0.100 M NaOH to the end point. What is the weight percent of oxalic acid in the leaves?
19. An acid such as HCl can be standardized by using it to titrate a base such as Na2CO3.
Sodium carbonate is a solid that can be obtained in pure form and can be weighed
accurately. If you find that 0.250 g of Na2CO3 requires 25.76 ml of HCl for titration to
the end point, what is the exact molarity of the HCl?
20. Hydrochloric acid, HCl, can be purchased from chemical supply houses in solutions that
are exactly 0.100 M, so these solutions can be used to standardize the solution of a base.
If you titrate to the end point 25.00 ml of a sodium hydroxide solution with 32.56 ml of
0.100 M HCl, what is the concentration of the base?
21. How many milliliters of 0.250 M HCl would be required to neutralize completely 2.50 g
of NaOH?
22. How many milliliters of 0.250 M HCl would be required to neutralize completely 36.5 ml
of 0.100 M NaOH?
23. You dissolve 2.50 g of Ba(OH)2 in enough water to make 250. ml of solution. How
many moles of HCl would be required to neutralize this solution? If the HCl solutions is
0.110M, how many milliliters would be required to neutralize the Ba(OH)2 solution?
24. Sodium carbonate, Na2CO3, is a good compound to use to standardize acid solutions. If
42.23 ml of HCl solution are used to titrate 0.251 g of Na2CO3 to the end point, what is
the molar concentration of the acid?
25. Potassium acid phthalate, KHC8H4O4, is used to standardize solution of bases. The acidic
anion reacts with bases according to the following equation. If a 0.902 g sample of
potassium acid phthalate is dissolved in water and titrated to the end point with 39.45 ml
of NaOH, what is the molarity of the NaOH?
KHC8H4O4
+
NaOH 
H2O
+
NaKC8H4O4
26. A soft drink contains an unknown amount of citric acid, C6H8O7. If 100. ml of the soft
drink require 36.51 ml of 0.0102 M NaOH to neutralize completely the citric acid, how
many grams of citric acid does the soft drink contain per 100. ml? What is the molarity
of the citric acid?
C6H8O7 +
NaOH 
Na3C6H5O7
+
H2O
27. Tartaric acid which can be found in wine and many fruits, has the formula C4H6O6, and it
reacts with sodium hydroxide according to the following equation. You are given 1.036
g of an impure sample of the acid. If the sample requires 25.95 ml of 0.467 M NaOH for
titration to the equivalence point, what is the percent weight of tartaric acid in the
sample?
C4H6O6 +
NaOH 
Na2C4H4O6
+
H2O