Acid/ Base Review
Problems
1. Explain ,by reacting HSO4 - with water, how it acts as an acid.
2. After addition to the unknown solution, methyl violet was blue, methyl orange was yellow,
methyl red was red, and phenolphthalein was colorless. What is the ph of the unknown solution?
3. Predict the predominate acid-base reaction between:
A) sodium hydrogen sulfate and sodium hydroxide
B) methanoic acid with sodium hydrogen sulfide
4. Answer the following questions about the pH curve below:
A. What is the titrant?
B. What is the sample being titrated?
C. What indicator could be used?
D. Is there a polyprotic substance involved?
E. What is/are the endpoint(s)?
F. What is/are the equivalence point(s)?
image from chem. guide
5. Predict the acid- base reaction when small amounts of NaOH are added to a
carbonic acid - hydrogen carbonate buffer.
6. Chemical analysis of stain remover containing oxalic acid was conducted. 10. ml Oxalic acid
was titrated with 0.485 mol/L potassium hydroxide to the second endpoint with phenolphthalein.
Calculate the concentration of oxalic acid in the stain remover.
Trial
1
2
3
Final buret reading (ml)
17.1
32.7
48.3
Initial buret reading (ml)
1.4
17.1
32.7
7. What is an Arrhenius base?
8. If 26 g of sodium hydroxide is added water to make 150 ml of solution. What are the pH
and pOH of this solution?
9. The hydrogen ion concentration of a 0.100 mol/L solution of propanoic acid is
1.16 X 10-3 mol/L. Calculate the Ka.
10. In a 0.1M solution of methanoic acid, the hydrogen ion concentration is 3.2 X 10-3 mol/L
Calculate the Ka for methanoic acid.
11. Calculate the [OH-] for
a. pH of 4.60
b. pH of 9.30
12. Using Bronsted-Lowry and a reaction, illustrate how NH3 behaves as a base.