Arkansas State University  Department of Chemistry and Physics
CHEM1013	Exam 3

Don't forget nomenclature of acids!!!

1.  Give the conjugate base for each acid below:    (8 points)

a)  HI

b)  H₂SeO₄

c)  CH₂O₂

d)  HPO₄^2-

2.  Give the conjugate acid for each base below:    (8 points)

a)  O^2-

b)  PH₃

c)  H₂S

d)  HSO₃^-

3.  Define the following as either acids or bases.   (4 points)

a)  Clorox, pH = 9.0

b)  vinegar, pH = 2.3

c)  eggs, pH = 7.8

d)  bananas, pH = 4.6

4.  Calculate the pH of a hydroiodic acid solution with a [H⁺] = 2.3 x 10^-2 M.   (4 points)

5.  Calculate the pH of a 0.0002 M KOH solution.   (6 points)

6.  For each pair of acids, circle the strongest one.   ( 2 points each)

a)  HBr / HI

b)  HBr / H₂Se

c)  HClO₃ / HClO₄

d)  H₃PO₄ / H₂SO₄

e)  H₃AsO₄ / H₃PO₄

7.  For each of the following, define the resulting solutions as either acidic, basic or neutral.  (2 points each)

a) NaOOCCH₃

b)  NO₂

c)  CaO

d)  ammonium bromide

e)  KCl

8.  Write the equilibrium equation and calculate the equilibrium concentrations of a 0.5 M HCN solution.  K_a = 4.0 x 10^-10    (10 points)

9.  Write the equilibrium equation and calculate the pH of a 0.6 M pyridine solution.  (10 points)  K_b = 2.0 x 10^-9  (Formula for pyridine is C₅H₅N)

10.  What is an adduct and what type of bond is formed between the acid and the base?  (4 points)

11. Calculate the K_a for a 0.3 M HF solution with a pH of 1.84.  (10 points)

12.  Draw a titration curve that would represent a titration of a strong acid with a weak base.  Label all parts and indicat the expected pH for the equivalence point.   (5 points)

13.  List the three acid base theories mentioned in class and define an acid and a base for each.  (9 points)

14. Define an amphoteric oxide.  (2 points)