Acid Base Equilibria-Module 3

Course Name:  Chemistry
Course No.132 NT
Teacher:  Bill Cook
Teacher's Email:  bcook@icc.edu

No. of Questions= 4


1.  What is the pH of a solution that is 0.100 M in acetic acid acid and 0.50 M in sodium acetate? (Ka = 1.8 x 10-5)
a) 7.00
b) 5.00
c) 4.04
d) 4.74
e) 5.44
2.  Which of the following statements is true of the titration of a weak monoprotic acid by a strong base such as sodium hydroxide?
a) At the equivalence point, the pH is 7.
b) The moles of acid are greater than the moles of base at the equivalence point.
c) The moles of base are greater than the moles of acid at the equivalence point.
d) The moles of acid equal the moles of base at the equivalence point.
e) The solution is acidic at the equivalence point.
3.  What is the pH of a solution which is 0.0100 M in HA and also 0.0020 M in NaA    (Ka = 9.0 x 10-6)?
a) 2.40
b) 4.35
c) 5.65
d) 6.65
e) 7.15
4.  What is the [H3O+1] concentration in a solution resulting from mixing 100.0 mL of 0.100 M HCN and 10.0 mL 0f 0.100 M KOH?  (Ka for HCN = 4.0 x 10-10.)
a) 9.1 x 10-3
b) 8.2 x 10-5
c) 5.7 x 10-6
d) 2.0 x 10-8
e) 3.6 x 10-9



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