Acid Base Equilibria-Module 1

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

No. of Questions= 4


1.  A 0.100 M solution of a weak monoprotic acid has a pH of 3.30. What is the equilibrium constant, Ka, for this acid?
a) 108.9
b) 5.0 x 10-3
c) 5.0 x 10-4
d) 2.5 x 10-7
e) 2.5 x 10-6
2.  What is the pH of a 0.100 M solution of pyruvic acid, HC3H3O3? (Ka = 1.4 x 10-4)
a) 1.93
b) 2.43
c) 3.85
d) 4.85
e) 7.00
3.  What is the pH in a titration when 20.0 mL of 0.0150 M KOH has been added to 35.0 mL 0f 0.0100 M HCl? (Note that the resulting salt is neutral)
a) 2.26
b) 2.20
c) 2.85
d) 3.04
e) 2.00
4.  Given the equilibrium constants for the following equilibria at 25oC,

H+1(aq) + SO3-2(aq) dblaro.jpg (896 bytes) HSO3-1 (aq)          K = 1.59 x 10+7

H-+1(aq) + HSO3-1 (aq) dblaro.jpg (896 bytes)H2SO3 (aq)       K = 7.69 x 10+1

calculate the K at 25oC for the following reaction.

H2SO3 (aq) dblaro.jpg (896 bytes)2 H+1(aq) + SO3-2(aq)

a) 1.22 x 109
b) 8.18 x 10-10
c) 2.07 x 105
d) 4.84 x 10-6
e) 1.59 x 107



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