Question

(8 pts) Comparing dissociation constants, circle the strongest base in the following pairs. You must justify your reasoning a
6. (10 pts) Calculate Ka of a weak acid given that a 2.3 M HA solution has a pH of 1.55. Ka: 7, (10 pts) Calculate the pH of
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Answer #1

5)

A)

Kb of C5H5N = 1.5 x 10-9

Kb of NH3 = 1.8 x 10-5

If Kb values is large then that is strong base. So, Kb of NH3 is large . So it is strongest base

NH3 has strongest base

B)

HAsO42- is weak acid than HPO42- .The conjugate base of weak acid is strong base.

Here HAsO42- is weak.So the base of AsO43- is strongest base.

6)

Given data,

pH = 1.55

Concentration = 2.3 M

We know pH = -log(H+)

H+ = 10-1.55

H+ = x = 0.0281 M

We know , Ka = x2 / C - x

= ( 0.0281 )2 / 2.3 - 0.0281

= 0.0007896 / 2.271

Ka = 3.47 x 10-4

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