(a) Step 1: Explanation We can first use Henry’s Law to determine the concentration of CO 2 dissolved in solution: Solubility = kP The amount of CO 2 in the atmosphere is 750 ppm. P C O 2 = 750 × 10 − 6 a t m = 0.00075 a t m Solubility = ( 3.2 × 10 − 2 m o l / L a t m ) ( 0.00075 a t m ) = 2.4 × 10 − 5 M (b) Step 2: To classify: The pH of rain using the concentration of H 2 CO 3 . We are told that all of the CO 2 that was dissolved converted to H 2 CO 3 , therefore, we know [ H 2 C O 3 ] = 2.4 × 10 − 5 M . We can now determine the equilibrium concentration of the various species in solution: H 2 C O 3 + H 2 O ⇌ H 3 O + + H C O 3 − K a = 4.3 × 10 − 7 To determine the equilibrium concentrations of a solution, we can use an ICE table: H 2 CO 3 H 3 O+ HSO 3 - I 2.4 x 10-5 0 0 C - x + x + x E 2.4 x 10-5 − x x x We now know the equilibrium concentrations and can use the equilibrium expression to solve for the variable x : K a = [ H + ] [ H C O 3 − ] / [ H 2 C O 3 ] 4 Interpretation Introduction (c) Step 3: To classify: If the increasing CO 2 level has an effect on rain pH.

7th Edition

ISBN: 9780321940872

Author: John E. McMurry, Robert C. Fay, Jill Kirsten Robinson

Publisher: PEARSON

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Chapter 15, Problem 15.32P

(a)

Step 1:

Interpretation Introduction

To classify:

The solubility of CO₂ using Henry’s Law.

Interpretation Introduction

(c)

Step 3:

To classify:

If the increasing CO₂ level has an effect on rain pH.

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Chapter 15, Problem 15.31P

Chapter 15, Problem 15.33P

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To classify: The solubility of CO 2 using Henry’s Law.