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When carbon dioxide “dissolves” in water, essentially all

An Introduction to Thermal Physics | 1st Edition | ISBN: 9780201380279 | Authors: Daniel V. Schroeder ISBN: 9780201380279 40

Solution for problem 91P Chapter 5

An Introduction to Thermal Physics | 1st Edition

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An Introduction to Thermal Physics | 1st Edition | ISBN: 9780201380279 | Authors: Daniel V. Schroeder

An Introduction to Thermal Physics | 1st Edition

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Problem 91P

Problem 91P

When carbon dioxide “dissolves” in water, essentially all of it reacts to form carbonic acid, H2CO3:

CO2(g) + H2O(1) ↔ H2CO3(aq).

The carbonic acid can then dissociate into H+ and bicarbonate ions,

H2CO3(aq) ↔ H+(aq) + HCO−(aq).

(The table at the back of this book gives thermodynamic data for both of these reactions.) Consider a body of otherwise pure water (or perhaps a raindrop) that is in equilibrium with the atmosphere near sea level, where the partial pressure of carbon dioxide is 3.4 × 10−4 bar (or 340 parts per million). Calculate the molality of carbonic acid and of bicarbonate ions in the water, and determine the pH of the solution. Note that even “natural” precipitation is somewhat acidic.

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Textbook: An Introduction to Thermal Physics
Edition: 1
Author: Daniel V. Schroeder
ISBN: 9780201380279

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When carbon dioxide “dissolves” in water, essentially all