Chemistry: An Atoms-Focused Approach
Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393912340
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster
Publisher: W. W. Norton & Company
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Chapter 10, Problem 10.113QA
Interpretation Introduction

To find:

Henry’s law constant (kH) in molL×atm for O2 dissolved in blood at 37.

Expert Solution & Answer
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Answer to Problem 10.113QA

Solution:

The value for the Henry’s law constant for dissolved O2 in arterial blood is

7.8 x 10-3molL ×atm

Explanation of Solution

1) Concept:

Henry’s law states that, the solubility of any gas in a liquid is directly proportional to its partial pressure of the gas above the surface of the liquid.

Cgas=kH × Pgas

Where, Cgas is the solubility of gas in a particular solvent in mol/L, kH is the Henry’s gas constant, Pgas is the partial pressure of gas in the aqueous solution in atm.

2) Given:

Arterial blood contains 0.25g O2/L

3) Calculations:

Cgas=kH×Pgas

The Cgas has the unit mol/L. So, we must first find the molarity of O2 in blood. Using molar mass of O2, we calculate moles of O2 and then molarity as follows:

0.25 g O2 ×  1 mol O231.998 g O2=  0.00781298 mol O2

Molarity=mol of O2L of blood =0.00781298 mol O21 L blood= 0.00781298 molL

Inserting the values of Cgas and Pgas = 1 atm, we get the Henry’s law constant for O2 as follows:

Cgas=kH×Pgas

0.00781298 molL=kH ×1 atm

kH=0.00781298molL ×atm

(A mole is the SI unit of amount chemical substance. When writing units, it is written as “mol”.)

Conclusion:

The value for the Henry’s law constant for dissolved O2 in arterial blood is

7.8 x 10-3molL ×atm

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Chapter 10 Solutions

Chemistry: An Atoms-Focused Approach

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