# A liter of water at 25°C dissolves 0.0404 g O 2 when the partial pressure of the oxygen is 1.00 atm. What is the solubility of oxygen from air, in which the partial pressure of O 2 is 159 mmHg?

### General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
Publisher: Cengage Learning
ISBN: 9781305580343

### General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
Publisher: Cengage Learning
ISBN: 9781305580343

#### Solutions

Chapter
Section
Chapter 12.3, Problem 12.4E
Textbook Problem

## A liter of water at 25°C dissolves 0.0404 g O2 when the partial pressure of the oxygen is 1.00 atm. What is the solubility of oxygen from air, in which the partial pressure of O2 is 159 mmHg?

Expert Solution
Interpretation Introduction

Interpretation:

The solubility of Oxygen in water at 159 mmHg has to be calculated.

Concept Introduction:

Solubility of a gas in liquid is explained by Henry’s law which states –

“At a constant temperature, the amount of a gas dissolved in a given volume of liquid is directly proportional to the partial pressure of the gas that is in equilibrium with the liquid.”

It is expressed as,

S α P

Where,

S = SolubilityP = Partial pressure

Introducing proportionality constant,

S = kHP

Where,

kH is Henry’s constant.

### Explanation of Solution

To determine: Solubility of Oxygen in water at 159 mmHg .

Let S1 be the solubility of Oxygen in water at partial pressure P1 and S2 be the solubility at partial pressure P2.   Then,

S1 = kHP1

S2 = kHP2

Solubility of a same gas at two different partial pressures can be calculated as,

S2S1 = kHP2kHP1 = P2P1                                            ......(1)

Given:  solubility of Oxygen in water S1 at pressure 1

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