   # Hydrogen gas has a Henry’s law constant of 7.8 × 10 −4 mol/kg·bar at 25 °C when dissolving in water. If the total pressure of gas (H 2 gas plus water vapor) over water is 1.00 bar, what is the concentration of H 2 in the water in grams per milliliter? (See Appendix G for the vapor pressure of water.) ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 13, Problem 22PS
Textbook Problem
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## Hydrogen gas has a Henry’s law constant of 7.8 × 10−4 mol/kg·bar at 25 °C when dissolving in water. If the total pressure of gas (H2 gas plus water vapor) over water is 1.00 bar, what is the concentration of H2 in the water in grams per milliliter? (See Appendix G for the vapor pressure of water.)

Interpretation Introduction

Interpretation The concentration of hydrogen gas has to be identified.

Concept introduction:

Solubility of a gas: It is defined as the concentration of the dissolved gas in equilibrium with the substance in the gaseous state.

Henry’s law: The solubility of a gas in liquid is directly proportional to the gas pressure.

Sg= kHPg,where,Sgisthegassolubility(inmol/kg)kHis Henry's constant Pg is the partial pressure of the gaseous solute.

### Explanation of Solution

Given data:

kH(H2 gas) = 7.8×10-4 mol/kg.barPtotal=1bar;Pwatervapor=23.8torr=0.0317bar

Ptotal=PH2+PwatervaporPH2=Ptotal-Pwatervapor=1bar-0.0317bar=0.968barConcentration of  H2 gas (Sg)=  ?

Sg= kHPg,=(7

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