To calculate *solubility* of a dissolves gas, **Henry's Law Constant** and *partial pressure* are used.

## Henry's Law Calculations Concept 1

## Henry's Law Calculations Example 1

## Henry's Law Calculations Concept 2

**The 2 Point Form of Henry's Law Formula** is used when dealing with 2 pressures and 2 solubilities of a given gas.

## Henry's Law Calculations Example 2

Henry’s Law Constant for nitrogen in water is 1.67 × 10^{-4} M • atm^{–1}. If a closed canister contains 0.103 M nitrogen, what would be its pressure in atm?

^{–5}atm

^{–3}atm

At 0°C and 1.00 atm, as much as 0.84 g of O_{2} can dissolve in 1.0 L of water. At 0°C and 4.00 atm, how many grams of O_{2} dissolve in 1.0 L of water?

The atmospheric pressure in a lab is calculated as 1.3 atm. If oxygen gas contributes 62% of this atmospheric pressure, determine its mass (in g) dissolved at room temperature in 25 L of water. The Henry’s Law Constant for oxygen in water at this temperature is 5.3 × 10^{–5} M/atm.

^{–3}g

^{–5}g

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