Here's how to calculate the solubility of N₂ in water at 25°C and 1.0 atm using the given Henry's Law constant (K_H):

Understanding Henry's Law

Henry's Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid. Mathematically:

* C = K_H * P

Where:

* C is the concentration of the dissolved gas (mol/L)

* K_H is Henry's Law constant (mol/L·atm)

* P is the partial pressure of the gas (atm)

Calculation

1. Identify the given values:

* K_H = 6.4 x 10⁻⁴ mol/L·atm

* P = 1.0 atm (partial pressure of N₂)

2. Apply Henry's Law equation:

* C = (6.4 x 10⁻⁴ mol/L·atm) * (1.0 atm)

3. Solve for C:

* C = 6.4 x 10⁻⁴ mol/L

Therefore, the solubility of N₂ in water at 25°C and 1.0 atm is 6.4 x 10⁻⁴ mol/L.