Final answer:
To determine the solubility of nitrogen in water at 25°C exposed to air at 1.0 atm, you can use Henry's Law. The solubility can be calculated using the equation C = kH × P, where C is the concentration of the gas in the liquid, kH is the Henry's Law constant, and P is the partial pressure of the gas above the liquid. Plugging in the given values, we find that the solubility of nitrogen in water at 25°C is approximately 4.758x10^-4 M.
Step-by-step explanation:
Henry's law relates the solubility of a gas in a liquid to the partial pressure of the gas above the liquid. The equation for Henry's Law is given as:
C = kH × P
where C is the concentration of the gas in the liquid, kH is the Henry's Law constant, and P is the partial pressure of the gas above the liquid.
In this case, you are given the partial pressure of nitrogen (N2) as 0.78 atm and the Henry's Law constant (kH,N2) as 6.1x10^-4 M/atm. To determine the solubility of nitrogen in water at 25°C, we can use the equation: C = kH × P
Plugging in the values, we get: C = (6.1x10^-4 M/atm) × (0.78 atm) = 4.758x10^-4 M
So, the solubility of nitrogen in water at 25°C exposed to air at 1.0 atm is approximately 4.758x10^-4 M.