Determine the partial pressure of oxygen necessary to form an aqueous solution that is 7.7 x 10-4 M O2 at 25oC. The Henry's Law Constant for oxygen in water at 25oC is 1.3 x 10-3 M/atm
To determine the partial pressure of oxygen necessary to form the given aqueous solution, we can use Henry's Law equation:
C = k * P
Where,
C = concentration of the gas in the solution (M)
k = Henry's Law Constant (M/atm)
P = partial pressure of the gas (atm)
Given:
C = 7.7 x 10^-4 M
k = 1.3 x 10^-3 M/atm
We need to solve for P.
Rearranging the equation, we get:
P = C / k
Substituting the given values:
P = (7.7 x 10^-4 M) / (1.3 x 10^-3 M/atm)
P = 5.92 x 10^-1 atm
Therefore, the partial pressure of oxygen necessary to form the aqueous solution is 5.92 x 10^-1 atm.
To determine the partial pressure of oxygen necessary to form an aqueous solution with a given concentration, we can use Henry's Law. Henry's Law states that the concentration of a gas in a solution is directly proportional to its partial pressure.
The equation for Henry's Law is:
C = k * P
where:
C is the concentration of the gas in the solution (in this case, 7.7 x 10^-4 M O2),
k is the Henry's Law Constant (1.3 x 10^-3 M/atm),
P is the partial pressure of the gas.
To find the partial pressure, we rearrange the equation as:
P = C / k
Plugging in the given values:
P = (7.7 x 10^-4 M O2) / (1.3 x 10^-3 M/atm)
Now, let's calculate:
P ≈ 0.592 atm
Therefore, the partial pressure of oxygen necessary to form an aqueous solution with a concentration of 7.7 x 10^-4 M O2 at 25°C is approximately 0.592 atm.
C = pO2*K
Substitute for C and K from the problem and solve for pO2.