The solubility of NH3 in H20 is 518 g/L at a partial pressure of 760.0 torr.
1. Calculate the value of the Henry's Law constant for NH3.
2. calculate the solubility of NH3 in H2O at a partial pressure of 225.0 torr.
The subject is not Pensacola State
I worked this for JD. Assuming you are not JD, here is what I wrote (more or less).
There are all kinds of unts used for Henry's Law constant and different equations for Henry's Law. The one I use is p = kc where p is in atm and c is in moles/L. That gives k = p/c = atm*L/moles for k. Convert 518 g NH3 to moles. moles = grams/molar mass and that is in 1 L; therefore, that is the molarity. 518/17 = 30.47 and k = 1/30.47. For the remaining part of the problem, p = kc = (225/760) = c/30.47 and solve for c.
p = kc and (225/760)
To calculate the Henry's Law constant for NH3, we can use the equation:
C = k * P
Where:
C is the concentration of NH3 in solution (in this case, solubility)
k is the Henry's Law constant
P is the partial pressure of NH3
1. Calculate the Henry's Law constant:
You have been given the solubility of NH3 in H2O, which is 518 g/L, and the partial pressure, which is 760.0 torr.
To convert the solubility from g/L to mol/L, we need to divide it by the molar mass of NH3 (17.03 g/mol):
Solubility (in mol/L) = 518 g/L / 17.03 g/mol
Next, substitute the values into the equation:
518 g/L / 17.03 g/mol = k * 760.0 torr
Simplify by canceling units and solving for k:
Solubility (in mol/L) / (760.0 torr) = k
Calculate the value of k to find the Henry's Law constant for NH3.
2. Calculate the solubility of NH3 in H2O at a partial pressure of 225.0 torr:
To calculate the solubility, we can rearrange the equation and solve for C:
C = k * P
Given that the partial pressure is 225.0 torr, substitute the values into the equation:
C = k * 225.0 torr
Use the calculated Henry's Law constant (k) from step 1 to find the solubility (C) at a partial pressure of 225.0 torr.