What pressure would be required to form a 0.050 M solution of helium (kH = 3.7 x 10-4 M/atm) at 25 °C?
oops twice. What I wrote above is wrong.
What I wrote is correct for K in different units.
What you want is k = C/p. Again, plug in C and solve for p.
I tried deleting the first two posts but my deleter is not working.
DrBob, I deleted them.
To find the pressure required to form a 0.050 M solution of helium at 25 °C, we can use Henry's Law. Henry's Law states that the concentration of a gas in a solution is directly proportional to the partial pressure of the gas above the solution.
The equation for Henry's Law is:
P = kH * C
Where:
P is the pressure of the gas above the solution,
kH is the Henry's Law constant for the gas,
C is the concentration of the gas in the solution.
In this case, the concentration of helium in the solution is given as 0.050 M, and the Henry's Law constant for helium (kH) is given as 3.7 x 10-4 M/atm.
Substituting the given values into the equation:
P = (3.7 x 10-4 M/atm) * (0.050 M)
P = 1.85 x 10-5 atm
Therefore, the pressure required to form a 0.050 M solution of helium at 25 °C is approximately 1.85 x 10-5 atm.