A saturated solution was formed when 4.48×10−2 L of argon, at a pressure of 1.0 atm and temperature of 25 C, was dissolved in 1.0 L of water. Calculate the Henry's law constant for argon in mol/atm.

I got an answer of 1.4*10^-3, maybe my units are wrong, idk but if u could show your work that would be awesome

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  1. Start with the Ideal Gas Law
    PV = nRT
    n = PV / RT
    K = n/P (from Henry's Law)
    n/P = V/RT (from the Ideal Gas Law)
    K = V/RT (by combining the last two equations)
    (V = liters, R = 0.0821 L.atm/K.mol, T = 298K)
    Substitute to get the constant, K

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  2. 2.2x10^-2

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