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Under an O2(g) pressure of 1.00 atm , 28.31mL of O2 (g) dissolves in 1.00L H2O at 298K.

What will be the molarity of O2 in the saturated solution at 298K when the pressure is 3.86atm ? (Assume that the solution volume remains at 1.00L .)

I used PV=nRT and found moles of solute was = 4.47*10^-3 moles which is in 1L of solution so is that the molarity? For some reason it doesn't seem right to me.

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