At a particular temperature, the solubility of O₂ in water is
0.0500 M when the partial pressure is 0.120 atm. What will the
solubility (in M) be when the partial pressure of O₂ is 0.320
atm?
A solution made by dissolving 150.0 g of an unknown compound in
370.0 mL of benzene to make a solution which has a freezing point
18.6 °C lower than that of pure benzene. Kf for benzene is 5.12
°C/m and the density of benzene is 0.877 g/mL.
a What was the molality of the solution?
b What quantity in moles of the unknown compound were dissolved
in the solution?
c What is the molar mass of the unknown compound?
At a particular temperature, the solubility of O₂ in water is 0.0500 M when the partial pressure is 0.120 atm. What will
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At a particular temperature, the solubility of O₂ in water is 0.0500 M when the partial pressure is 0.120 atm. What will
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