Slide 1Slide 2Slide 3Slide 4Slide 5Slide 6Slide 7Determine the solubility of oxygen in water at 25 °C exposed to air at 1.0 atm. Assume a partial pressure for oxygen of 0.21 atm.A pressure of 3.5 atm in CO2 is required to maintain a 0.12 M CO2 concentration in soda. Calculate the Henry’s Law constant for CO2.Calculate the vapor pressure at 25 °C of a solution containing 55.3 g ethylene glycol (HOCH2CH2CH2OH) and 285.2 g water. The vapor pressure of pure water at 25 °C is 23.8 torr.Calculate the freezing point and melting point of a solution containing 10g of naphthalene (C10H8) in 100 ml benzene (d=0.877g/cm3)A solution of 5.00 g of an unknown substance in 0.100 kg of benzene freezes at 4.1°C. What is the molar mass of the unknown substance? Kf (benzene) = 5.12°C/m; ΔTf (benzene) = 5.50°C.Calculate the osmotic pressure of the solution containing 1.5g of ethylene glycol (C2H6O2) in 50ml of solution at 25◦CA solution containing 27.55 mg of an unknown protein per 25ml solution has an osmotic pressure of 3.22 torr at 25◦C. What is the molar mass of the
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