Calculate the molarity and mole fraction of acetone in a 1.70-m solution of acetone (CH3 COCH,) in ethanol ( C,H;OH). (Density of acetone -0.788 g/cm"; density of ethanol -0.789 g/cm".) Assume that the volumes of acetone and ethanol add. Molarity | M Mole fraction

What is the concentration of O2 in freshwater? Air temperature= 295.65 K.  Air pressure = 1 bar(about = to 1atm).  Henry's constant, from the table= 1.3 x 10-3 mol/ (kg x bar). PO2 can be calculated from the fact that oxygen is .21 mole fraction of air.  Hint- The partial pressure of a gas in a mix of gasses is found by multiplying the total pressure by the mole fraction of that gas. Find the concentration in g/kg from the answer you just got.

A 2.66 m (molal) solution of propanal (C3H7OH) prepared by dissolving a known amount of the subatance in 200,0a of octane (C Hig),what was the mass af propanol added? what is the mole fraction of octane? - was

Calculate the solubility of MNCO3 (in mol/L) in the following. Assume the Кр of MnCOз 1.8 х 10-11. (a) water mol/L (b) 0.0467 M Mn(NO3)2 mol/L (c) 0.0467 М К.СОз mol/L

Henry's law constant for transferring 02 from air into water, at room temperature, mmol liter – atm • - is 1.3 Given that the partial pressure of O2 in the atmosphere is 0.21 atm, the concentration of dissolved oxygen (mg/liter) in water in equilibrium with the atmosphere at room temperature is (Consider the molecular weight of O2 as 32 g/mol)

Henry's law constant for carbon dioxide dissolving in water is 3.5*10^-2 mol/L*atm at 20 degrees celsius. What is the maximum molar concentration of carbon dioxide in a pond at this temperature ? The mole fraction of CO2 in air is 3.14*10^-4