1.  The log P for chloroform (CHCl₃) was found to be 1.97 for a mixture of 200 mL of water and 300 mL of 1-octanol.

• Calculate the value of the partition coefficient P.
• Based upon the value of P, discuss the underlying reasons ( in terms of intermolecular forces) for  the solubility behavior of chloroform in 1-octanol vs. water.
• If the water phase had a chloroform concentration of 0.125 mM, calculate the expected  concentration of chloroform in the 1-octanol phase.
• Describe how the two chloroform concentrations would change (increase, decrease, or no change) if 100 mL of water were added to the mixture.
• For the addition of this 100 mL of water to the mixture, predict whether and how the total mass of chloroform present in the octanol phase would change.
• Draw a diagram of a container holding this mixture and clearly label the concentration of each of the phases.
• Use thermodynamics to explain and to predict how the concentration of chloroform in water would change with an increase in temperature (assume constant volumes of liquids).

• Temperature
• Increase in the chain length of phospholipid fatty acid components
• Increase in the degree of unsaturation of phospholipid fatty acid chains
• Increase in the amount of cholesterol found in the membrane