Name all the intermolecular forces involved in the following situations and use the concepts of intermolecular forces to explain what is happening:     Both sodium carbonate and methyl ethyl ketone are soluble in water, but only methyl ethyl ketone is soluble in benzene.

Which of the following compounds can form hydrogen bond with water: ethanol, 1-decanol, glycerin, sucrose and urea? State a reason why each compound will or will not form hydrogen bond with water. What effect will hydrogen bonding have on the solubility of each compound in water? In hexane?

Henry's Law constant is 0.000600 mol/kg-bar and 0.00130 mol/kg.bar for N2 and O2 respectively at 25°C. What pressure of O2 is required to achieve the same solubility as 0.616 bar of N2 in units of atm? (1 bar = 0.9869 atm; 1 atm = 760 mmHg) O 1.3 atm 0.276 atm O 4.8 x 10-7 atm O 1.3 x 106 atm O 3.5 atm

1.) Are there any intermolecular forces (IMF’s) between water molecules and cyclohexane molecules? What kind(s)? Given this, what would the magnitude and sign of DHMIXING be for cyclohexane dissolving in water?   a) Are there any IMF’s between water molecules and other water molecules? What kind(s)? Given this, what would the magnitude and sign of DHSOLVENT be for cyclohexane dissolving in water?   c) Are there any IMF’s between cyclohexane molecules and other cyclohexane molecules? What kind(s)? Given this, what would the magnitude and sign of DHSOLUTE  be for cyclohexane dissolving in water?   d) Why do you think cyclohexane does not dissolve in water? Analyze this the way it was done in class, thinking about the three contributions to DHSOLUTION. What do you think the magnitude and sign of DHSOLUTION would be for dissolving cyclohexane in water?  (Explain.)  Would you expect these substances to dissolve in each other? Why?