Do you feel comfortable in making the assumption that the NaCl in your experiment was completely dissociated? Why or why not?

1. Do all saturated solutions have the same

density?  Based on your data, which salt is more soluble?

Saturated solution do not have the same density.

11.812g /10 mL = 1.181  g/mL NaCl

9.783g / 10 mL = 0.978 g/mL CaSO4

2. Of 100% of the NaCL molecules dissociated, the Van’t Hoff factor i, would be equal to 2 for NaCl. We assumed it equaled two when we figured out Kb of the NaCl solution.

a. Now we want it find the percent dissociation of the NaCl molecules by finding i using the equation below (use Kb = 0.512℃/m and 3.456m molarity of  NaCl  )          show all work

i = ( ▵Tb) / Kb x m)

i experimental = 1.8 [ {1.8/2} * 100% = 90% dissociation]    i theoretical = 2 (100% dissociation)

b. Do you feel comfortable in making the assumption that the NaCl in your experiment was completely dissociated? Why or why not?

c. How does making this assumption (as we did) affect the boiling point elevation of Kb?