Question

. The i value assumes that an ionic compound dissociates 100% in solution. Is this true? Explain this by considering the percent difference in ΔT values and the behavior of ions in solution (you might want to read up on ion behavior). This is looking at three different compounds Nacl with delta T of .9 degree celcius and Na2SO4 with a delta t value of 1.1 and Na3 PO4 of a delta t of 1.5. Each of these compounds in increasing order have vant hoff factors of 2, 3 and 4.

Answer #1

**Answer** – We know as the compound is 100 %
dissociated, means ionic compound then its vant hoff factors i
value is consider, so **it is true**. When the ionic
compound dissociates 100% in solution then there is more free
particle in the solution and there is more disorder or solution and
form the more ∆T and hence it is more percent difference in ΔT
values. Example for the NaCl there are 2 ion like Na^{+}
and Cl^{-} so the vant hoff factors i value is 2, for
Na_{2}SO_{4} there are 3 ions and for
Na_{3}PO_{4} there are 4 ions, so as the vant hoff
factors i value increased the percent difference in ΔT values also
increase, since the ΔT value is directly proportional to the vant
hoff factors i.

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