Question

List the following aqueous solutions in order of increasing melting point. (The lastthree are all assumed to dissociate completely into ions in water.)(a) 0.1 m sugar(b) 0.1 m NaCl(c) 0.08 m CaCl2(d) 0.04 m Na2SO4

Answer 1

0.1M sugar < 0.1 M NaCl < 0.08M CaCl2 < 0.04 M Na2SO4​

Explanations:

First we must understand that the higher thecnoncentration of a compound, the lower the melting point. This shows that 0.04 m Na2SO4​ will have highest melting point followed by 0.08 M CaCl2

Since 0.1M of sBgar and 0.1M of NaCl have the same molarity, we will determine the effect of solute and ionic bonding between compound on melting point. Since common salt (NaCl) is made up of stronger ionic bonds, it will have higher melting point than sugar.

The increasing order of their melting point wile be 0.1M sugar < 0.1 M NaCl < 0.08M CaCl2 < 0.04 M Na2SO4​