(a) Does a 0.10 m aqueous solution of NaCl have a higher boiling point, a lower boiling point, or the same boiling point as a 0.10 m aqueous solution of C6H12O6?

Video transcript

Hey everyone, we're asked how will a 0.125 morality of calcium chloride solution compared to a 0.125 Morality sodium chloride solution in terms of our boiling point. Will its boiling point be higher? Lower or the same as the sodium chloride solution? To answer this question, we have to look at our boiling point elevation formula, which is going to be I which is our Van Hoff constant times R K B, which is our boiling point elevation constant times. Our morality Looking at our two solutions, we can see that we have a 0.125 morality for both and since KB only depends on the solvent, it should also be the same for both solutions. So we have to look at our eye which is our Van Hoff constant. Starting with our calcium chloride, this will dissociate into calcium ions plus our chlorine ions. Since we produce three ions in our solution, our Van Hoff constant is going to be three. Next looking at sodium chloride, we got sodium ions plus our chlorine ions. As we can see right here, our Van Hoff constant comes up to two since we produced two ions in solution. Since our calcium chloride has a higher value of I this means it will have a higher boiling point than our sodium chloride solution. So our answer here is going to be higher. Now I hope that made sense. And let us know if you have any questions