Final answer:
The aqueous solution with the highest boiling point is 0.5M Na3PO4, as it has the largest van 't Hoff factor among the given choices, leading to the highest boiling point elevation.
option d is the correct
Step-by-step explanation:
The question asks which of the following aqueous solutions would have the highest boiling point: 0.5M NaCl, 0.5M NaNO3, 0.5M Na2SO4, 0.5M Na3PO4, and 0.5M Na2CO3.
To determine the highest boiling point among the given solutions, we will apply the concept of boiling point elevation, which states that the boiling point of a solvent increases when a solute is dissolved in it. This effect is quantified using the van 't Hoff factor (i), which is the number of particles into which a compound dissociates in solution. The larger the van 't Hoff factor, the greater the boiling point elevation.
In the given solutions, NaCl dissociates into 2 ions, NaNO3 also dissociates into 2 ions, Na2SO4 dissociates into 3 ions, Na3PO4 dissociates into 4 ions, and Na2CO3 dissociates into 3 ions. Since all solutions are 0.5M, the number of particles produced is directly related to the van 't Hoff factor of the solute.
Considering this, the order of the boiling points from the lowest to highest is as follows:
0.5M NaCl < 0.5M NaNO3 < 0.5M Na2CO3 ≈ 0.5M Na2SO4 < 0.5M Na3PO4
Therefore, the aqueous solution with the highest boiling point among the choices given would be 0.5M Na3PO4, as it produces the most number of particles when dissolved, leading to the highest boiling point elevation.