Solution Density(g/L) Boiling Point Freezing Point
1.0m C2H5OH(aq) 1.05 100.5 -1.8
1.0m HCI(aq) 1.03 101.0 -3.7
1.0m NaCl(aq) 1.06 101.0 -3.7
2.0m NaCl(aq) 1.12 102.1 -7.4
1. Which properties in the table are colligative properties?
2. What can you conclude about the relationship between colligative properties and the type of ions in solution from the 1.0m HCl(aq) and 1.0m NaCl(aq) solutions?
1. Colligative properties are those that depend on the number of solute particles present in a solution, regardless of their identity. In the given table, boiling point elevation and freezing point depression are colligative properties because they are affected by the concentration of solute particles.
2. From the comparison between the 1.0m HCl(aq) and 1.0m NaCl(aq) solutions, we can conclude that the type of ions in solution does affect the colligative properties. Both solutions have the same concentration (1.0m), but the boiling point and freezing point of the HCl solution are slightly higher than those of the NaCl solution. This can be attributed to the fact that HCl dissociates into one hydrogen ion (H+) and one chloride ion (Cl-) in solution, while NaCl dissociates into one sodium ion (Na+) and one chloride ion (Cl-). Since the HCl solution has more ions per mole of solute particles compared to the NaCl solution, it exhibits a greater effect on the colligative properties.