Final answer:
The truth of the statement regarding the solubility of the generic salt AB2 cannot be confirmed without additional information, such as the specific salt or its solubility product constant. Understanding solubility often involves the van 't Hoff factor, which influences colligative properties and needs to be considered in solubility and boiling point elevation calculations.
Step-by-step explanation:
To determine if the statement 'At 25, only 0.0570 mol of the generic salt AB2 is soluble in 1 L of water' is true or false, one needs more information such as the specific identity of the salt or its solubility product constant (Ksp). Solubility can vary widely among different salts, and the given value could be reasonable for one salt but not another. To understand solubility, it is helpful to look at the van 't Hoff factor, which provides insight into the effect of solute particles on colligative properties. For instance, the osmotic pressure of a 0.050 M LiCl solution at 25.0°C yields a true van 't Hoff factor that is less than the ideal due to ion pairing or other interactions. Similarly, the freezing point depression of a 0.500 m MgCl2 solution leads to a true van 't Hoff factor that is less than the maximum value of 3 expected for complete dissociation into ions, again likely due to ion interactions.
Specific examples like these illustrate how the van 't Hoff factor is crucial in understanding colligative effects such as boiling point elevation and freezing point depression, and plays a key role in calculations involving solubility and solubility equilibria. Without adequate context for the solubility of AB2, the truth of the statement cannot be determined. The comparison of solubilities based on Ksp values or stoichiometry would be more meaningful.
Determining the elements represented by X, Y, and Z based on boiling point elevation and a van 't Hoff factor involves applying the concept of molality and the colligative property constants for boiling point elevation. The solubility of salts like I2 can also be calculated using molarity, as solubility typically depends on the temperature and the nature of the solute and solvent.