Liquid Solution

Given information:Mass of solute (naphthoic acid) = 2 gMolecular weight of naphthoic acid = 172 g/molCalculate the moles of naphthoic acid: Now, converting volume of solvent (benzene) to mass in kg:Volume of benzene = 20 mLDensity of benzene = 0.88 g/mLCalculate the mass of benzene: Determine the molality (m): Given constants:Freezing point depression, Freezing point depression constant, Using the formula for freezing point depression: Solve for the van't Hoff factor, :

Solution X (Hexane and Benzene):Nature of Interaction:Both hexane and benzene are non-polar substances. Their intermolecular forces are primarily London dispersion forces (a type of van der Waals force).Deviation Type:Ideal BehaviorSince the intermolecular forces between hexane and benzene are similar, the solution typically adheres closely to Raoult's Law. Thus, it either behaves ideally or exhibits very minor deviations, which are often negligible.Solution Y (Water and HCl):Nature of Interaction:Water is a polar compound with strong hydrogen bonds. When HCl is dissolved in water, it dissociates into and ions, leading to strong ion-dipole interactions between these ions and water molecules.Deviation Type:Negative DeviationThe ion-dipole interactions between water and HCl are significantly stronger than the hydrogen bonding in pure water or the weaker dipole-dipole interactions in pure HCl. Consequently, the vapor pressure of the solution is lower than predicted by Raoult's Law, resulting in a negative deviation.

The osmotic pressure ( ) of a solution is described by the formula: Where: is the osmotic pressure, is the number of moles of the solute, is the universal gas constant, is the temperature in Kelvin, is the volume of the solution.In this scenario, the amount of solute ( ) and the temperature ( ) remain constant. Therefore, the relationship between osmotic pressure and volume simplifies to: This implies that as the volume ( ) approaches zero, the osmotic pressure ( ) tends towards infinity.