Physical Pharmaceutics I (MCQ-2) (Practical)

When a substance dissolves, the solute particles separate and disperse throughout the solvent. In order for this to happen, the attractions between the solute and solvent particles must be stronger than the attractions within the solute and solvent themselves. This means that the solute-solvent attractions must overcome the attractions within both the solute and solvent. Therefore, the given statement accurately describes the dissolving process.

When a substance dissolves, the solute particles separate and disperse throughout the solvent. This process occurs when the attractions between the solute and solvent molecules are stronger than the attractions within the solute and solvent themselves. Therefore, for a substance to dissolve, the solute-solvent attractions must overcome the attractions within both the solute and solvent. This explanation aligns with the given statement.

When osmotic pressure and temperature are the same, it means that the conditions for osmosis are identical for both solutions. Osmotic pressure is directly proportional to the number of moles of solute particles in a solution. Therefore, if the osmotic pressure and temperature are the same, it implies that the two solutions have an equal number of moles of solute particles. As a result, equal volumes of these solutions would contain an equal number of moles of the solute.

Acetanilide is not a volatile substance because it has a high boiling point and does not easily evaporate at room temperature. Volatile substances, such as camphor, petrol, and acetone, have low boiling points and readily evaporate into the air.

Ionic compounds and polar covalent compounds will dissolve in polar solvents because these compounds have either ionic or polar covalent bonds, which allow them to interact with the polar solvent molecules through electrostatic attractions or dipole-dipole interactions. Polar solvents have a partial positive and partial negative charge, which can interact with the positive and negative ions or polar molecules in the compounds, causing them to dissolve. Non-polar solvents and covalent compounds, on the other hand, do not have the necessary polarity to interact with polar solvents and therefore do not dissolve in them.

The freezing point is not a colligative property because it is not dependent on the number of solute particles present in a solution. Colligative properties, such as osmotic pressure, elevation of boiling point, and depression in freezing point, are only affected by the concentration of solute particles and not the identity of the solute itself.

Hydration is the term that describes the process in which ions are surrounded by water molecules. When ions dissolve in water, the water molecules surround the ions, forming a hydrated ion. This process is important in many chemical reactions and biological processes, as it helps to stabilize and solvate the ions, allowing them to interact with other molecules.

A saturated solution refers to a solution that contains the maximum quantity of solute at a given temperature. In a saturated solution, the solute is completely dissolved and in equilibrium with any undissolved solute. This means that if more solute is added, it will not dissolve and will instead settle at the bottom of the container.

A carbonated drink is an example of a supersaturated solution because it contains more dissolved carbon dioxide than would normally be possible at that temperature and pressure. The drink is able to hold the excess carbon dioxide due to the high pressure in the bottle or can. When the container is opened, the sudden release of pressure causes the excess carbon dioxide to come out of solution, resulting in the characteristic fizzing or effervescence of the drink.

An ideal solution is one that obeys Raoult's law, meaning that the vapor pressure of each component in the solution is directly proportional to its mole fraction. Additionally, an ideal solution should not undergo any chemical reactions between the solute and solvent. However, the volume change on mixing is not equal to zero in an ideal solution. This means that when the solute and solvent are mixed together, there is a change in the volume of the solution.