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How are DeltaT(b) and DeltaT(f) related...

How are `DeltaT_(b)` and `DeltaT_(f)` related to the molar mass of the solute?

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To understand how the elevation in boiling point (ΔT_b) and depression in freezing point (ΔT_f) are related to the molar mass of the solute, we can break down the explanation into several steps: ### Step-by-Step Solution: 1. **Define ΔT_b and ΔT_f**: - ΔT_b is the elevation in boiling point, which is the increase in boiling point when a solute is added to a solvent. - ΔT_f is the depression in freezing point, which is the decrease in freezing point when a solute is added to a solvent. ...
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A system of greater disorder of molecules is more probable. The disorder of molecules is reflected by the entropy of the system. A liquid vapourizes to form a more disordered gas. When a solute is present, there is additional contribution to the entropy of the liquid due to increased randomness. As the entropy of solution is higher than that of pure liquid, there is weaker tendency to form the gas. Thus, a solute (non-volatile) lowers the vapour pressure of a liquid, and hence a higher boiling point of the solution. Similarly, the greater randomness of the solution opposes the tendercy to freeze. In consequence, a lower temperature must be reached for achieving the equilibrium between the solid (frozen solvent) and the solution. The elevation in boiling point (DeltaT_(b)) and depression in freezing point (DeltaT_(f)) of a solution are the colligative properties which depend only on the concentration of particles of the solute and not their identity. For dilute solutions, (DeltaT_(b)) and (DeltaT_(f)) are proportional to the molarity of the solute in the solution. A mixture of two immiscible liquids at a constant pressure of 1.0 atm boils at temperature

A system of greater disorder of molecules is more probable. The disorder of molecules is reflected by the entropy of the system. A liquid vapourizes to form a more disordered gas. When a solute is present, there is additional contribution to the entropy of the liquid due to increased randomness. As the entropy of solution is higher than that of pure liquid, there is weaker tendency to form the gas. Thus, a solute (non-volatile) lowers the vapour pressure of a liquid, and hence a higher boiling point of the solution. Similarly, the greater randomness of the solution opposes the tendercy to freeze. In consequence, a lower temperature must be reached for achieving the equilibrium between the solid (frozen solvent) and the solution. The elevation in boiling point (DeltaT_(b)) and depression in freezing point (DeltaT_(f)) of a solution are the colligative properties which depend only on the concentration of particles of the solute and not their identity. For dilute solutions, (DeltaT_(b)) and (DeltaT_(f)) are proportional to the molarity of the solute in the solution. To aqueous solution of Nal , increasing amounts of solid Hgl_(2) is added. The vapour pressure of the solution

A system of greater disorder of molecules is more probable. The disorder of molecules is reflected by the entropy of the system. A liquid vapourizes to form a more disordered gas. When a solute is present, there is additional contribution to the entropy of the liquid due to increased randomness. As the entropy of solution is higher than that of pure liquid, there is weaker tendency to form the gas. Thus, a solute (non-volatile) lowers the vapour pressure of a liquid, and hence a higher boiling point of the solution. Similarly, the greater randomness of the solution opposes the tendercy to freeze. In consequence, a lower temperature must be reached for achieving the equilibrium between the solid (frozen solvent) and the solution. The elevation in boiling point (DeltaT_(b)) and depression in freezing point (DeltaT_(f)) of a solution are the colligative properties which depend only on the concentration of particles of the solute and not their identity. For dilute solutions, (DeltaT_(b)) and (DeltaT_(f)) are proportional to the molarity of the solute in the solution. Dissolution of a non-volatile solute into a liquid leads to

How is density of gas related to its molar mass ?

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Molarity is related to molality (m) , density of the solution (d) and molar mass of the solute ( M^(@)) by which of following relation.

Derive the relation between elevation of boiling point and molar mass of the solute .

The expression relating mole fraction of solute (chi_(2)) and molarity (M) of the solution is: (where d is the density of the solution in g L^(-1) and Mw_(1) and Mw_(2) are the molar masses of solvent and solute, respectively

A dilute solution contains m mol of solute A in 1 kg of a solvent with molal elevation constant K_(b) . The solute dimerises in solution as 2A hArr A_(2) . Show that equilibrium constant for the dimer formation is K =(K_(b)(K_(b)m-DeltaT))/((2DeltaT_(b)-K_(b)m)^(2)) where DeltaT_(b) is the elevation of the boiling point for the given solution. Assume molarity = molarity

Derive a relation between density and molar mass of the gas.

ICSE-SOLUTIONS-EXERCISE (PART-II Descriptive Questions) (VERY SHORT ANSWER QUESTIONS)
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  15. What do you mean by saying that the molarity of a solution is one.

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  16. What is the relation between normality and molarity of a solution?

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  17. Write expressions for the Raoult's law for non-volatile solutes.

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  18. Define an ideal solution and write one of its characteristics.

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  19. State any two characteristics of ideal solutions.

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  20. What type of liquids form ideal solutions?

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