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Chapter 5: Problem 37

Which one of the following solution has least vapour pressure? (a) \(0.01 \mathrm{M} \mathrm{CaCl}_{2}\) (b) \(0.01 \mathrm{M}\) glucose (c) \(0.01 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4}\) (d) \(0.01 \mathrm{M} \mathrm{Na}_{3} \mathrm{PO}_{4}\)

Short Answer

Expert verified
The solution with Na鈧働O鈧� has the least vapor pressure due to the highest particle concentration.

Step by step solution

01

Understand Molality Influence

Vapor pressure lowering is a colligative property. It depends on the number of solute particles in the solution rather than the type of solute. This means we need to find which solution has the highest number of particles in solution.
02

Determine Ion Count for Each Compound

To determine the number of dissolved particles, we will calculate ions produced from 1 mole of each solute: - **CaCl鈧�**: Dissociates into 3 ions (1 Ca虏鈦� and 2 Cl鈦�) - **Glucose**: Does not dissociate in solution, so 1 particle - **Na鈧係O鈧�**: Dissociates into 3 ions (2 Na鈦� and 1 SO鈧劼测伝) - **Na鈧働O鈧�**: Dissociates into 4 ions (3 Na鈦� and 1 PO鈧劼斥伝)
03

Calculate Effective Particle Concentration

Each solution has a concentration of 0.01M. The concentration of particles will be: - **CaCl鈧�**: 0.01 M x 3 particles = 0.03 M particles - **Glucose**: 0.01 M x 1 particle = 0.01 M particles - **Na鈧係O鈧�**: 0.01 M x 3 particles = 0.03 M particles - **Na鈧働O鈧�**: 0.01 M x 4 particles = 0.04 M particles
04

Identify Least Vapor Pressure

Higher the concentration of particles, the lower the vapor pressure of the solution. Comparing concentrations: - Glucose has the fewest particles and thus the highest vapor pressure. - Na鈧働O鈧� has the highest concentration of particles at 0.04 M, hence provides the lowest vapor pressure.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Vapor Pressure
Vapor pressure is an essential concept in chemistry that describes the pressure exerted by the vapor in equilibrium with its liquid at a given temperature. In simpler terms, it is a measure of how easily molecules can escape from a liquid to form a gas above the liquid's surface.

When a solute is dissolved in a solvent, the vapor pressure of the solvent typically decreases, a phenomenon governed by colligative properties.
  • These properties depend solely on the number of solute particles, not their identity.
  • This means any solute, whether it is ionic or molecular, will affect vapor pressure based on how many particles it contributes to the solution.
  • As the particle count in a solution increases, the vapor pressure decreases because fewer solvent molecules are able to escape into the gas phase.
Understanding vapor pressure is crucial for predicting boiling and freezing points of solutions.
Solution Chemistry
Solution chemistry focuses on the study of solutes and solvents forming solutions, which can be gases, liquids, or solids. It is important to understand how solutes dissolve, interact with solvents, and affect properties like vapor pressure.

  • In a solution, a solute is the substance that is dissolved, while the solvent is the substance doing the dissolving.
  • Dissolving a solute in a solvent involves breaking the solute's bonds and forming new interactions between solute and solvent molecules.
  • In this context, colligative properties are vital, as they depend on the number of particles the solute releases into the solution rather than the solute's identity.
These properties include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. They can provide insights into molecular weights and ionization properties of substances.
Ionic Dissociation
Ionic dissociation occurs when ionic compounds dissolve in water, releasing ions into the solution. Understanding this process is fundamental to predicting many solution behaviors, including changes to vapor pressure.

  • When an ionic compound like NaCl dissolves, it separates into its constituent ions, \({ Na^+ }\) and \({ Cl^- }\).
  • This action increases the number of particles in the solution, significantly impacting colligative properties like vapor pressure.
  • The degree of dissociation depends on the solute, affecting how many ions are produced per formula unit.

In the original exercise, among the options, \({ CaCl_2 }\), \({ Na_2SO_4 }\), and \({ Na_3PO_4 }\) all dissociate into multiple ions, whereas glucose does not, illustrating the direct impact of ionic dissociation on the overall particle count in solution.

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Most popular questions from this chapter

The osmotic pressure of a solution containing \(4.0\) \(\mathrm{g}\) of solute (molar mass 246 ) per litre at \(27^{\circ} \mathrm{C}\) is \(\left(\mathrm{R}=0.082 \mathrm{~L} \mathrm{~atm} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)\) (a) \(0.1 \mathrm{~atm}\) (b) \(0.3 \mathrm{~atm}\) (c) \(0.4 \mathrm{~atm}\) (d) \(0.9 \mathrm{~atm}\)

Mercuric iodide is added to an aqueous solution of potassium iodide. Identify the correct statement(s) (a) Freezing point is raised. (b) Freezing point is lowered. (c) Freezing point and boiling point does not change. (d) Boiling point is raised. (a) 1 and 4 (b) 3 and 4 (c) Only 1 (d) 2 and 4

The freezing point of equimolal aqueous solution will be highest for (a) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{~N}^{+} \mathrm{H}_{3} \mathrm{Cl}^{-}\)(aniline hydrochloride) (b) \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) (c) \(\mathrm{La}\left(\mathrm{NO}_{3}\right)_{3}\) (d) \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) (glucose)

An aqueous solution of \(6.3 \mathrm{~g}\) oxalic acid dihydrate is made up to \(250 \mathrm{~mL}\). The volume of \(0.1 \mathrm{~N} \mathrm{NaOH}\) required to completely neutralize \(10 \mathrm{~mL}\) of this solution is (a) \(40 \mathrm{~mL}\) (b) \(20 \mathrm{~mL}\) (c) \(10 \mathrm{~mL}\) (d) \(4 \mathrm{~mL}\)

The vant Hoff factor 'i' accounts for (a) the extent of dissociation of solute (b) the extent of dissolution of solute (c) the degree of decomposition of solution (d) degree of solubilization of solute
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