Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 14: Problem 94

What is "dynamic" about the equilibrium that is established when a sparingly soluble salt is added to water?

Short Answer

Expert verified
The dynamic aspect of the equilibrium established when a sparingly soluble salt is added to water refers to the simultaneous, ongoing processes of dissolution and precipitation. Although the macroscopic properties, such as solubility and concentration, remain constant, the ions in the solution are continuously exchanging with the solid and liquid phases at a microscopic level. These continuous and opposing processes of dissolution and precipitation occur at equal rates, maintaining a constant concentration of dissolved salt in the solution while the system remains in a constant state of motion and exchange, defining the equilibrium as dynamic.

Step by step solution

01

1. Understanding the concept of dynamic equilibrium

Dynamic equilibrium is a state in which the rates of two opposing processes (dissolution and precipitation, in this case) are equal. During dynamic equilibrium, there is no change in the concentration of dissolved components or the amount of solid substance. However, this doesn't mean that the substance stops dissolving or precipitating. Both processes are continuously happening at equal rates, maintaining the overall balance.
02

2. Dissolution and precipitation in sparingly soluble salts

When a sparingly soluble salt is added to water, it dissolves to some extent, forming a solution of ions in equilibrium with the undissolved solid. As the salt dissolves, the concentration of ions in the solution increases. At the same time, precipitation reactions are occurring as ions from the solution collide and form back into solid molecules. This continues until the rates of dissolution and precipitation become equal, and the system reaches equilibrium.
03

3. The dynamic nature of equilibrium in sparingly soluble salts

In the case of sparingly soluble salts, the equilibrium established with water is dynamic because both dissolution and precipitation processes continue to occur simultaneously even at equilibrium. The ions in the solution are constantly colliding with the solid salt, and some of them precipitate back to form the solid again. Conversely, some of the solid salt particles dissolve in the water to maintain the ion concentrations in the solution. Thus, the system is constantly changing at a microscopic level, while the macroscopic properties, like solubility and concentration, remain constant. This continuous exchange of ions between the solid and liquid phases is what makes the equilibrium dynamic.
04

4. Conclusion

The dynamic nature of the equilibrium established when a sparingly soluble salt is added to water refers to the ongoing processes of dissolution and precipitation occurring simultaneously. The rates of both processes are equal, maintaining a constant concentration of dissolved salt in the solution while continuing to dissolve and precipitate individual ions at the microscopic level. The equilibrium is dynamic due to the continuous motion and exchange of ions in the system, sustaining the overall balance between the solid and liquid phases.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

A certain reaction has a \(K_{\text {eq }}\) value of \(1.5 \times 10^{-6}\). (a) Would this be a practical reaction from which to isolate pure product? Explain your answer.

(a) Rewrite this reaction with the word heat in it: $$ 2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \rightleftarrows 2 \mathrm{CO}_{2}(g) \quad \Delta E=-563.5 \mathrm{~kJ} $$ (b) Which way does the reaction shift when the temperature is raised? Explain your answer.

Phosphorus pentachloride gas decomposes to \(\mathrm{PCl}_{3}(\mathrm{~g})\) and \(\mathrm{Cl}_{2}(\mathrm{~g}) .\) At equilibrium, the concentrations of the decomposition products are \(5.50 \times 10^{-3} \mathrm{M}\) for \(\mathrm{PCl}_{3}(\mathrm{~g})\) and \(0.125 \mathrm{M}\) for \(\mathrm{Cl}_{2}(g)\). What is the equilibrium concentration of \(\mathrm{PCl}_{5}\) ? The equilibrium constant for this reaction is \(7.50 \times 10^{-2}\).

Write the expression for \(K_{\mathrm{eq}}\) for the reaction \(\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftarrows 2 \mathrm{NO}_{2}(g)\).

The saturation solubility of \(\mathrm{Ag}_{2} \mathrm{~S}\) at \(25^{\circ} \mathrm{C}\) is \(1.14 \times 10^{-17} \mathrm{M}\). What are the equilibrium concentrations of the cation and anion?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Physical Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Organic Chemistry

Read Explanation

Making Measurements

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free