1 / 10

Understanding Equilibrium in Homogeneous and Heterogeneous Phase Chemical Reactions

This article explains the concept of equilibrium in homogeneous and heterogeneous phase chemical reactions. It explores the factors affecting equilibrium, such as solubility product constant and solubility ratios. Numerical examples are provided to illustrate the concepts discussed.

kboles
Download Presentation

Understanding Equilibrium in Homogeneous and Heterogeneous Phase Chemical Reactions

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Homogeneous phase chemical reaction Always can reach equilibrium Never the reaction is 100% complete

  2. Heterogeneous phase chemical reaction Different K for different nB ?? Need more B to reach equilibrium

  3. dissolution: precipitation: pure solid, activity =1 Solubility product constant:

  4. (or molar solubility), S, is the salt molar concentration in a saturated solution

  5. In general, we should not directly compare Kps to estimate solubility ratios! solubility: KPs:

  6. Numerical example: In NaCl 0,1 M solution In pure water 10000 times smaller!

  7. … while in pure water: s2=KPs → s= 1.3 10-5 M

  8. By means of balances … while in pure water: s2=KPs → s= 1.3 10-5 M

  9. Convention: we say that the precipitation of an ion is complete when its concentration is reduced one thousand times.

More Related