CBSE Class 12-science Answered
how to calculate the degree of disociation?
Asked by Mayuri dave | 12 Jul, 2013, 08:28: AM
Expert Answer
Step 1. The species present before dissociation are identified as Brönsted-Lowryacids / bases.
Step 2. Balanced equations for all possible reactions i.e., with a species acting both as acid as well as base are written.
Step 3.The reaction with the higher Ka is identified as the primary reaction whilst the other is a subsidiary reaction.
Step 4.Enlist in a tabular form the following values for each of the species in the primary reaction
- (a) Initial concentration, c.
- (b) Change in concentration on proceeding to equilibrium in terms of ?, degree of dissociation.
- (c) Equilibrium concentration.
Step 5.Substitute equilibrium concentrations into equilibrium constant equation for principal reaction and solve for ?.
Answered by | 12 Jul, 2013, 02:55: PM
Concept Videos
CBSE 12-science - Chemistry
Asked by hannamaryphilip | 17 Apr, 2024, 11:20: PM
ANSWERED BY EXPERT
CBSE 12-science - Chemistry
Asked by sameerteli003 | 08 Apr, 2024, 11:48: PM
ANSWERED BY EXPERT
CBSE 12-science - Chemistry
Asked by rashmij34 | 27 Feb, 2024, 04:42: PM
ANSWERED BY EXPERT
CBSE 12-science - Chemistry
Asked by sagarmishra | 27 Feb, 2024, 04:01: PM
ANSWERED BY EXPERT
CBSE 12-science - Chemistry
Asked by kalandi.charan.407 | 08 Feb, 2024, 01:42: PM
ANSWERED BY EXPERT
CBSE 12-science - Chemistry
Asked by premkhare2006 | 24 Jan, 2024, 09:50: AM
ANSWERED BY EXPERT
CBSE 12-science - Chemistry
Asked by saritanohar22 | 13 Jan, 2024, 01:25: PM
ANSWERED BY EXPERT
CBSE 12-science - Chemistry
Asked by kaushikmisty07 | 31 Dec, 2023, 11:42: AM
ANSWERED BY EXPERT
CBSE 12-science - Chemistry
Asked by kamlesh.kumar.malee | 20 Dec, 2023, 06:59: AM
ANSWERED BY EXPERT
CBSE 12-science - Chemistry
Asked by varinder2149 | 10 Dec, 2023, 08:21: PM
ANSWERED BY EXPERT