CHEM1100 Lecture Notes - Lecture 10: Acid Dissociation Constant, Lattice Energy, Supersaturation

53 views3 pages
20 Jul 2018
School
Department
Course
Professor

Document Summary

Initial concentrations- before there is any dissociation of the acid: change when dissociation occurs, equilibrium concentrations are a sum of the initial concentration and change. Salt solubility: all ionic solids have some solubility in water , some are very soluble (e. g. nacl, others are very sparingly soluble (sometimes called insoluble , e. g. agbr, hgbr2) Ionic compounds dissolve in water when the ion-dipole attractions overcome both ion-ion and diploe-dipole attractions. Dissolution equilibrium: the equilibrium constant for this heterogenous equilibrium, nacl(s) na+(aq) + cl-(aq) Ksp = [na+][cl-: this equilibrium constant has a special name: solubility product ksp, ksp, as all equilibrium constant, depends on temperature. If the molar solubility of agbr is 6. 9 x 10-7mol/l, then s = [ag+] = [br-] = 6. 9 x 10-7mol/l. And ksp = [ag+][br-] = s2 = 4. 8 x 10-13 (note that the s has the unit mol/l, while the equilibrium constant ksp is dimensionless)

Get access

Grade+20% off
$8 USD/m$10 USD/m
Billed $96 USD annually
Grade+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
40 Verified Answers
Class+
$8 USD/m
Billed $96 USD annually
Class+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
30 Verified Answers

Related textbook solutions

Related Documents

Related Questions