Ch.12 - Advanced Topics in EquilibriumWorksheetSee all chapters
All Chapters
Ch.1 - Chemical Measurements
Ch.2 - Tools of the Trade
Ch.3 - Experimental Error
Ch.4 + 5 - Statistics, Quality Assurance and Calibration Methods
Ch.6 - Chemical Equilibrium
Ch.7 - Activity and the Systematic Treatment of Equilibrium
Ch.8 - Monoprotic Acid-Base Equilibria
Ch.9 - Polyprotic Acid-Base Equilibria
Ch.10 - Acid-Base Titrations
Ch.11 - EDTA Titrations
Ch.12 - Advanced Topics in Equilibrium
Ch.13 - Fundamentals of Electrochemistry
Ch.14 - Electrodes and Potentiometry
Ch.15 - Redox Titrations
Ch.16 - Electroanalytical Techniques
Ch.17 - Fundamentals of Spectrophotometry
BONUS: Chemical Kinetics
Davies Equation 

Concept #1: When the size parameter of the ion is unknown we can instead use the Davies Equation

Example #1: Calculate the activity coefficient of Ca2+ in 0.025 M Ca3(PO4)2.

Ionic Salts & Solubility 

Concept #2: Cations are able to create acidic or neutral solution and increasing the basicity will increase their solubility. 

Concept #3: Anions are able to create basic or neutral solution and increasing the acidity will increase their solubility. 

Example #2:

BaCO3 is the slightly soluble ionic salt that results from the reaction between Ba(OH)2 and H2CO3. Identify the effect of increasing acidity on the solubility of the given compound. 

 

Example #3:

Which salts will be more soluble in an acidic solution than in pure water?

a. CuBr

b. Ag2SO4

c. BaSO3

d. Sn(OH)2

e. KClO4