Clutch Prep is now a part of Pearson
Ch.7 - Activity and the Systematic Treatment of 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
Ionic Strength of Soluble Salts
Activity Coefficients
pH Revisited

In this section we now include activity coefficients when calculating the pH values of solutions. 

pH Revisited Calculations

Example #1: If at 50 oC the ionization of pure water, Kw, is 7.94 x 10-14 what is the pH of a neutral solution?

a) 7.00

b) 6.55

c) 13.10

d) Since Kw is a constant the number doesn’t change. 

Example #2: What would be the pH of the same pure water when it contains 0.005 M NaBr at 50 oC? 

Example #3: Find the pH of a saturated solution of Barium hydroxide, Ba(OH)2 when dissolved in 0.05 LiNO2. The Ksp of Ba(OH)2 is 5.0 x 10-3