1. Equilibrium Equilibrium Constant, K (or K eq ) describes conditions AT equilibrium CaCO 3(calcite) + H +  Ca 2+ + HCO 3 -

2. Activity Sometimes called ‘effective concentration’, which is misleading and reflects a poor understanding of the property… Think of more of the effect the rest of a solution has on how easily two ions come together..

3. Activity For solids or liquid solutions: a i =X i  i For gases: a i =P i  i = f i For aqueous solutions: a i =m i  i X i =mole fraction of component i P i = partial pressure of component i m i = molal concentration of component i

4. Activity Coefficients Where do they come from?? The standard state for dissolved ions is actually an infinitely dilute solution… Activity of phases - gases, minerals, and bulk liquids (H 2 O) are usually pretty close to 1 in waters Dissolved molecules/ ions have activity coefficients that change with concentration (ions are curved lines relating concentration and activity coefficients, molecules usually more linear relation)

5. Application to ions in solution Ions in solutions are obviously nonideal mixtures! a i =  i m i The activity coefficient,  i, is found via some empirical foundations Dependent on the other ions in water…

6. Dissolved species  i First must define the ionic strength (I) of the solution the ion is in: Where m i is the molar concentration of species i and z i is the charge of species I

7. Activity Coefficients Debye-Huckel approximation (valid for I: Where A and B are constants (depending on T, see table 10.3 in your book), and a is a measure of the effective diameter of the ion (table 10.4)

8. Different ways to calculate  i Limiting law Debye-Huckel Davies TJ, SIT models Pitzer, HKW models

10. Neutral species Setchnow equation: Log  n =k s I For activity coefficient (see table 4-2 for selected coefficients)