1) A buffer (either acidic or basic) and its buffering capacity. *[AP Notes on Calculating pH when Adding Strong Base to a Acid Buffer] (AP Book: Section 15.3) |
1) A buffer (either acidic or basic) and its buffering capacity. (AP Book: Section 15.3) *[AP Notes on Calculating pH when Adding Strong Base to a Acid Buffer] |
What happens?
Answer
For any solution, the added strong acid (therefore H+) or the strong base (therefore OH1-) will be consumed by the available acid/base until there is either no more added strong acid/strong base or the acid/base in the solution is gone. This is determined by STOICHIOMETRY calculation (net ionic equation is 1 H+ + 1 OH1- --> 1 H2O). Then you re-evaulate the type of bucket (all the resulting species and their concentration in the bucket).
So what does this mean for Calculating method for Equilibrium systems?
The stoichiometry calculation and resulting concentration changes for all the species in the bucket will come before you determine the major species in the bucket (STEP 1) and the resulting analysis of which reaction is "running the show" in the bucket.
What are the most common calculations using this concept (adding strong acid/base to a solution)?
1) A buffer (either acidic or basic) and its buffering capacity. (AP Book: Section 15.3)
The following are major points on the Titration Curve and notes on how to calculate the pH of the solution.