3. The Henderson-Hasselbalch equation can be written for a base instead of an acid: A student needs to create a buffer of pH 9.8. a) What would the pOH of this buffer be? b) Which base, carbonate or pyridine would be best to use for this buffer? Why? c) What is the ratio of [Acid]/[Base] necessary to create a buffer of this pH? d) What mass of the base you chose is required to prepare half a liter of this buffer with an [Acid] =1.50 M? e) Which would have a higher buffer capacity, a buffer built to have an [Acid] of 1.50 M or one to have a [Base] of 1.50 M? Why?

define the buffer capacity. a) buffer capacity is the amount of acid that can be added until all of the acid is used up b) buffer capacity is the amount of base that can be added until all of the base is used up c) buffer capacity is the amount of acid that can be added until all of the base is used up d) buffer capacity is the amount of acid ir base that can be added to a buffer without destroying its effectiveness e) buffer capacity is the amount of base that can be added until all of the acid is used up

50.0 mL of 0.25 M potassium nitrate with 30.0 mL of 0.25 M nitric acid.  1) Determine if it yields a buffer or not and if it does not form a buffer, explain why not. If the combination does yield a buffer, calculate its pH.

1. Explain how a buffer made of hydrofluoric acid (0.20M) and fluoride ion (0.20M) adjusts to a small amount of added NaOH. 2. Calculate the amount of 0.1M NaOH that must be added to destroy the buffer solution from question 1.