Buffers Buffers are solutions in which the pH remains relatively constant when small amounts of acid or base are added made from a pair of chemicals: a.

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Presentation transcript:

Ch. 15 – 3 Buffer Solutions p. 565-567

Buffers Buffers are solutions in which the pH remains relatively constant when small amounts of acid or base are added made from a pair of chemicals: a weak acid and one of it’s salts (conjugate base); or a weak base and one of it’s salts (conjugate acid)

Buffers A buffer system is better able to resist changes in pH than pure water Since it is a pair of chemicals: one chemical neutralizes any acid added, while the other chemical would neutralize any additional base AND, they produce each other in the process!!!

Buffers Example: Ethanoic (acetic) acid and sodium ethanoate (also called sodium acetate) The buffer capacity is the amount of acid or base that can be added before a significant change in pH

Buffers Buffers that are crucial to maintain the pH of human blood: 1. carbonic acid (H2CO3) & hydrogen carbonate (HCO31-) 2. dihydrogen phosphate (H2PO41-) & monohydrogen phoshate (HPO42-)