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AP Chemistry Unit 8.9 Practice Problems - Henderson-Hasselbalch Equation

Identify the pH of a buffer solution based on the identity and concentrations of the conjugate acid-base pair used to create the buffer. The pH of the buffer is related to the pK, of the acid and the concentration ratio of the conjugate acid-base pair. This relation is a consequence of the equilibrium expression associated with the dissociation of a weak acid, and is described by the Henderson-Hasselbalch equation. Adding small amounts of acid or base to a buffered solution does not significantly change the ratio of [A]/[HA] and thus does not significantly change the solution pH. The change in pH on addition of acid or base to a buffered solution is therefore much less than it would have been in the absence of the buffer. EQN: pH = pKa + log[A]/[HA]