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A solution that resists drastic changes in pH, containing a weak acid and its conjugate base or a weak base and its conjugate acid. Weak Acid
An acid that partially dissociates in solution, such as HF, contributing to buffer formation. Conjugate Base
The species formed when a weak acid loses a proton, often combined with a metal, like NaF. pH
A measure of the acidity or basicity of a solution, influenced by the presence of buffers. Buffer Capacity
The ability of a buffer to neutralize added acids or bases, enhanced by higher concentrations of buffer components. Buffer Range
The pH range over which a buffer effectively neutralizes added acids or bases, typically between a 10:1 or 1:10 ratio. Ideal Buffer
A buffer where the concentrations of the weak acid and conjugate base are equal, providing optimal pH stability. Half Equivalence Point
The point in a titration where the concentration of the weak acid equals that of its conjugate base, forming an ideal buffer. Henderson-Hasselbalch Equation
An equation used to calculate the pH of a buffer solution, involving pKa and the ratio of conjugate base to weak acid. pKa
The negative logarithm of the acid dissociation constant, used in the Henderson-Hasselbalch equation to find buffer pH. Strong Acid
An acid that completely dissociates in solution, potentially destroying a buffer if added in excess. Strong Base
A base that completely dissociates in solution, potentially destroying a buffer if added in excess. Molarity
A measure of concentration, used to express the amount of solute in a given volume of solution, relevant in buffer calculations. Titration
A technique to determine the concentration of a solution, involving the gradual addition of a titrant to a known volume of analyte. Neutralization
The reaction between an acid and a base to form water and a salt, a key process in buffer function.
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