뒤로Buffers definitions
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A solution that resists drastic pH changes by neutralizing added acids or bases using a weak acid and its conjugate base or vice versa. Weak Acid
A substance that partially dissociates in water, providing limited H+ ions, and forms the acidic component of a buffer. Conjugate Base
A species formed when a weak acid loses an H+ ion, often paired with a metal in buffer solutions for stability. pH
A measure of hydrogen ion concentration, indicating the acidity or basicity of a solution, which buffers help stabilize. Buffer Capacity
The effectiveness of a buffer, which increases with higher concentrations of weak acid and conjugate base. Buffer Range
The ratio window (10:1 to 1:10) of weak acid to conjugate base concentrations where a buffer works most effectively. Strong Acid
A substance that completely dissociates in water, providing a high concentration of H+ ions, which can destroy buffers if added in excess. Strong Base
A substance that fully dissociates in water, yielding a high concentration of OH- ions, capable of overwhelming a buffer. Half Equivalence Point
The stage in a titration where equal amounts of weak acid and conjugate base exist, resulting in an ideal buffer. Neutralization
The process where an acid and a base react to minimize pH changes, central to how buffers function. Molarity
A unit expressing concentration as moles of solute per liter of solution, crucial for buffer calculations. Titration
A laboratory technique involving gradual addition of one solution to another to study reactions, often used to analyze buffer behavior. Acid-Base Pair
A combination of a weak acid and its conjugate base or a weak base and its conjugate acid, forming the foundation of buffer systems. Dilution
The process of adding water to a solution, which does not affect buffer effectiveness due to proportional concentration changes.
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