Buffer-pH and Acid-Base Balance

Buffer = An aqueous solution of a weak acid and its conjugated salt or a weak base with its conjugated salt pH = A measure of the acidity or basicity of a solution Conjugate salt = The species formed when a weak acid or base donates or accepts a proton Acid-base balance = The maintenance of a constant pH in biological and chemical systems

Buffers in solutions = Prevent large changes in pH when small amounts of strong acid or base are added Biological and chemical reactions = Require a constant pH for optimal progression Usefulness of buffers = Maintain the pH at a constant value in systems Change in pH for buffers = Occurs but is not as significant as in non-buffered solutions

P = -log [H+] = Equation for calculating the negative logarithm of hydrogen ion concentration pH = -log [H+] = Expression for measuring the acidity or basicity of a solution Buffer capacity = Ability of a buffer solution to resist changes in pH upon addition of acid or base Conjugate base concentration = Amount of the species formed when a weak acid donates a proton

Buffer-pH relationship = Used to maintain stable conditions for enzymatic reactions in biological systems Buffer solutions = Applied in laboratory settings to control and stabilize pH levels during experiments Acid-base balance in biological systems = Critical for maintaining homeostasis and proper functioning of cells Conjugate salt formation = Occurs when weak acids or bases react to maintain equilibrium in solutions