A buffer solution is related to Le Chatelier’s Principle as it demonstrates the principle in action. According to Le Chatelier’s Principle, a system at equilibrium will respond to any change in conditions such as temperature, pressure, or concentration by shifting its position of equilibrium to counteract the change. A buffer solution contains both a weak acid and its conjugate base or a weak base, and its conjugate acid. When a strong acid or base is added to the buffer solution, the buffer system reacts to maintain the pH of the solution, by either neutralizing the added acid or base, or by producing the excess acid or base, thereby shifting the equilibrium position to counteract the change in concentration of the added species. This demonstrates Le Chatelier’s Principle in action, as the buffer system responds to a change in concentration by adjusting its equilibrium position to maintain the pH of the solution.
