The Henderson-Hasselbalch equation is a valuable tool that can be used to understand the pH of a solution at equilibrium. The equation is often used in biochemistry, especially when studying proteins and enzymes.
How to use the Henderson-Hasselbalch equation?
The Henderson-Hasselbalch equation is used to calculate the pH of a buffer solution. It can also be used to calculate the buffer capacity or protein stability, but most commonly it’s used as a tool for calculating how much acid or base needs to be added in order to change the pH of a solution.
To use it, you must know two things: the ratio of your weak acid and its conjugate base (HAc and HAc^-) respectively, and their concentrations. Then:
Henderson-Hasselbalch equation derivation
The Henderson-Hasselbalch equation is used to calculate the pH of a solution that has been buffered by weak acid and base.
The formula is derived from Le Chatelier’s principle, which states that when a system at equilibrium is disturbed, it will shift to counteract the change. In this case, if you add an acid or base to an otherwise neutral solution and then try to measure its pH directly (using say pH paper), you will get a different reading than what would have been predicted from just adding those ingredients alone. This discrepancy arises because adding additional amounts of strong acids or bases affects the relative concentrations of H+ cations in the solution compared with OH- anions; when these ratios are changed too much from their original state, it causes shifts backward in terms of what was originally measured by your test strips/paper
Buffer pH in the calculator’s results
The buffer capacity of a solution can be described in terms of the amount of acid or base needed to raise or lower the pH by one unit. It’s usually measured as millimoles per liter (mM). The number we use for our formula, pKa, is dependent on both the concentration and nature of your buffers.
The Henderson–Hasselbalch equation can be used to calculate the amount of acid and conjugate base to be combined for the preparation of a buffer solution having a particular pH, as demonstrated in the following problem.
The Henderson Hasselbalch equation is an approximate equation that shows the relationship between the pH or pOH of a solution and the pKa or pKb and the ratio of the concentrations of the dissociated chemical species.
The Henderson-Hasselbalch equation describes the relationship between blood pH and the components of the H2 CO3 buffering system. This qualitative description of acid/base physiology allows the metabolic component to be separated from the respiratory components of acid/base balance.