Acidity and basicity are ways of measuring the concentration of protons in a solution--protons are acidic, so an acidic solution is characterized by having a high [H+]. One equation that is commonly used in biology and chemistry is the Henderson-Hasselbalch equation (which I primarily chose to write on because of its cool name). This equation relates the pH of a solution (the negative log of [H+]) with the chemical's acidity (pKa--an inherent property of the chemical) and its concentrations in both its acidic ([HA]) and basic ([A-]) forms: \[pH=pK_a+log(\frac{[A^-]}{[HA]})\]If we imagine a solution of a chemical with a defined pKa and a known ratio of \(\frac{[A^-]}{[HA]}\), we can easily calculate the pH of that solution using this equation. This equation is especially useful in buffers--solutions whose pH's change very little even when strong acids or strong bases are added.
Sources:
https://en.wikipedia.org/wiki/Henderson%E2%80%93Hasselbalch_equation
https://en.wikipedia.org/wiki/Buffer_solution
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