Henderson-Hasslbach equation

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The document discusses the Henderson-Hasselbach equation, which relates pH and the concentration of hydrogen ions [H]. It notes that pH of 7.4 corresponds to a hydrogen ion concentration of 40 nmol/L. The equation shows that an increase in pH means a decrease in [H] concentration, and that a change of 1 pH unit corresponds to a 10-fold difference in [H]. The body maintains high [H] levels, and buffers help stabilize pH. The Henderson-Hasselbach equation is useful for understanding pH and [H] concentration.

Henderson-Hasselbach equation
Fadail Al Haddad

Whatis PH ?
• [H] = .000 000 04 EQL
• [H] = 40 n eql
• -log [H] = 7.4
• Pour of [H] = 7.4
• Ph= 7.4
SO INCREASE PH = DECREASE [H] because( – log)
ALSO one different in ph means 10 different in [H]

The document discusses buffers and how they maintain pH levels in the blood. It specifically focuses on the carbonic acid-bicarbonate buffer system, which is the most important buffer. This buffer system involves the equilibrium between carbonic acid, which donates hydrogen ions, and bicarbonate ions, which accept hydrogen ions. This helps regulate pH levels and protects against changes that could be harmful or fatal.

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Buffers resist changes in pH upon the addition of small amounts of acid or base. They work by providing conjugate acid-base pairs that absorb added H+ or OH- ions. Common buffer systems include acetic acid/sodium acetate and phosphoric acid/sodium phosphate. The Henderson-Hasselbalch equation relates a buffer's pH to the pKa of the acid/base pair and the concentrations of the components. Buffers have important applications in biological systems like blood and pharmaceutical products where a stable and precise pH is required.

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