The normal pH of blood is 7.40 ±0.05 and is controlled in part by the H3 CO3 / HCO3^- buffer sys

step 1 The equation for the dissociation of carbonic acid is given here. I wrote it down beforehand. An

The normal pH of blood is 7.40 ±0.05 and is controlled in...

The normal pH of blood is $7.40 \pm 0.05$ and is controlled in part by the $\mathrm{H}_{3} \mathrm{CO}_{3} / \mathrm{HCO}_{3}^{-}$ buffer system. (a) Assuming that the $K_{\mathrm{a}}$ value for carbonic acid at $25^{\circ} \mathrm{C}$ applies to blood, what is the $\left[\mathrm{H}_{2} \mathrm{CO}_{3}\right] /\left[\mathrm{HCO}_{3}-\right]$ ratio in normal blood? (b) In a condition called acidosis, the blood is too acidic. What is the $\left[\mathrm{H}_{2} \mathrm{CO}_{3}\right] /\left[\mathrm{HCO}_{3}-\right]$ ratio in a patient whose blood $\mathrm{pH}$ is 7.20$?$

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Key Concepts

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation provides a practical way to relate the pH of a solution to the pKa and the ratio of the concentrations of the conjugate base and the weak acid. It is essential for calculating the necessary proportions of acid and conjugate base to achieve or maintain a desired pH.

pKa and Its Relationship to pH

The pKa value is a logarithmic measure of the acid dissociation constant (Ka) and indicates the strength of a weak acid. The relationship between pH, pKa, and the ratio of the concentrations of the conjugate base and the weak acid is critical in understanding how buffers maintain pH.

Acid-Base Equilibria

Acid-base equilibria describe the balance between an acid and its conjugate base in solution. This equilibrium is established through the dissociation of the weak acid, and it is characterized by an equilibrium constant (Ka) that quantifies the acid’s tendency to donate protons.

Buffer Systems

Buffer systems are solutions that resist changes in pH when small amounts of acid or base are added. They typically consist of a weak acid and its conjugate base, or a weak base and its conjugate acid, which work together to mitigate fluctuations in hydrogen ion concentration.