When the ratio of the bicarbonate [HCO3-] to carbonic acid $\left[\mathrm{H}_{2} \mathrm{CO} 2\right]$ is $30: 2$, the systemic $\mathrm{pH}$ is likely to be:
a. The $\mathrm{pH}$ is affected only by $[\mathrm{H}+]$ in the blood.
b. Above 7.4
c. Lower than 7.4
d. Equals to 7.4

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Question

When the ratio of the bicarbonate [HCO3-] to carbonic acid $\left[\mathrm{H}_{2} \mathrm{CO} 2\right]$ is $30: 2$, the systemic $\mathrm{pH}$ is likely to be:
a. The $\mathrm{pH}$ is affected only by $[\mathrm{H}+]$ in the blood.
b. Above 7.4
c. Lower than 7.4
d. Equals to 7.4

Accepted Answer

***B*** ∻Key Concept∻ ⚹Henderson-Hasselbalch equation⚹ ∻Explanation∻ ⚹The pH is determined by the ratio of bicarbonate to carbonic acid, as described by the Henderson-Hasselbalch equation: pH = pKa + log([HCO3-]/[H2CO3]). A higher ratio indicates a higher pH, which would be above the normal blood pH of 7.4 in this case◊What is the Henderson-Hasselbalch equation and how can it be used to calculate pH in a buffer system?⍭ Generate me a similar question◊⚹

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