## How acid–base balance works

Normal arterial pH is approximately **7.35–7.45**, although laboratory reference intervals vary. That narrow range is maintained through a sequence of four processes: the body produces acid, buffers limit the immediate change in pH, the lungs regulate carbon dioxide, and the kidneys regulate bicarbonate and eliminate nonvolatile acid.

### Step 1: Metabolism continuously produces acid

Cells generate two broad categories of acid:

- **Volatile acid:** Aerobic metabolism produces carbon dioxide (CO₂). In water, CO₂ combines with water to form carbonic acid, which can dissociate into hydrogen ions (H⁺) and bicarbonate (HCO₃⁻). Because CO₂ can be exhaled, the lungs can eliminate this acid load.
- **Nonvolatile or fixed acid:** Metabolism of sulfur-containing amino acids and phosphates generates acids that cannot be exhaled. Lactate, ketoacids, and ingested toxins can add much larger acid loads during illness. These acids must ultimately be metabolized or excreted by the kidneys.

The central reversible reaction is:

**CO₂ + H₂O ⇌ H₂CO₃ ⇌ H⁺ + HCO₃⁻**

The enzyme carbonic anhydrase rapidly accelerates this reaction in red blood cells, renal tubular cells, and other tissues. The reaction can move in either direction. Adding CO₂ pushes it toward more hydrogen ions; removing CO₂ pulls it toward less hydrogen ion.

### Step 2: Buffers limit the immediate pH change

When hydrogen ions appear, buffers bind some of them within seconds. The bicarbonate system is the principal extracellular buffer, while hemoglobin, intracellular proteins, and phosphate also contribute.

For example, when a nonvolatile acid releases H⁺, bicarbonate binds that H⁺ and is converted through carbonic acid into CO₂ and water. The lungs then exhale the generated CO₂. The blood bicarbonate concentration falls because bicarbonate was consumed while buffering the acid.

This explains an important laboratory pattern: in **metabolic acidosis**, a low bicarbonate is not merely a marker. It reflects bicarbonate consumption, bicarbonate loss, or impaired renal bicarbonate generation.

 InlinePopup label="What buffers can and cannot do" title="Buffering buys time but does not eliminate the acid load" tone="sky" analyticsId="acid-base-buffering-limits" 
Buffers reduce the immediate rise or fall in free hydrogen-ion concentration. They do not make the underlying acid disappear. Carbon dioxide created during bicarbonate buffering still has to be ventilated, while nonvolatile acid must be metabolized or excreted by the kidneys. If ventilation or kidney function is impaired, the compensatory pathway becomes less effective and acidemia can worsen rapidly.
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### Step 3: The lungs regulate carbon dioxide within minutes

Carbon dioxide production and alveolar ventilation determine arterial carbon dioxide tension (PaCO₂):

- If alveolar ventilation **increases**, more CO₂ is exhaled, PaCO₂ falls, the reaction shifts left, and pH rises.
- If alveolar ventilation **decreases**, CO₂ accumulates, PaCO₂ rises, the reaction shifts right, and pH falls.

This is why primary respiratory disorders are defined by their carbon dioxide change:

- **Respiratory acidosis:** inadequate effective ventilation causes CO₂ retention.
- **Respiratory alkalosis:** ventilation exceeds CO₂ production, causing excessive CO₂ removal.

Chemoreceptors respond to changes in carbon dioxide, pH, and oxygenation. In metabolic acidosis, increased ventilation can lower PaCO₂ within minutes. This response reduces the fall in pH but cannot replace bicarbonate or remove the original nonvolatile acid.

### Step 4: The kidneys preserve bicarbonate and excrete nonvolatile acid

The kidneys perform three related tasks:

1. **Reclaim filtered bicarbonate.** Nearly all filtered bicarbonate is normally returned to the blood, primarily in the proximal tubule. Failure to reclaim it causes urinary bicarbonate loss.

 LessonImage src="/api/assets/ff881da9-6680-4e84-8988-2586dd6139c7" alt="bicarbonate reabsorption in the proximal tubule2" size="medium" align="center" caption="Bicarbonate resorption in the proximal tubule." / 

2. **Excrete hydrogen ions as titratable acid.** Secreted H⁺ binds urinary buffers, especially phosphate, allowing acid to leave the body without lowering urine pH indefinitely.

 LessonImage src="/api/assets/85302a1c-b895-4efc-8d8f-88b0822acfa5" alt="phosphate transport in the proximal tubule 3" size="medium" align="center" caption="Phosphate in acid-base regulation in the kidneys." / 

3. **Generate and excrete ammonium.** Proximal tubular metabolism of glutamine produces ammonium (NH₄⁺) and new bicarbonate. Ammonium is ultimately trapped in the urine and excreted, while the new bicarbonate enters the blood. This pathway can increase substantially during sustained acidosis.

 LessonImage src="/api/assets/c451539e-c771-44c7-bdd6-458d5d8fcfca" alt="metabolism of ammonia in response to metabolic acidosis 2" size="medium" align="center" caption="Ammonia generation in kidney acid-base balance. You can see that as ammonia is created with the H+ that bicarbonate is resorbed into the blood." / 

The kidney response takes hours to begin and several days to reach its full effect. In chronic respiratory acidosis, persistently elevated CO₂ stimulates greater bicarbonate retention and net acid excretion. In chronic respiratory alkalosis, the kidneys excrete more bicarbonate. Kidney failure, hypoaldosteronism, tubular disease, or severe hyperkalemia can impair these responses.

 InlinePopup label="How ammonium creates new bicarbonate" title="Renal acid excretion replaces bicarbonate consumed by fixed acid" tone="violet" analyticsId="acid-base-ammonium-new-bicarbonate" 
Reclaiming filtered bicarbonate prevents bicarbonate loss but does not add new bicarbonate to the body. New bicarbonate is added when the kidney excretes acid as ammonium or titratable acid. For each hydrogen ion excreted with one of these urinary buffers, one bicarbonate is effectively returned to the extracellular fluid. This distinction explains why impaired ammonium excretion can cause metabolic acidosis even when urine pH is relatively low.
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### Step 5: pH depends on the relationship between bicarbonate and carbon dioxide

The Henderson–Hasselbalch relationship can be written as:

**pH = 6.1 + log[HCO₃⁻ / (0.03 × PaCO₂)]**

You do not need to calculate this equation at the bedside. Its value is conceptual: pH depends on the **ratio** of bicarbonate to dissolved carbon dioxide, not on either value alone.

- A fall in bicarbonate lowers the ratio and lowers pH unless ventilation also lowers CO₂.
- A rise in carbon dioxide lowers the ratio and lowers pH unless the kidneys retain more bicarbonate.
- A rise in bicarbonate or fall in carbon dioxide raises the ratio and raises pH.
- If bicarbonate and carbon dioxide change in the same direction and in the expected proportion, one is usually the primary disturbance and the other is compensation.
- If they change by an unexpected amount—or move in directions that cannot be explained by compensation—more than one primary disorder is present.

 LessonImage src="/lesson-media/acid-base/lung-kidney-buffer-balance.png" alt="Simplified illustration of lungs removing carbon dioxide and kidneys reclaiming bicarbonate and excreting hydrogen ions to maintain blood pH" caption="The lungs control the carbon dioxide side of the ratio; the kidneys control bicarbonate and net acid excretion." size="full" align="center" / 

A low pH is **acidemia**; a high pH is **alkalemia**. An **acidosis** is a process that pushes pH down, whereas an **alkalosis** pushes it up. These terms are not interchangeable. A patient can have metabolic acidosis and respiratory alkalosis at the same time, leaving the measured pH near the reference interval. Therefore, never stop after deciding that the pH is “normal.”

### Step 6: Primary disorders arise when one control system fails or is driven abnormally

| Primary disorder | Initial physiologic problem | Immediate effect | Expected compensation |
|---|---|---|---|
| Metabolic acidosis | Acid is added, bicarbonate is lost, or renal acid excretion fails | HCO₃⁻ falls and pH falls | Ventilation increases, lowering PaCO₂ |
| Metabolic alkalosis | Hydrogen ions are lost or bicarbonate is gained and retained | HCO₃⁻ rises and pH rises | Ventilation decreases modestly, raising PaCO₂ |
| Respiratory acidosis | Alveolar ventilation is inadequate | PaCO₂ rises and pH falls | Kidneys retain/generate HCO₃⁻ and excrete more acid |
| Respiratory alkalosis | Alveolar ventilation is excessive for CO₂ production | PaCO₂ falls and pH rises | Kidneys excrete more HCO₃⁻ and reduce net acid excretion |

Compensation is limited. Hypoventilation during metabolic alkalosis is constrained by the need to maintain oxygenation. Respiratory compensation for metabolic acidosis is constrained by respiratory muscle capacity and lung disease. Renal compensation is limited by kidney function, distal sodium delivery, potassium balance, and the time available for adaptation.

 InlinePopup label="Why compensation never means correction" title="Compensation changes the ratio—it does not remove the primary disorder" tone="sky" analyticsId="acid-base-compensation-not-correction" 
Compensation moves the pH toward normal by changing the other side of the bicarbonate-to-carbon-dioxide ratio. It does not eliminate the initiating process, and a simple compensatory response usually does not return pH completely to normal. If the measured response is greater or smaller than expected, suspect an additional primary disorder rather than “overcompensation.”
 /InlinePopup 

 InlinePopup label="Optional depth: the Stewart approach" title="A physicochemical view of acid–base physiology" tone="violet" analyticsId="acid-base-stewart-optional-depth" 
The traditional approach organizes disorders around bicarbonate and carbon dioxide. The Stewart model instead treats pH as dependent on carbon dioxide, the strong-ion difference, and the total concentration of weak acids such as albumin and phosphate. It can clarify complex intensive-care patterns—especially chloride-related acidosis, hypoalbuminemic alkalinizing effects, and multiple simultaneous processes—but it does not replace careful clinical interpretation. The physiologic bicarbonate approach remains an efficient first-line framework.

[Review the major diagnostic frameworks](https://pubmed.ncbi.nlm.nih.gov/19812535/)
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 LessonImage src="/api/assets/df8b933a-11af-4728-8336-c399cdc44bec" alt="HH_acid_base" size="large" align="center" caption="Acid Base Physiology" / 

## What the blood gas actually reports

| Value | What it represents | Typical arterial reference | Key caution |
|---|---|---:|---|
| pH | Net acid–base state | 7.35–7.45 | A near-normal value can conceal mixed disease. |
| PaCO₂ | Arterial partial pressure of CO₂ | 35–45 mmHg | Primarily reflects alveolar ventilation. |
| HCO₃⁻ | Calculated bicarbonate on most analyzers | 22–26 mmol/L | May differ slightly from chemistry total CO₂. |
| Base excess |  InlinePopup label="Estimated metabolic contribution after standardization" title="Estimated metabolic contribution after standardization" **Base excess (BE)** estimates the **metabolic component** of an acid–base disturbance. It represents the amount of strong acid or base required to titrate blood to a **pH of 7.40** under standardized conditions—typically **37°C and PaCO₂ 40 mmHg**—thereby removing the respiratory contribution. 
* **Positive BE:** Excess base → metabolic alkalosis or renal compensation for respiratory acidosis. 
* **Negative BE (base deficit):** Deficient base → metabolic acidosis or renal compensation for respiratory alkalosis. 
* Normal range: approximately **−2 to +2 mEq/L**. 

It is **calculated**, not directly measured, from the measured **pH and PaCO₂**, which determine bicarbonate, with adjustment for hemoglobin/buffering. A simplified approximation is: 
BE≈0.93([HCO3−​]−24.4+14.8(pH−7.40)) 
In practical terms, BE asks: **After normalizing CO₂, how much nonrespiratory acid or base remains?** /InlinePopup  | About −2 to +2 mmol/L | Helpful adjunct, not a replacement for the full analysis. |
| PaO₂ | Arterial partial pressure of oxygen | Context dependent | Interpret with inspired oxygen, age, altitude, and clinical setting. |

The serum chemistry bicarbonate is usually reported as **total carbon dioxide**. The blood-gas bicarbonate is commonly calculated from pH and measured carbon dioxide. Small differences are expected; large differences should prompt review of sampling time, processing, and specimen identity.

Preanalytical problems can create false patterns:

- Air bubbles tend to move the sample toward room-air gas values.
- Delayed analysis allows ongoing cellular metabolism to consume oxygen and generate carbon dioxide and acid.
- Excess liquid heparin can dilute the specimen.
- A sample drawn while ventilation or perfusion is rapidly changing may become obsolete within minutes.
- A mislabeled venous sample can mimic severe arterial hypoxemia.

## ABG or VBG?

A peripheral VBG is often sufficient for an initial **acid–base assessment** in a hemodynamically stable adult. Venous pH usually tracks arterial pH closely enough to identify clinically important acidemia or alkalemia. However:

- Venous carbon dioxide is not an exact substitute for arterial carbon dioxide.
- Venous oxygen tension must not be used to assess arterial oxygenation.
- Pulse oximetry estimates saturation but does not provide pH, ventilation, or a reliable value in every dyshemoglobinemia or low-perfusion state.

Choose an ABG when you need precise arterial oxygenation, an exact arterial carbon dioxide value, assessment of severe or changing respiratory failure, or clarification when the VBG and bedside picture disagree. Use co-oximetry when carbon monoxide exposure, methemoglobinemia, or another dyshemoglobinemia is suspected.

 InlinePopup label="Evidence: VBG versus ABG" title="Systematic review and meta-analysis: what is interchangeable?" tone="emerald" analyticsId="acid-base-vbg-abg-meta-analysis-pico" 
**Population:** Eighteen studies including 1,768 adults with paired peripheral venous and arterial samples in varied clinical settings.

**Intervention/exposure:** Peripheral venous blood-gas measurement.

**Comparator:** Paired arterial blood-gas measurement.

**Outcome:** Arterial pH averaged about 0.03 units higher than venous pH. Carbon-dioxide prediction intervals were too wide for exact substitution, and venous and arterial oxygen tensions compared poorly.

**Evidence base:** Systematic review and random-effects meta-analysis.

**Applicability limits:** Heterogeneity was extremely high, populations and sampling methods varied, and agreement is not the same as evidence that choosing a VBG produces equivalent patient outcomes. A 2024 systematic review found no studies directly testing clinical outcomes from the choice of sample.

**Practice meaning:** A VBG is often useful for screening acid–base status, but do not convert venous oxygen or carbon dioxide into assumed arterial values when precision changes the decision.

[Read the 2014 meta-analysis](https://pubmed.ncbi.nlm.nih.gov/24383789/) · [Read the 2024 systematic review](https://pubmed.ncbi.nlm.nih.gov/38856155/)
 /InlinePopup 

## Practice: explain the physiology before opening the answer

1. Why does bicarbonate fall when a nonvolatile acid is added to the blood?
2. Why can the lungs compensate for metabolic acidosis but not eliminate its cause?
3. What is the difference between reclaiming filtered bicarbonate and generating new bicarbonate?
4. Why can a patient have a near-normal pH despite two serious acid–base disorders?
5. Which measurements from a peripheral venous blood gas should not be treated as exact substitutes for arterial carbon dioxide or oxygen tension?

 InlineDropdown label="Show physiology answers" variant="block" tone="info" analyticsId="acid-base-physiology-practice-answers" 
1. Bicarbonate accepts hydrogen ions and is converted through carbonic acid into carbon dioxide and water. The bicarbonate concentration therefore falls as it buffers the added acid.
2. Increased ventilation removes carbon dioxide and raises the bicarbonate-to-carbon-dioxide ratio, limiting the fall in pH. It does not metabolize or excrete the original lactate, ketoacid, toxin, or other fixed acid.
3. Reclamation prevents filtered bicarbonate from being lost in urine. New bicarbonate is added to the extracellular fluid when the kidney excretes hydrogen ions as ammonium or titratable acid.
4. Opposing primary processes can move pH in opposite directions. For example, metabolic acidosis and respiratory alkalosis may coexist and produce a pH near the reference interval.
5. Venous carbon dioxide is not an exact arterial substitute, and venous oxygen tension must not be used to assess arterial oxygenation.
 /InlineDropdown 

## Summary

- Metabolism continuously produces carbon dioxide and nonvolatile acids.
- Buffers limit immediate changes in free hydrogen-ion concentration but do not eliminate the underlying acid load.
- The lungs regulate carbon dioxide within minutes by changing alveolar ventilation.
- The kidneys preserve filtered bicarbonate, generate new bicarbonate, and excrete nonvolatile acid over hours to days.
- pH depends on the relationship between bicarbonate and dissolved carbon dioxide.
- Acidemia and alkalemia describe the measured pH; acidosis and alkalosis describe processes that push pH down or up.
- A venous blood gas often supports an initial acid–base assessment, but arterial sampling is needed when precise arterial oxygenation or carbon dioxide measurement changes the decision.

## References

- Adrogué HJ, Gennari FJ, Galla JH, Madias NE. Assessing acid-base disorders. Kidney International. 2009. [Link](https://pubmed.ncbi.nlm.nih.gov/19812535/)
- Kraut JA, Madias NE. Metabolic acidosis: pathophysiology, diagnosis and management. Nature Reviews Nephrology. 2010. [Link](https://pubmed.ncbi.nlm.nih.gov/20308999/)
- Byrne AL, Bennett M, Chatterji R, et al. Peripheral venous and arterial blood gas analysis in adults: are they comparable? A systematic review and meta-analysis. Respirology. 2014. [Link](https://pubmed.ncbi.nlm.nih.gov/24383789/)
- Weimar Z, Smallwood N, Shao J, et al. Arterial blood gas analysis or venous blood gas analysis for adult hospitalised patients with respiratory presentations: a systematic review. Internal Medicine Journal. 2024. [Link](https://pubmed.ncbi.nlm.nih.gov/38856155/)