Water, electrolyte and acid-base balance

Published on 02/03/2015 by admin

Filed under Internal Medicine

Last modified 22/04/2025

Print this page

rate 1 star rate 2 star rate 3 star rate 4 star rate 5 star
Your rating: none, Average: 0 (0 votes)

This article have been viewed 1427 times

11 Water, electrolyte and acid-base balance

Salt and volume distribution

Na+ retention and excretion control extracellular volume (water will passively follow salt). Systemic baro-receptors (carotid sinus, aortic arch) ‘sense’ changes in arterial tone (a function of cardiac output and systemic vascular resistance). A fall in effective arterial blood volume (EABV) activates the sympathetic nervous system, leading to Na+ retention by the kidney. With an expanded EABV, increased renal Na+ loss occurs.

Sodium

Disorders of sodium are more accurately disorders of water than of sodium, as disturbances of sodium concentration are mainly caused by a disturbance of water balance. The danger posed by a low or high serum Na+ comes from both the electrolyte abnormality and its correction; the skull does not allow the brain to change in volume, so movement of water into the CNS risks increased intracranial pressure (and eventually tentorial herniation). Equally, movement of water out of the brain can lead to sudden and irreversible osmotic injury (central pontine myelinolysis (CPM)).

Hyponatraemia

Hyponatraemia (plasma Na+ < 135 mmol/L) is common in hospitalized patients, but symptomatic hyponatraemia is very much less common — and more dangerous.

Hyponatraemia with a normal extracellular volume

Excess body water results from an abnormally high intake.

Hypernatraemia

Defined as a serum Na+ > 145 mmol/L, hypernatraemia is almost always due to a water deficit. As osmolality increases, water leaves cells, including the cells in the brain. The brain compensates over time by retaining organic solutes, increasing cellular tonicity and so reducing water loss into the hyperosmolar ECF. Sudden correction may lead to a rapid gain of water with intracranial expansion of the brain and tentorial herniation. Symptoms and signs include thirst, weakness and confusion progressing to coma and fits.

Potassium

Most of the total body K+ (about 3500 mmol) is intracellular, with only 2% (or 70 mmol) in the extracellular space. Total body K+ is kept in strict balance; dietary intake amounts to about 100 mmol/day, with 90 mmol/day lost in the urine (and the rest in stool). This gives a normal range for serum K+ of 3.5–5.5 mmol/L; this is, however, a poor indicator of total body potassium.

Abrupt changes in K+ can be life-threatening, so a number of compensatory mechanisms exist to maintain serum K+ within the normal range.

Hyperkalaemia

Always exclude spurious hyperkalaemia — usually due to haemolysis after phlebotomy, particularly with abnormal cells. Hyperkalaemia is a relative state; patients with longstanding renal impairment can tolerate K+ of up to 7 mmol/L, while those accustomed to low–normal K+ may develop dangerous arrhythmias if K+ is about 6.0. It is never safe to ignore a K+ > 6.5 mmol/L.

Management (See Emergencies in medicine p. 711)

Hypokalaemia

Magnesium

Magnesium contributes to all energy (ATP)-requiring reactions, as well as cell membrane function, nerve conduction and muscle contraction. Plasma Mg2+ is tightly controlled by the kidney (modifying urinary losses) within a normal range of 0.75–1.1 mmol/L (1.5–2.2 mEq/L).

Phosphate

Phosphate is essential to almost all biochemical systems, and its control is closely linked to that of calcium. Active vitamin D3 increases dietary phosphorus absorption, with most (80%) total body phosphate (the inorganic fraction of phosphorus) found in the skeleton. Sodium–phosphate co-transporters in the kidney retain phosphate (depending on oral phosphorus intake) for a normal plasma range of 0.8–1.4 mmol/L (3.0–4.5 mg/dL) (higher in children). Parathyroid hormone and phosphatonins inhibit renal reabsorption to encourage phosphate wasting in response to a rising plasma phosphate.

Check Ca2+, Na+, K+, renal function and bicarbonate, glucose and parathormone levels.

Acid–base disorders

The concentration of hydrogen ions [H+] is tightly regulated in all body compartments. In extracellular fluid (including blood), the normal pH range is 7.38–7.42 (pH = negative log of [H+]). To maintain pH within this narrow range, buffering systems work in concert with the lungs and kidneys to minimize sudden changes in [H+].

Diagnostic tests

Urinary anion gap (UAG). Measurement is useful in distinguishing a renal tubular acidosis from an extra-renal bicarbonate loss such as in diarrhoea. Again, it is the difference between the major measured anions and cations:

image

In diarrhoea, urinary ammonium chloride (NH4Cl) is high, giving a negative UAG. A positive (or zero) UAG is seen in renal disease and distal renal tubular acidosis (low urinary NH4 production).

Metabolic acidosis

Metabolic acidosis (Fig. 11.4) is defined as a fall in systemic pH to < 7.35 with a primary decrease in plasma bicarbonate. It may be caused by excess generation or retention of acid, or by increased bicarbonate losses.

Metabolic acidosis is often associated with serious underlying disease, and history and examination should be directed toward a global patient assessment, with particular attention to haemodynamic stability and excluding sepsis.

If the systemic pH falls < 7.2, acidaemia leads to impaired cardiac contractility, vasodilatation, resistance to catecholamines and ineffective oxygen delivery. This reflects the severity of the associated insult.

Metabolic acidosis with high AG

Causes

Metabolic acidosis commonly occurs, e.g. in cholera, when there is an expected normal AG acidosis owing to massive gastrointestinal losses of bicarbonate but the AG is often increased owing to renal failure and lactic acidosis as a result of hypovolaemia.

Clinical features. There is stimulation of respiration, leading to air hunger or Kussmaul respiration. Acidosis increases delivery of oxygen to the tissues by shifting the oxyhaemoglobin dissociation curve to the right but it also leads to inhibition of 2,3DPG production, which returns the curve towards normal. Cardiovascular dysfunction is common, as acidosis is negatively ionotropic. Severe acidosis is often associated with confusion and fits.

Metabolic alkalosis

The retention of bicarbonate or loss of H+ leads to a metabolic alkalosis (Fig. 11.4), usually due to primary chloride or potassium depletion. Any significant loss of Cl (vomiting, diuretics) will lead to HCO3 retention to maintain electrical neutrality. Any cause of secondary hyperaldosteronism (e.g. hypovolaemia) will lead to Na+ retention, and potassium and H+ depletion. Hypoventilation may buffer an evolving alkalosis to a degree, and modest elevations of PCO2 are usual.

Share this: