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A complex yet elegant system of chemical buffers together with highly specialized mechanisms of the lungs and kidneys continuously work in tandem to ensure a precise balance of water, electrolytes, and pH in both the intracellular and extracellular compartments of the human body. Although these systems display impressive resilience and responsiveness to perturbation by illness or injury, they do have limits, at which point medical evaluation and treatment are required.
This chapter describes the various fluid compartments in the body and reasons for differences in composition between these compartments. Laboratory testing algorithms are used to investigate and treat perturbations of water and electrolytes in pathologic settings, including the role of such simple tests as urine electrolytes. Similarly, testing algorithms and mnemonic tools are presented to diagnose and manage disturbances in acid-base homeostasis. The clinical laboratorian needs to understand the nuances and pitfalls associated with these algorithms and associated tests to provide accurate and meaningful results to the clinician.
Adaptation to terrestrial life led to the evolution of physiologic systems to maintain the composition of the internal milieu of animals, including humans. These systems require the interaction of multiple organ systems such as the kidneys, lungs, heart, liver, brain, and lymphatics. In particular, a variety of chemical buffers and highly specialized mechanisms of the lungs and kidneys work together to regulate water, electrolytes, and pH between and within intracellular and extracellular compartments. Perturbations in the dynamic equilibria that exist for water, electrolytes, and pH may arise from external (e.g., trauma, changes in altitude, ingestion of toxic substances) or internal (e.g., normal metabolism, disease state) sources. Endogenous correction of these imbalances may not always be adequate; at these times, the clinical laboratory can provide valuable information for guiding therapy. a
a Laboratories should verify that the values presented in this chapter, including the reference intervals are appropriate for use in their own settings.
During gestation, ≈90% of fetal body weight is water. Water is 70% of body weight for full-term infants. Water gradually decreases as percent of body weight, so that it accounts for 60% of body weight in adolescents and adult males and ≈55% for adult females. As depicted in Fig. 50.1 , approximately two-thirds of total body water (TBW) is distributed into the intracellular fluid (ICF) compartment, and one-third exists in the extracellular fluid (ECF) compartment. The ECF may be further subdivided into interstitial (≈75% of ECF) and intravascular (≈25% of ECF) compartments, which are separated by the capillary endothelium. The average adult has 5 L of blood volume (intravascular compartment) and a plasma volume of ≈3.0 L when the hematocrit is 40%. Although fluid from other clinically relevant ECF compartments (e.g., cerebrospinal fluid [CSF], urine) may be analyzed in the clinical laboratory, most laboratory tests used to determine hydration, electrolyte, and acid-base status are performed on samples from the intravascular compartment.
The minimum daily requirement for water can be estimated from renal (1200 to 1500 mL in urine) and “insensible” losses (≈400 to 700 mL) as a result of evaporation from the skin and respiratory tract. Activity, environmental conditions, and disease all have dramatic effects on daily water (and electrolyte) requirements. On average, an adult must take in ≈1.5 to 2.0 L of water daily to maintain fluid balance. Because primary regulatory mechanisms are designed to primarily maintain intracellular hydration status, imbalances in TBW are initially reflected in the ECF compartment. Table 50.1 lists common causes and clinical manifestations of expansion and contraction of the ECF compartment.
Clinical Manifestations | Causes | |
---|---|---|
ECF loss | Thirst, anorexia, nausea, lightheadedness, orthostatic hypotension, syncope, tachycardia, oliguria, decreased skin turgor and “sunken eyes,” shock, coma, death | Trauma (and other causes of acute blood loss), “third-spacing” of fluid (e.g., burns, pancreatitis, peritonitis), vomiting, diarrhea, diuretics, renal or adrenal (i.e., sodium wasting) disease |
ECF gain | Weight gain, edema, dyspnea (secondary to pulmonary edema), tachycardia, jugular venous distention, portal hypertension (ascites), esophageal varices | Heart failure, cirrhosis, nephrotic syndrome, iatrogenic (intravenous fluid overload) |
The primary cationic (positively charged) electrolytes are sodium (Na + ), potassium (K + ), calcium (Ca 2+ ), and magnesium (Mg 2+ ), whereas the anions (negatively charged) include chloride (Cl − ), bicarbonate (HCO 3 − ), phosphate (HPO 4 2− , H 2 PO 4 − ), sulfate (SO 4 2− ), organic ions such as lactate, and negatively charged proteins. Electrolyte concentrations of the body fluid compartments are shown in Table 50.2 . Na + , K + , Cl − , and HCO 3 − in the plasma or serum are commonly analyzed in an electrolyte profile because their concentrations provide the most relevant information about the osmotic, hydration, and acid-base status of the body. Although hydrogen (H + ) is a cation, its concentration is approximately 1 million–fold lower in plasma than the major electrolytes listed in Table 50.2 (10 −9 versus 10 −3 mol/L) and is negligible in terms of osmotic activity.
Component | Plasma | Interstitial Fluid | Intracellular Fluid a |
---|---|---|---|
Volume, H 2 O (TBW = 42 L) | 3.5 L | 10.5 L | 28 L |
Na + | 140 | 145 | 12 |
K + | 4 | 4 | 156 |
Ca 2+ | 2.4 | 2–3 | 0.3 |
Mg 2+ | 1 | 0.5–1 | 13 |
Trace elements | 1 | — | — |
Cl − | 103 | 114 | 4 |
HCO 3 − | 27 | 31 | 12 |
Protein − | 16 | — | 55 |
Organic acids − | 5 | — | — |
HPO 4 2− | 1 | — | — |
SO 4 2− | 0.5 | — | — |
Any increase in the concentration of one anion is accompanied by a corresponding decrease in other anions or by an increase in one or more cations or both because total electrical neutrality must be maintained. Similarly, any decrease in the concentration of anions involves a corresponding increase in other anions, a decrease in cations, or both. In the case of polyvalent ions (e.g., Ca 2+ , Mg 2+ ), it is important to distinguish between the substance concentration of the ion itself and the concentration of the ion charge. Thus although the concentration of total calcium ions in normal plasma is ≈2.5 mmol/L, the concentration of the total calcium ion charge is 5.0 mmol/L (also called 5 milliequivalents per liter [mEq/L]).
The extracellular compartment is composed of plasma and interstitial fluid.
Plasma generally has a volume of 1300 to 1800 mL/m 2 of body surface and constitutes approximately 5% of the body volume (≈3.5 L for a 66-kg subject). Total body volume is derived from body mass by using an estimated body density of 1.06 kg/L. Table 50.2 describes the electrolyte composition of plasma. The mass concentration of water in normal plasma is approximately 0.933 kg/L, depending on the protein and lipid content (see “Electrolyte Exclusion Effect” in Chapter 37 ). Thus a concentration of sodium in the plasma of 140 mmol/L would correspond to a molality of sodium in plasma water of 150 mmol/kg H 2 O (140 mmol/L divided by 0.933 kg/L). The concentration of net protein ions in plasma is ≈12 mmol/L.
Interstitial fluid is essentially an ultrafiltrate of blood plasma (see Fig. 50.1 ). When all extracellular spaces except plasma are included, the volume accounts for about 26% (10.5 L) of the total body volume. Plasma is separated from the interstitial fluid by the endothelial lining of the capillaries, which acts as a semipermeable membrane and allows passage of water and diffusible solutes but not compounds of high molecular mass proteins. The exchange of water between the interstitial and intravascular compartments is governed by Starling forces, which demonstrates that the net movement of fluid across a capillary membrane is a function of membrane permeability and differences in hydrostatic and oncotic pressures on the two sides of the membrane. The “impermeability” to proteins is not absolute, and in some pathologic conditions causing shock, such as bacterial sepsis, the permeability of the vascular endothelium increases dramatically, resulting in leakage of albumin, a reduction in the effective circulating volume, and hypotension. If not aggressively treated with intravenous fluids and/or vasopressors, this condition can result in death as the result of decreased cerebral perfusion.
The exact composition of ICF is difficult to measure. Therefore data for ICF (see Table 50.2 ) are considered only approximations. The ICF constitutes ≈66% of the total body volume (see Fig. 50.1 ).
The composition of ICF can differ markedly from that of ECF because of separation of these compartments by the cell membrane. The composition differences are a consequence of both the Gibbs-Donnan equilibrium and active and passive transport of ions, as well as active transport of larger molecules.
Two solutions separated by a semipermeable membrane will establish an equilibrium, so that all ions are equally distributed in both compartments, provided the solutes can move freely through the membrane. At the state of equilibrium, the total ion concentration and therefore the total concentration of osmotically active particles are equal on both sides of the membrane.
If solutions on two sides of a membrane contain different concentrations of ions that cannot freely move through the membrane (e.g., proteins), distribution of diffusible ions (e.g., electrolytes) at the steady state will be unequal, but the sum of the concentrations of ions in one compartment is equal to the sum of ions in the other compartment ( Fig. 50.2 ). This is referred to as Gibbs-Donnan equilibrium. Importantly, the law of electrical neutrality must also be obeyed for both compartments. An example of the uneven distribution of an ion in two compartments with different protein content (nondiffusible ions) is the concentration of chloride ions in plasma and CSF. As a result of increased selectivity of the blood-brain barrier against proteins, Cl − ions are ≈15% higher in CSF to establish electrical and osmotic equilibrium. Cells, most notably those of the central nervous system (CNS), that contain nondiffusible protein anions can withstand only a limited and temporary difference in osmotic pressure across the cell membrane. Osmotic pressure is normally identical inside and outside the cells because the cell membrane can correct concentration differences by excluding some small ions through active, energy-requiring transport processes. If these processes cease, the cells will swell and eventually will burst (osmotic lysis).
Examination of Table 50.2 reveals that the electrolyte compositions of blood plasma and interstitial fluid are similar and differ markedly from that of ICF. The major ECF ions are Na + , Cl − , and HCO 3 − , but in ICF, the main ions are K + , Mg 2+ , organic phosphates, and protein. This unequal distribution of ions is due to active transport of Na + from inside to outside the cell against an electrochemical gradient. An active sodium pump deriving its energy from glycolysis-generated adenosine triphosphate (ATP) is present in most cell membranes and frequently is coupled with transport of K + into the cell.
In addition to the Na + /K + -ATPase, a ubiquitous Na + -H + exchanger (often referred to as an antiporter ) actively pumps H + out of the ICF in exchange for Na + . This exchanger is critical for maintaining intracellular pH homeostasis. At least six different isoforms of this transmembrane protein have been identified. Of particular importance is the role of this exchanger for acid-base regulation in renal tubular cells, as discussed later in this chapter.
Disorders of Na + , K + , Cl − , and HCO 3 − will now be separately considered, even though disorders of electrolyte and water homeostasis need a systematic evaluation rather than an individual review of each ion.
Disorders of Na + homeostasis can occur because of excessive loss, gain, or retention of Na + , or as the result of excessive loss, gain, or retention of H 2 O. It is difficult to separate disorders of Na + and H 2 O balance because of their close relationship in establishing normal osmolality in all body water compartments. As described in detail in Chapter 49 , the primary organ for regulating body water and extracellular Na + is the kidney. As a brief introduction to this section, it is important to remind the reader of the functions of healthy kidneys.
The human body is in a dynamic state of flux as fluids and electrolytes are constantly being gained through mechanisms such as thirst and hunger and lost through processes such as sweating and urination. Homeostasis within a narrow window is necessary for life, and the body must defend against excessive gains or losses. Although certain behavioral adaptations are undoubtedly important (e.g., drinking when thirsty to prevent water and volume loss) others may be more debatable (as in the case of dietary sodium restriction). The kidney is responsible for not only clearing uremic toxins from the circulation but also in maintaining fluid balance and defending electrolyte homeostasis across a wide range of these gains and losses. In the proximal tubules, 70 to 80% of filtered Na + is actively reabsorbed, with H 2 O and Cl − following passively to maintain electrical neutrality and osmotic equivalence. In the descending loop of Henle, H 2 O, but not electrolytes, is passively reabsorbed because of the high osmotic strength of interstitial fluid in the renal medulla. In the ascending loop of Henle, Cl − is reabsorbed actively, with Na + following. At the level of the distal tubule, the first of the two primary Na + /H 2 O regulating processes occurs. Here, aldosterone stimulates the cortical collecting ducts to reabsorb Na + (with water following passively) and secrete K + (and to a lesser extent, H + ) to maintain electrical neutrality. Aldosterone is produced by the adrenal cortex in response to angiotensin II derived by the action of renin. The secretion of renin by renal juxtaglomerular cells is stimulated by low chloride, β-adrenergic activity, and low arteriolar pressure. Thus when the kidneys are hypoperfused (as occurs when blood volume decreases, or when the renal arteries are obstructed), the distal tubules, under the influence of aldosterone, reclaim Na + .
Further water regulation in the kidney occurs from the distal tubule through the collecting duct, where tubular permeability to H 2 O is under the influence of vasopressin (also called antidiuretic hormone [ADH]) (see Chapters 49 and 55 ). Vasopressin is released by the posterior pituitary under the influence of baroreceptors in the aortic arch and hypothalamic chemoreceptors that are responsive to circulating osmolality, which is primarily a reflection of Na + concentration. When ECF volume is decreased, or when plasma osmolality is increased, vasopressin is secreted, tubular permeability to H 2 O increases via aquaporins, and H 2 O is reabsorbed in an attempt to restore blood volume or to decrease osmolality. In contrast, when ECF volume is increased or osmolality decreased, vasopressin secretion is inhibited, and more H 2 O is excreted in the urine (diuresis).
Besides the kidney, the body’s only other mechanism for restoring Na + /H 2 O homeostasis is ingestion of H 2 O. Thirst is stimulated by decreased blood volume or hyperosmolality. It is important to remember that baroreceptors that influence renal handling of Na + and H 2 O, and thirst, sense changes only in the intravascular blood volume and not the total ECF, whereas osmoreceptors in the brain, such as the organum vasculosum lamina terminalis (OVLT) neurons, sense the osmolality of the ECF surrounding the cells. Laboratory assessment of water and electrolyte disorders is made primarily from the blood volume (plasma); the clinician must assess the status of TBW and blood volume before interpreting laboratory values. The physical findings of these disorders are as important as the laboratory values in management of water and electrolyte disorders (see Table 50.1 ).
Hyponatremia is defined as a decreased plasma Na + concentration (generally <135 mmol/L) and is the most commonly encountered disorder of electrolytes, with incidences as high as 15 to 30% in acutely and chronically hospitalized patients. Hyponatremia typically manifests clinically as nausea, generalized weakness, and mental confusion at values less than 120 mmol/L and severe mental confusion plus seizures at less than 105 mmol/L. The rapidity of development of hyponatremia influences the Na + concentrations at which symptoms develop (i.e., clinically apparent symptoms may manifest at higher Na + concentrations [≈125 mmol/L] when hyponatremia develops rapidly). It is important to note that symptoms are due to changes in osmolality rather than to the Na + concentration per se. CNS symptoms are due to movement of H 2 O into cells to maintain osmotic balance and subsequent swelling of CNS cells. These symptoms can occur more rapidly in children, so there is a need to be particularly vigilant in the pediatric population.
Hyponatremia can be hypo-osmotic, hyperosmotic, or iso-osmotic. Measurement of plasma osmolality is an important initial step in the assessment of hyponatremia. Of these, the most common form is hypo-osmotic hyponatremia, and it is important to distinguish it from the other two forms (hyperosmotic or iso-osmotic) because these represent situations where hyponatremia does not need to be treated. Fig. 50.3 describes an algorithm for laboratory measurements and physical examination findings in the differential diagnosis of plasma Na + less than 135 mmol/L.
Typically, when plasma Na + concentration is low, calculated, or measured, osmolality will also be low. This type of hyponatremia can be due to excess loss of Na + (depletional hyponatremia) or increased ECF volume (dilutional hyponatremia). Differentiating these initially requires clinical assessment of TBW and ECF volume by history and physical examination.
Depletional hyponatremia results from a loss of Na + from the ECF space that exceeds the concomitant loss of water. Hypovolemia is apparent in the physical examination (orthostatic hypotension, tachycardia, decreased skin turgor). If urine Na + is low (<10 mmol/L), the kidneys are properly retaining filtered Na + and the loss is extrarenal, most commonly from the gastrointestinal tract or skin (see Fig. 50.3 ). Preventing ongoing loss and restoring ECF volume with isotonic fluid is sufficient to correct hyponatremia in these situations.
Alternatively, if urine Na + is increased in this setting (generally >20 mmol/L), renal loss of Na + is likely. Renal loss of Na + occurs with (1) osmotic diuresis, (2) use of diuretics (which inhibit reabsorption of Cl − and Na + in the ascending loop), (3) adrenal insufficiency (no aldosterone or cortisone prevents distal tubule reabsorption of Na + ), or (4) salt-wasting nephropathies, as can occur with interstitial nephritis and tubular recovery after acute tubular necrosis or obstructive nephropathy. Hypo-osmotic hyponatremia has also been attributed to cerebral salt wasting, a controversial diagnosis associated with subarachnoid hemorrhage (SAH) and other intracranial diseases/trauma. Despite being described in literature for ≈70 years, the condition remains controversial because the mechanism of the condition remains undefined. If it is a physiologic condition, it is exceedingly rare as evidenced in a publication detailing a series of 100 patients with SAH. Of this population of 100 patients, 49 developed hyponatremia and the cause of the hyponatremia was ascribed to syndrome of inappropriate secretion of antidiuretic hormone (SIADH) in 71.4% patients. Of the remaining hyponatremic patients, 10.2% were incorrectly treated with hypotonic saline (0.45% saline), 10.2% were hypovolemic, and the remaining 8.2% had acute cortisol deficiency.
Renal loss of Na + in excess of H 2 O can also occur in metabolic alkalosis from prolonged vomiting, because increased renal HCO 3 − excretion is accompanied by Na + ions. In this case, urine sodium is increased (>20 mmol/L), but urine chloride remains low. In proximal renal tubular acidosis (RTA) type 2, bicarbonate is lost because of a defect in HCO 3 − reabsorption, and Na + is co-excreted to maintain electrical neutrality. As with extrarenal Na + loss, management of hyponatremia attributable to renal Na + loss is centered on the reversal of underlying cause and restoration of ECF volume.
Dilutional hyponatremia is a result of excess H 2 O retention and often can be detected during the physical examination as edema. In advanced renal failure, water is retained because of decreased filtration and H 2 O excretion. When ECF is increased but the circulating blood volume is decreased, as occurs in hepatic cirrhosis, heart failure, and nephrotic syndrome, a vicious cycle is established. The decreased blood volume is sensed by baroreceptors and results in increased aldosterone and vasopressin, even though ECF volume is excessive. The kidneys reabsorb Na + and H 2 O in response to increased aldosterone and vasopressin in an attempt to restore the blood volume, resulting in further increases in ECF and further dilution of Na + . In dilutional hyponatremia, the low serum sodium concentrations reflect the severity of the underlying disease process. Management should be focused on the treatment of the underlying disease, as correction of Na + concentrations alone have no effect on overall morbidity or mortality.
In hypo-osmotic hyponatremia with a normal or euvolemic volume status, the most common causes are the syndrome of inappropriate ADH (vasopressin) (SIADH), primary polydipsia, and endocrine disorders such as adrenal insufficiency and hypothyroidism (see Fig. 50.3 ). Adrenal insufficiency causes hyponatremia through increased cortisol-releasing hormone, which stimulates vasopressin release, while hypothyroidism impairs free H 2 O excretion. SIADH describes hyponatremia attributable to “inappropriate” vasopressin release, as from a malignancy, which stimulates excessive H 2 O retention and increased urine osmolality. Free water restriction is the mainstay of therapy in SIADH. However, in severe or symptomatic hyponatremia from any cause, the use of hypertonic saline solutions may be required to correct serum Na + concentrations. In such cases, the hyponatremia must be corrected cautiously because too rapid correction can lead to brain demyelination (a condition known as osmotic demyelination syndrome). The pons is particularly sensitive to this, and rapid correction can lead to central pontine myelinolysis, a devastating condition characterized by dysarthria, dysphagia, weakness, and paralysis of the appendages, and, in the most serious cases, coma, paralysis of all voluntary muscles except those controlling the eye (locked-in syndrome), and death. Current recommendations are to increase Na + by 0.5 to 2.0 mmol/L per hour and not to exceed a total increase in Na + greater than 18 over 48 hours. For patients with severe symptoms, an easy-to-remember strategy called the “rule of sixes” is recommended (using the abbreviations six’s for symptoms): “six a day makes sense for safety; so six [mmol/L] in 6 hours for severe sx’s and stop.”
Finally, euvolemic hyponatremia also can be found in primary polydipsia when water intake is greater than the renal capacity to excrete excess H 2 O. This can be the result of psychiatric illness, but diseases that cause hypothalamic disorders, such as sarcoidosis, also may cause polydipsia by altering the thirst reflex (see Fig. 50.3 ).
Hyponatremia in the presence of increased quantities of other solutes in the ECF is the result of an extracellular shift of water or an intracellular shift of Na + to maintain osmotic balance between ECF and ICF compartments. The most common cause of this type of hyponatremia is severe hyperglycemia (see Fig. 50.3 ). As a general rule, Na + is decreased by ≈1.6 to 2.0 mmol/L for every 100-mg/dL (5.6-mmol/L) increase in glucose greater than 100 mg/dL (5.6 mmol/L). Correction of hyperglycemia alone will restore normal blood Na + . It also may occur when unmeasured solutes, such as mannitol, radiographic contrast agents, and glycine (surgical irrigant solutions), enter the intravascular fluid compartment. In these circumstances, plasma osmolality cannot be calculated accurately and it must be ascertained by direct measurement.
If the measured Na + concentration in plasma is decreased, but measured plasma osmolality, glucose, and urea are normal, the most likely explanation is pseudohyponatremia caused by the electrolyte exclusion effect (see Chapter 37 ). This occurs when Na + is measured by an indirect ion-selective electrode (ISE) in patients with severe hyperlipidemia or, less commonly, hyperproteinemia. Hyperlipidemia, manifested primarily as hypertriglyceridemia, although a more common cause of pseudohyponatremia, is typically detected by visual or spectrophotometric screening of samples prior to analysis. Hypercholesterolemia, which in contrast, is not reliably detected by visual or spectrophotometric screening, may produce pseudohyponatremia. The common culprit in hypercholesterolemia-induced pseudohyponatremia is lipoprotein X, an abnormal lipid particle arising in the setting of cholestasis. However, it is worth noting that high cholesterol concentrations are less likely to produce pseudohyponatremia, because the molecular mass of cholesterol is approximately 2.5 times lower than triglycerides and thus displaces a smaller amount of plasma water than triglycerides.
Hyperproteinemia, the other common cause of pseudohyponatremia, also cannot be detected by visual or spectrophotometric inspection. As shown in a recent study, only 10.9% of sodium test orders included an order for total protein, and the prevalence of pseudohyponatremia due to hyperproteinemia (>7.9 g/dL) at a large academic medical center was 5.3%. Of note, 36.6% of high total protein results in that study came from the hematology and oncology clinics, and many of the patients had restricted protein bands consistent with monoclonal disorders such as multiple myeloma or waldenstrom macroglobulinemia. Given that a high proportion of those patients with high total protein also had restricted peaks consistent with a plasma cell disorder, it is important to raise awareness of the potential for these patients to be at risk for pseudohyponatremia.
For laboratories serving a population with a high percentage of plasma cell disorders, the availability of a direct ISE method to help with the investigation of potential pseudohyponatremia cases is important because direct ISE methods are not subject to pseudohyponatremia.
Hypernatremia (defined as plasma Na + >145 mmol/L) is always hyperosmolar and is considerably less common than hyponatremia because a mild increase (1%) in serum osmolality increases thirst. However, hypernatremia occurs frequently in critically ill patients, where patients may be unable to drink water, and it is associated with very high mortality rates (40 to 60%) and prolonged length of intensive care unit (ICU) stay. Symptoms of hypernatremia are primarily neurologic (because of neuronal cell loss of H 2 O to the ECF) and include tremors, irritability, ataxia, confusion, and coma. , As with hyponatremia, the rapidity of development of hypernatremia will determine the plasma Na + concentration at which symptoms occur. Acute development may cause symptoms at 160 mmol/L, although in chronic hypernatremia, symptoms may not occur until Na + exceeds 175 mmol/L. In chronic hypernatremia, the intracellular osmolality of CNS cells will increase to protect against intracellular dehydration. Because of this, rapid correction of hypernatremia can cause dangerous cerebral edema because CNS cells will take up too much water if the ICF is hyperosmotic when normonatremia is achieved.
In many cases, the symptoms of hypernatremia may be masked by underlying conditions. Hypernatremia rarely occurs in an alert patient with a normal thirst response and access to water. Most cases are observed in patients with altered mental status or infants, both of whom may not be capable of rehydrating themselves.
Hypernatremia arises in the setting of (1) hypovolemia (excessive water loss or failure to replace normal water losses), (2) hypervolemia (a net Na + gain in excess of water gain), or (3) normovolemia. Again, assessment of TBW status by physical examination and measurement of urine Na + and osmolality are important initial steps in establishing a diagnosis ( Fig. 50.4 ).
Hypernatremia in the setting of decreased ECF is caused by renal or extrarenal loss of hypo-osmotic fluid, leading to dehydration. Thus once hypovolemia is established by physical examination, measurement of urine Na + and osmolality is used to determine the source of fluid loss. Patients who have large extrarenal losses will have concentrated urine (often >800 mOsmol/kg) with low urine Na + (<20 mmol/L), reflecting a proper renal response to conserve Na + and water to restore ECF volume. Extrarenal causes include diarrhea, skin losses (burns, fever, or excessive sweating), and respiratory losses coupled with failure to replace the water. When gastrointestinal loss is excluded, and the patient has normal mental status and access to H 2 O, a hypothalamic disorder (tumor or granuloma) inducing diabetes insipidus (DI) should be suspected.
In patients with poorly controlled diabetes with glucose values greater than 600 mg/dL (33.3 mmol/L), an osmotic diuresis can occur that results in extreme dehydration and hypernatremia. This condition is referred to as hyperosmolar hyperglycemic nonketotic syndrome and occurs most commonly in elderly individuals with type 2 diabetes.
Hypernatremia in the presence of normal ECF volume is often a prelude to hypovolemic hypernatremia. Insensible losses through the lung or skin must be suspected and are characterized by concentrated urine as the kidneys conserve water. Another cause of normovolemic hypernatremia is water diuresis, which is manifested by polyuria (see Fig. 50.4 ). The differential for polyuria (generally defined as greater than 3 L urine output/day) is a water or solute diuresis. Solute diuresis is exemplified by the osmotic diuresis of diabetes mellitus and generally is characterized by urine osmolality greater than 300 mOsmol/kg and hyponatremia (see previous discussion in this chapter). Water diuresis, a manifestation of DI, is characterized by dilute urine (osmolality <250 mOsmol/kg) and hypernatremia. DI can be central or nephrogenic. Central DI is due to decreased or absent vasopressin secretion resulting from head trauma, hypophysectomy, pituitary tumor, or granulomatous disease. Nephrogenic DI is due to renal resistance to vasopressin as a result of drugs (e.g., lithium, demeclocycline, amphotericin, propoxyphene); electrolyte disorders (e.g., hypercalcemia, hypokalemia); sickle cell anemia or Sjögren syndrome, which affect collecting duct responsiveness to vasopressin; or, more rarely, mutant vasopressin receptors. When thirst and access to water are uncompromised, many patients with DI will remain normonatremic because their free water losses are offset by intake. Such patients display symptoms of only polyuria and polydipsia. However, overt hypernatremia can manifest with progression of underlying causes, impaired thirst, or restricted access to water. Administration of vasopressin can be used to treat central DI, although patients with nephrogenic DI may be resistant to it. Correction of underlying disorders or discontinuation of offending drugs may be required to normalize Na + concentrations in nephrogenic DI.
The presence of excess TBW and hypernatremia indicates a net gain of water and Na + , with Na + gain in excess of water (see Fig. 50.4 ). This rare condition is observed most commonly in hospitalized patients receiving hypertonic saline or sodium bicarbonate. It affects acute kidney injury (AKI) patients in the ICU at a high rate because these patients are often given large quantities of physiologic saline, leading to sodium and water retention (as evidenced by edema and substantial weight gain). Hypernatremia then develops during the recovery of their renal function due to loss of water in excess of sodium and potassium. This type of hypernatremia can be prevented by paying close attention to the water and sodium balance in patients with large urine or stool outputs.
Rarely, hypervolemic hypernatremia may also be the result of the intentional or accidental ingestion of large quantities of sodium rich fluids, otherwise known as salt poisoning. Ingestion of a concentrated salt (NaCl) solution may induce vomiting and had previously been used as an emetic. However, because a salt water solution may also produce life-threatening hyponatremia, the use of salt water as an emetic should be strongly discouraged.
The causes of salt poisoning also include inappropriately reconstituted oral rehydration solutions and infant formula, as well as the intentional ingestion of high-sodium solutions such as soy sauce, in suicide attempts.
In contrast to other causes of hypernatremia, in which a rapid correction of hypernatremia may produce osmotic demyelination, the rapid correction of acute salt poisoning with hypotonic solutions can prevent intracranial hemorrhage and neurologic sequelae.
The total body potassium of a 70-kg subject is ≈3.5 mol (40 to 59 mmol/kg), of which only 1.5 to 2% is present in the ECF. Nevertheless, plasma K + is often a good indicator of total K + stores. Disturbance of K + homeostasis has serious consequences. For example, a decrease in extracellular K + (hypokalemia) is characterized by muscle weakness, irritability, and paralysis. Plasma K + concentrations less than 3.0 mmol/L are often associated with marked neuromuscular symptoms and indicate a critical degree of intracellular depletion. At lower concentrations, tachycardia and cardiac conduction defects are apparent on electrocardiogram (ECG) (flattened T waves) and can lead to cardiac arrest.
High extracellular K + (hyperkalemia) concentrations may produce symptoms of mental confusion, weakness, tingling, flaccid paralysis of the extremities, and weakness of the respiratory muscles. Cardiac effects of hyperkalemia include bradycardia and conduction defects evident on the ECG as prolonged PR and QRS intervals and “peaked” T waves. Prolonged, severe hyperkalemia greater than 7.0 mmol/L can lead to peripheral vascular collapse and cardiac arrest. Symptoms or ECG abnormalities are almost always present at K + concentrations greater than 6.5 mmol/L. Concentrations greater than 10.0 mmol/L in most cases are fatal, although fatalities can occur at significantly lower values.
Causes of hypokalemia (plasma K + <3.5 mmol/L) are classified as redistribution of extracellular K + into ICF, or true K + deficits, caused by decreased intake or loss of potassium-rich body fluids ( Fig. 50.5 ).
Intracellular redistribution of K + is illustrated by the fall in plasma K + that occurs after insulin therapy for diabetic hyperglycemia. Insulin plays a crucial role in maintaining the intracellular distribution of K + through active cellular transport and glucose control. In alkalosis, redistribution hypokalemia occurs when K + moves from ECF into cells as H + ions are pumped out by the Na + -H + antiporter. The resulting increase in intracellular Na + concentration from the action of the Na + -H + antiporter increases the activity of the Na + /K + -ATPase, resulting in a decrease in ECF K + . In addition, renal conservation of H + in the distal tubule occurs at the expense of K + . Hypokalemia is not an uncommon condition in in patients with cancer, either due to effects of the tumor itself on adrenal or renal tissues or from side effects of the chemotherapeutic medications. However, it is important in this group to be sure that the hypokalemia is true hypokalemia and not due to pseudohypokalemia.
The risk of pseudohypokalemia is higher in patients with hematologic malignancies associated with acute leukemia. Pseudohypokalemia can arise when blood samples from patients with very high white blood cell counts are allowed to stand at room temperature prior to processing and analysis. Pseudohypokalemia arises in this setting due to a time-dependent redistribution of K + from the plasma fraction into leukemic cells after the blood sample is collected. In addition, use of myelopoietic growth factors after chemotherapy can lead to rapid K + uptake by new cells. In these settings, it is important to process the samples as quickly as possible. Other causes of intracellular redistribution are listed in Fig. 50.5 . Clinically, redistributive hypokalemia is generally a transient phenomenon that is reversed once underlying conditions are corrected. Therefore careful monitoring during treatment of these patients is essential to avoid overcorrection (termed “rebound hyperkalemia”), especially when considering that supplemental potassium is a common cause of hyperkalemia in hospitalized patients.
Hypokalemia reflecting true total body deficits of K + because of potassium loss can be classified into renal and nonrenal losses, based on daily excretion of K + in the urine (see Fig. 50.5 ). If urine excretion of K + is less than 30 mmol/d, it can be concluded that the kidneys are functioning properly and are attempting to reabsorb K + . The cause may be decreased K + intake or extrarenal loss of K + -rich fluid. Causes of decreased intake include chronic starvation and postoperative intravenous fluid therapy with K + -poor solutions. Gastrointestinal loss of K + occurs most commonly with diarrhea and loss of gastric fluid through vomiting.
Urine excretion exceeding 25 to 30 mmol/day in a hypokalemic setting is inappropriate and indicates that the kidneys are the primary source of K + loss. Renal losses of K + may occur during the diuretic (recovery) phase of acute tubular necrosis and during states of excess mineralocorticoid (primary or secondary aldosteronism) or glucocorticoid (Cushing’s syndrome) production when the distal tubules increase Na + reabsorption and K + excretion. Renal loss of K + is also caused by thiazide and loop diuretics. In addition to redistribution of K + into cells in an alkalotic setting, K + can be lost from the kidneys in exchange for reclaimed H + ions. This cause of true hypokalemia will be evident in low urine Cl − and an alkaline urine. In patients with cancer, increased renal K + loss may be due to chemotherapy (e.g., cisplatin)-induced nephron and tubular damage. Magnesium deficiency also can lead to increased renal loss of K + , which is attributable to a reduction in the inhibitory effect of magnesium on luminal potassium channels.
True potassium deficit requires replacement of potassium. Although there are dietary sources of potassium, such as potatoes and tomatoes, significant K + losses may require oral or intravenous supplementation with potassium chloride. The oral route is generally preferred, although intravenous correction should be pursued in patients with severe or symptomatic hypokalemia and those who are unable to take oral medication. In individuals with ongoing sources of potassium losses, such as patients on diuretics, chronic supplementation with a daily regimen of oral potassium chloride is often used.
Hyperkalemia (commonly listed as a plasma K + >5.0 mmol/L in adults) is a result of (singly or in combination) (1) redistribution, (2) increased intake, or (3) increased retention. In addition, preanalytical conditions—such as hemolysis, thrombocytosis (>500 × 10 9 /L, when serum rather than plasma potassium is measured), and leukocytosis (>50 × 10 9 /L together with delayed sample analysis)—have been known to cause marked pseudohyperkalemia, as described in detail in Chapter 37 ( Fig. 50.6 ).
The transfer of intracellular K + into ECF invariably occurs in acidemia as K + shifts outward as the result of pH-induced changes in Na + /K + -ATPase activity. In general, K + concentrations can be expected to rise 0.2 to 0.5 mmol/L for every 0.1-unit drop in pH. When acidemia is corrected, normokalemia will be restored rapidly. Extracellular redistribution of K + also may occur in (1) tissue hypoxia; (2) insulin deficiency (e.g., diabetic ketoacidosis); (3) massive intravascular hemolysis; (4) severe burns; (5) violent muscular activity, as in status epilepticus; (6) rhabdomyolysis; and (7) tumor lysis syndrome. Finally, important iatrogenic causes of redistribution hyperkalemia include digoxin toxicity and β-adrenergic blockade, especially in patients with diabetes or on dialysis. Redistributive hyperkalemia can be corrected by reversing the aberrations that cause K + to shift out of cells. Insulin and sodium bicarbonate are commonly used and have a quick onset of action, particularly in the diabetic or acidemic setting. Drug-induced causes require cessation or dose reduction of the offending agent. Patients with digoxin toxicity should be given antibodies to digoxin as well, because of the high risk for mortality associated with hyperkalemia and supratherapeutic administration of digoxin.
When glomerular filtration rate (GFR) or renal tubular function is decreased, hyperkalemia will often occur. In the absence of severe renal failure, hyperkalemia is seldom prolonged and may not even occur in some cases. Decreased excretion of K + in moderate and acute renal disease and end-stage renal failure (with oliguria or anuria) are the most common causes of prolonged hyperkalemia (see Fig. 50.6 ). Hyperkalemia occurs along with Na + depletion in adrenocortical insufficiency (e.g., Addison disease) because diminished Na + reabsorption results in decreased tubular K + secretion. Drugs that block the production of aldosterone, such as inhibitors of angiotensin-converting enzyme (ACE inhibitors; e.g., lisinopril), nonsteroidal antiinflammatory drugs, and angiotensin II–receptor blockers, may also cause hyperkalemia. Excess administration of potassium-sparing diuretics that block distal tubular K + secretion (e.g., triamterene, spironolactone) may also cause hyperkalemia. In patients with cancer, hyperkalemia can be caused by adrenal insufficiency secondary to metastases to the adrenal glands, nephrotoxic chemotherapy agents (e.g., mitomycin-C, methotrexate, platinum compounds), postrenal obstruction, or tumor lysis syndrome. Treatment of hyperkalemia includes agents that increase cellular uptake of K + , such as glucose given with insulin, sodium bicarbonate, and β 2 -adrenergic agonists. The rapid onset of these agents provides a quick reduction in ECF potassium concentrations, thus reducing the risk for immediate life-threatening cardiac effects of hyperkalemia.
In the setting of hyperkalemia, calcium salts are also frequently administered to counteract the depolarizing effects of high extracellular K + . High K + concentration increases the resting membrane potential of the myocyte from approximately −90 to −80 mV, which is close to the depolarization threshold of −75 mV. This results in a greater likelihood of myocyte depolarization and arrhythmia. Infusion of calcium, in the form of CaCl 2 or calcium gluconate, rapidly increases extracellular Ca 2+ concentrations, which raise the depolarization threshold to approximately −65 mV. Raising the depolarization threshold to −65 mV re-establishes the interval between the normal resting potential and normal depolarization threshold, in effect decreasing myocyte excitability.
However, infusion of calcium does not contribute to the redistribution of extracellular potassium and should be combined with other treatment modalities. It is also important to note that treatments that increase intracellular redistribution of potassium are only temporizing measures when there is a true excess of potassium, and they need to be coupled with interventions that remove potassium from the circulation. To reduce the total body content of potassium, patients can be given K + -losing diuretics, cation-exchange resins, and, finally, hemodialysis. Stimulation of renal potassium excretion is preferred because the use of cation-exchange resins can be associated with bowel necrosis, particularly when given per rectum. Hemodialysis is an option of last resort, removing potassium through an extracorporeal circuit, which stimulates diffusion of potassium out of the circulating blood and into the discarded dialysate.
In the absence of acid-base disturbances, Cl − concentrations in plasma generally will follow those of Na + . However, determination of plasma Cl − concentration is useful in the differential diagnosis of acid-base disturbances and is essential for calculating the anion gap. Fluctuations in serum or plasma Cl − were believed to have little clinical consequence and serving only as signs of an underlying disturbance in fluid or acid-base homeostasis. The specific replacement of chloride is rarely targeted at chloride deficit independently, but it is a cornerstone of management for metabolic alkalosis. This notion has been challenged in recent studies linking lower chloride levels with reduced loop diuretic response. In addition, oral supplementation of sodium-free chloride in patients receiving high doses of loop diuretics saw increases in serum chloride levels and changes in cardiorenal parameters.
In general, causes of hypochloremia (generally defined as Cl − <98 mmol/L) parallel causes of hyponatremia. Persistent gastric secretion and prolonged vomiting result in significant loss of Cl − and ultimately in hypochloremic alkalosis and depletion of total body Cl − with retention of HCO 3 − . Respiratory acidosis, which is accompanied by increased HCO 3 − , is another common cause of decreased Cl − with normal Na + .
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