Buffer Systems in the Body

Buffer Systems in the Body Understanding Buffer Systems in the Body The body of an adult human consists approximately 60% water. Water within the body is divided into that which is contained within cellular walls and that which is located outside of the cellular walls. Water located inside of the cellular walls is referred to as intercellular fluid (ICF) and extracellular fluid (ECF). It is vital that this fluid maintain the proper pH in order to function properly.

The body has a buffer system designed to make certain that the pH remains in the appropriate range for proper cellular function. This research will explore the buffer systems and their role in maintaining proper body pH. The normal pH of body fluids ranges from 7.35-7.45. When the pH lies outside of this range it can produce a condition of either acidosis or alkalosis, depending on the direction of the change. A pH below 6.8 or above 7.8 is fatal.

Carbonic acid is the most important factor influencing the pH of the ECF. CO2 reacts with water to form carbonic acid. This process releases hydrogen ions. Whether the solution is an acid or a base depends on the number of hydrogen ions. Buffers are dissolved compounds that can provide or remove hydrogen ions in order to stabilize a solution. Buffers within the body are typically weak acids or weak bases. There are three major buffer systems within the body. There are protein buffer systems in both the ECF and ICF.

The carbonic acid-bicarbonate system is the most important in the ECG. The phosphate buffer system is the most important buffer system in the ICF. In the protein buffer system, amino acids respond to changes in hydrogen ion concentrations. Blood plasma proteins and hemoglobin in red blood cells help to prevent drastic changes in pH. The carbonic acid-bicarbonate system helps to prevent pH changed due to organic acids in the ECF. The Phosphate buffer system is important in preventing pH changes in the intracellular fluid.

Changes in pH When changes occur to shift the balance of acid-base systems to a range that is out of the norm it has an effect on several bodily systems. For instance, when changes occur in the respiratory tract, the system may be unable to eliminate all of the CO2 generated by the peripheral tissues. Metabolic acidosis occurs when the body produces an overabundance of metabolic acids, such as lactic acid or ketones.

This reaction is the result of kidney damage that impairs the ability of the kidneys to excrete ions. The opposite condition occurs when the pH becomes too alkaline. Metabolic alkalosis occurs when bicarbonate ion concentrations become elevated. Bicarbonate ions interact with hydrogen ion to form carbonic acid. Alkalosis is occurs when H+ ions are reduced drastically. Sodium Sodium is the most abundant cation in the ECF. It is one of the main components to maintaining proper water balance.

Sodium effects serum ocmosis, nerve impulse transmission, and regulation of the acid-base balance. Sodium is a component in numerous chemical reactions in many systems in the body. Sodium is regulated by dietary intake and the production of aldersterone. An excess of sodium, caused by water loss or sodium excess causes a state called hypermatremia. In this condition, plasma sodium levels exceed 145 mcg. There are a number of conditions that can cause excess sodium levels including excess salt intake, hypertonic solutions, excess aldersterone, diabetes insipidus, and water loss.

Hyponatremia occurs when sodium levels fall below 135 mcg. This can occur with loss of sodium or net water excess. This can be the result of kidney disease with salt wasting, adrenal insufficiency, GI losses, increased sweating, or the use of diuretics. Potassium Potassium is another important cation in the ECF. It regulates metabolic action necessary for glycogen deposits in liver and skeletal muscle. It also plays an important role in the transmission and conduction of nerve impulses.

It is essential for normal cardiac conduction and the contraction of skeletal and smooth muscles. It is regulated by dietary intake and renal excretion. The body conserves potassium poorly. Any condition that increases urine output will have the effect of decreasing serum potassium. An excess of potassium in the body is generally considered anything above 5.3 mcg in the blood plasma. Cardiac irregularity is the most common symptom, includign bradycardia and other cardiac irregularities. The primary cause of high potassium levels is renal failure.

However, this can stem from a number of sources including a bodily fluid volume deficiency, massive cell damage, excess K+ given to the patient, adrenal insufficiency, acidosis, and a rapid infusion of blood. Hypokalemia occurs when the blood plasma level of potassium is too low (below 3.5 mcg). This is the most common electrolyte imbalance. It effects cardiac conduction and function. Calcium Calcium is a cation that is stored in the bone, plasma and body cells. In plasma, it binds with albumin.

It is well-known that calcium is necessary for healthy teeth and bones. However, it is also necessary for blood clotting, hormone secretion, maintaining the integrity of cell membranes, cardiac conduction, transmission of nerve impulses and muscle contraction. Calcium levels in the body are regulated by bone resorption. Hypercalcemia occurs when calcium levels rise above 5 mcg in the plasma. One of the most common symptoms is cardiac arrhythmia. X-rays will show calcium loss in the bones when blood plasma levels are high.

This is frequently a symptom of and underlying disease with excess bone resorption and the release of calcium. It can be caused by hyperparathyroidism, malignant neoplastic disease, Paget's disease, osteoporosis, prolong immobilization, and acidosis. The most common symptoms presented are anorexia, nausea, vomiting, weakness, and kidney stones. Hypocalcemia occurs when calcium levels fall below 4.0 mcg. This is often seen in severe illness, after a rapid blood transfusion with citrate, hypoparathyroidism, Vitamin D deficiency, pancreatitis, and alkalosis.

Some of the most common symptoms are numbness and tingling, hyperactive reflexes, muscle cramps and pathological fracture. Chlorine Chloride, an ion of chlorine is one of the most important compounds that assists with oxygenation of the blood in the lungs. As bicarbonate diffuses into cells, chloride goes from hemoglobin to plasma, causing an anion shift. The lungs will adapt quickly to these changes and will attempt to correct the pH before biological buffers from the kidneys kick in.

Chloride levels that are out of norm typically indicate that the pH is out of balance. When sodium levels are high and bicarbonate levels are low, it typically indicates that a high level of chloride is present. Hypochloremia occurs when the pH rises above 7.45. This condition can lead to excessive vomiting. It can lead to metabolic alkalosis due to reabsorption of bicarbonate. Typically, abnormal chloride levels occur in conjunction with other electrolyte imbalances. Hydrogen Hydrogen and carbon dioxide levels provide stimulus for respirations.

The lungs alter their depth and rate according to hydrogen concentration. In metabolic acidosis, respiration increases as the body attempts to exhale excess carbon dioxide. In metabolic alkalosis, the lungs attempt to retain carbon dioxide by decreasing respirations. The carbonic acid-bicarbonate system is the first to respond to ECF changes. It reacts in seconds to regulate the acid-base balance. Increased.