Electrolyte or electrolyte. It is any substance that contains free ions , which behave as an electrical conducting medium . Because they generally consist of ions in solution, electrolytes are also known as ionic solutions, but molten electrolytes and solid electrolytes are also possible .
Summary
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- 1 story
- 2 Physiological importance
- 3 Affectations
- 1 Measurement
- 4 uses
- 1 Sports drinks
- 2 Electrochemistry
- 5 dry electrolyte
- 6 sources
History
Electrolytes commonly exist as solutions of acids , bases , or salts . Furthermore, some gases can behave as electrolytes under conditions of high temperature or low pressure. Electrolyte solutions can result from the dissolution of some biological (eg DNA , polypeptides ) or synthetic (eg polystyrenesulfonate , in which case they are called polyelectrolyte ) polymers , and contain multiple charged centers. Electrolyte solutions are normally formed when a salt is placed in a solvent such aswater , and the individual components dissociate due to interactions between the solvent and solute molecules , in a process called solvation . For example, when common salt , NaCl , is placed in water, the following reaction occurs:
NaCl(s) → Na + + Cl −
It is also possible for substances to react with water when added to it, producing ions. For example, carbon dioxide reacts with water to produce a solution containing hydronium , bicarbonate , and carbonate ions .
In simple terms, the electrolyte is a material that dissolves completely or partially in water to produce a solution that conducts an electrical current.
Molten salts can also be electrolytes. For example, when sodium chloride melts, the liquid conducts electricity.
If an electrolyte in solution has a high proportion of the solute dissociating to form free ions, the electrolyte is said to be strong ; if most of the solute does not dissociate, the electrolyte is weak . The properties of electrolytes can be exploited by using electrolysis to extract the constituent chemical elements .
physiological importance
In physiology , the primary ions of electrolytes are sodium (Na + ), potassium (K + ), calcium (Ca 2+ ), magnesium (Mg 2+ ), chloride (Cl − ), hydrogen phosphate (HPO 4 2− ) and bicarbonate (HCO 3 − ).
All higher life forms require a subtle and complex balance of electrolytes between the intracellular and extracellular milieu . In particular, the maintenance of a precise osmotic gradient of electrolytes is important. Such gradients affect and regulate body hydration , blood pH , and are critical for nerve and muscle function . There are several mechanisms in living species to keep the concentrations of the different electrolytes under tight control.
Both muscle tissue and neurons are considered electrical tissues of the body. Muscles and neurons are activated by the activity of electrolytes between the extracellular fluid or interstitial fluid and the intracellular fluid . Electrolytes can enter or leave through the cell membrane by means of specialized membrane-incorporated protein structures called ion channels . For example, muscle contractions depend on the presence of calcium (Ca 2+ ), sodium (Na + ), and potassium (K +). Without sufficient levels of these key electrolytes, muscle weakness or severe muscle contractions can occur.
Electrolyte balance is maintained orally or, in emergencies, by intravenous (IV) administration of electrolyte-containing substances, and is regulated by hormones , usually with the kidneys removing excess levels. In humans, electrolyte homeostasis is regulated by hormones such as antidiuretic hormone , aldosterone , and parathormone . Serious electrolyte imbalances , such as dehydration and overhydration , can lead to cardiac and neurological complications and, unless promptly resolved, can result in death.medical emergency .
Affectations
Electrolytes affect the amount of water in the body, the acidity of the blood (pH), muscle activity, and other important processes. You lose electrolytes when you sweat, and you must replenish them by drinking fluids. Common electrolytes include:
- Calcium
- Chloride
- Magnesium
- Match
- Potassium
- Sodium
Electrolytes can be acids, bases, and salts.
Measurement
Measurement of electrolytes is a commonly performed diagnostic procedure, performed via selective electrode blood examination or urinalysis by medical technologists . Interpretation of these values is somewhat meaningless without clinical history and is often impossible without parallel measurement of renal function . The most frequently measured electrolytes are sodium and potassium. Chloride levels are rarely measured except for arterial blood gas interpretation since they are inherently linked to sodium levels. An important test carried out with urine is the urine test.specific gravity to determine the existence of electrolyte imbalance .
Each electrolyte can be ordered as a separate test, such as:
- ionized calcium
- Serum calcium
- serum chloride
- Serum magnesium
- Serum phosphorus
- Serum potassium
- serum sodium
Applications
Sport drinks
Electrolytes are often found in sports drinks . In oral rehydration therapy , electrolyte drinks containing sodium and potassium salts restore the body’s water and electrolyte levels after dehydration caused by exercise, diaphoresis , diarrhea , vomiting , intoxication , or starvation .
Because sports drinks typically contain very high levels of sugar , they are not recommended for regular use by children. Water is considered the only essential drink for children during exercise. Medicated rehydration sachets and drinks are available to replace key electrolytes lost during diarrhea and other gastrointestinal problems. Dentists recommend that regular sports drink consumers take precautions against tooth decay .
Sports and electro drinks can be made at home, using the correct proportions of sugar, salt and water.
Electrochemistry
When an electrode is placed in an electrolyte and a voltage is applied , the electrolyte will conduct electricity. Electrons alone cannot normally pass through the electrolyte; instead, one chemical reaction occurs at the cathode , consuming the cathode’s electrons, and another reaction occurs at the anode , producing electrons to be captured by the anode. As a result, a cloud of negative charge develops in the electrolyte around the cathode, and a positive charge develops around the anode. Ions in the electrolyte move to neutralize these charges so reactions can continue and electrons can keep flowing. For example, in an ordinary salt solution (sodium chloride , NaCl) in water, the reaction at the cathode will be:
2H 2 O + 2e − → 2OH − + H 2
whereupon hydrogen gas will bubble ; the reaction at the anode is:
2H 2 O → O 2 + 4H + + 4e −
thereby releasing oxygen gas . The positively charged Na + sodium ions will react towards the cathode, neutralizing the negative charge of the OH − present there, and the Cl − chloride ions will react towards the anode neutralizing the positive charge of the H + there. Without the ions from the electrolyte, the charges around the electrodes would slow the continued flow of electrons; the diffusion of H + and OH −through the water to the other electrode would take longer than the movement of the more prevalent sodium ions. In other systems, the electrode reactions may involve the electrode metals as well as the electrolyte ions. Electrolytic conductors can be used in electronic devices where the chemical reaction at the metal/electrolyte interface produces useful effects.
dry electrolyte
Dry electrolytes are: essentially gels in a flexible crystalline molecular structure.
