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What Is The Normal Level Of Potassium In Human Body

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Potassium (K), a chemical element in Group 1 (Ia) of the periodic table, the alkali metal group, essential to both plant and animal life. Potassium was the first metal to be isolated by electrolysis, by the English chemist Sir Humphry Davy, when he obtained the element (1807) by decomposing molten potassium hydroxide (KOH) with a voltaic battery.

Potassium metal is soft and white with a silvery luster, has a low melting point and is a good conductor of heat and electricity. Potassium gives a lavender color to the flame and its vapor is green. It is the seventh most abundant element in the Earth’s crust, making up 2.6 percent of its mass.

The potassium content of the Dead Sea is estimated at about 1.7 percent potassium chloride, and many other salty bodies of water are rich in potassium. Liquid waste from some salt pans can contain up to 40 grams per liter of potassium chloride and is used as a source of potassium.

Most potassium is found in igneous rocks, shale, and sediments in minerals such as muscovite and orthoclonic feldspar that are insoluble in water. This makes it difficult to obtain potassium. As a result, most commercial potassium compounds (often called loose potash) are obtained by electrolysis from soluble potassium compounds, such as carnallite (KMgCl

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Potash is produced by sodium reduction of molten potassium chloride, KCl, at 870 °C (1,600 °F). Molten KCl is continuously fed to a packed distillation column while sodium vapor is passed through the column. By condensing the more volatile potassium at the top of the distillation tower, the reaction Na + KCl → K + NaCl is pushed to the right. Attempts to devise a scheme for the commercial electrolytic production of potassium have been unsuccessful because there are few salt additives that can lower the melting point of potassium chloride at temperatures where electrolysis is effective.

There is little commercial demand for potassium metal itself, and most of it is converted by direct combustion in dry air to potassium peroxide, KO

, which is used in breathing equipment because it releases oxygen and removes carbon dioxide and water vapor. (Potassium peroxide is a yellow solid composed of K

Of ions. It can also be formed by oxidizing potassium amalgam with dry air or oxygen.) The metal is also used as an alloy with sodium as a liquid metal heat transfer medium. Potassium reacts very strongly with water, releasing hydrogen (which ignites) and forming a solution of potassium hydroxide, KOH.

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Sodium-potassium alloy (NaK) is used to a limited extent as a heat transfer coolant in some nuclear fast breeder reactors and experimentally in gas turbine power plants. The alloy is also used as a catalyst or reducing agent in organic synthesis.

In addition to potassium alloys with lithium and sodium, alloys with other alkali metals are also known. There is complete miscibility in the potassium-rubidium and potassium-cesium binary systems. The latter system forms an alloy that melts at about −38 °C (−36 °F). Modification of the system by the addition of sodium leads to a ternary eutectic melting at about −78 °C (−108 °F). The composition of this alloy is 3 percent sodium, 24 percent potassium, and 73 percent cesium. Potassium is virtually immiscible with all the alkaline earth metals, as well as zinc, aluminum and cadmium.

) is required by all plants and animals. Plants need it for photosynthesis, regulation of osmosis and growth, and activation of enzymes. Every animal has a closely maintained potassium level and a relatively constant potassium-to-sodium ratio. Potassium is the major inorganic cation inside the living cell and sodium is the most abundant cation in the extracellular fluid. In higher animals, selective complexes for Na

Act on cell membranes to provide ‘active transport’. This active transport transmits electrochemical impulses to nerve and muscle fibers and balances the activity of nutrient uptake and waste removal from cells. Too little or too much potassium in the body is fatal. However, potassium in the soil ensures the presence of this essential element in food.

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The potassium content of plants varies considerably, although it is usually between 0.5-2 percent of the dry weight. In humans the ratio of potassium between cells and plasma is about 27:1. The potassium content of muscle tissue is about 0.3 percent, while that of blood serum is about 0.01-0.02 percent. The dietary requirement for normal growth is about 3.3 grams (0.12 oz) of potassium per day, but ingestion of more than 20 grams of potassium results in distinct physiological effects. Excess potassium is excreted in the urine and a significant amount can be lost through sweating.

Natural potassium consists of three isotopes: potassium-39 (93.26 percent), potassium-41 (6.73 percent), and radioactive potassium-40 (about 0.01 percent). several artificial isotopes have also been prepared. Potassium-39 is typically about 13.5 times more abundant than potassium-41. The natural radioactivity of potassium is due to beta radiation from the isotope potassium-40 (10

Electron, so it normally has an oxidation state of +1 in its compounds, although compounds containing the anion, KE every year at our phlebotomy conference, I present a talk called “Phlebotomy Top Gun.” The format for ‘Phlebotomy Top Gun’ is a case-based presentation. I am asking conference attendees for case ideas based on issues or questions you have about phlebotomy. I present them as case-based scenarios, and using an audience response voting mechanism, conference participants vote on the action or response they feel is appropriate for each case. I then present the evidence and data from the literature and Mayo’s collective experience related to the topic.

At the end of the case, the attendees vote again. Just in case, I can see if I was able to change someone’s mind on the issue at hand by presenting the facts and information relevant to the issue. This is a real-life case from a presentation at last year’s Phlebotomy Top Gun conference, which arose from a question about the validity of measuring potassium from capillary blood samples.

Phlebotomy Top Gun: Measuring Potassium In Capillary Blood Samples

Based on a question posed by a phlebotomy conference attendee two years ago, I presented this question to the conference audience. Regarding capillary versus venous potassium (K) measurement, which of the following statements are true:

At the conference, we would use a live audience feedback system to poll the audience and see what answers audience members think were correct on this issue. For those of you watching now, what do you think is the correct answer?

What I do next with each case in the “Phlebotomy Top Gun” presentation is go through data and evidence, either internal or external to the Mayo Clinic, that I can find about the question. At the end of each case, I poll the audience again to see if anyone’s opinion has changed.

To remind our audience today, capillary “blood” is really a mixture of arterial blood, venous blood, interstitial fluid (the fluid that bathes the cells in our tissues), and fluid released from the cells during the capillary puncture itself. This combination of interstitial fluid and cellular fluid is often called “tissue fluid.” While the concentrations of most chemical analytes are identical or very similar between arterial and venous blood, tissue fluid can vary dramatically in the concentration of the various analytes we measure in the laboratory. To make matters more complicated, each capillary puncture will have a different amount of fluid tissue collected in the sample.

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The significance of this variable amount of tissue fluid collected in a capillary sample varies by analyte and depends on how different cellular and interstitial concentrations of the measured analyte are compared to venous or arterial blood. For example, there is no hemoglobin in the interstitial fluid, so variable amounts of interstitial fluid will cause variability in the capillary hemoglobin measurement compared to venous hemoglobin or plasma hemoglobin. After meals, interstitial fluid glucose concentration changes more slowly than venous or arterial glucose, and this complicates the interpretation of capillary glucose in the nonfasting state. So what about capillary sampling to measure potassium? Let’s explore this question further, remembering that we break more cells during capillary puncture than during venipuncture.

In this slide, I provide a reference to an earlier study comparing potassium values ​​from infants with simultaneous blood collection from an indwelling arterial catheter versus a heel stick capillary puncture. Capillary samples yielded potassium readings that were an average of 1.2 milligrams higher than the paired arterial serum sample, consistent with the results of several other studies showing that capillary potassium readings were higher than values ​​obtained from intravenous or

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