What is potash and is it poisonous?

Answer 1

Potash is potassium carbonate.

It is commonly used as a fertilizer although it has other uses, such as in photographic chemistry.

It isn't poisonous per se (although like many substances, in excessive amounts it can cause harm), but it isn't intended as a food additive.

Answer 2

1

Answer 3

Potash is the common name for a compound called Potassium Carbonate (K2CO3). Since it is an ionic compound, it exsists more as these two ions floating around in solution than actually bound together. Potassium is an essential mineral needed by your body, which is why bananas are so good for you, and carbonates are found in many common foods such as baked goods, soda, etc.

The only harmful part about potash is not the main compound itself, but instead all the unknown impurities. A block of potash found on the ground in of itself is not hazardous, but who knows what that block may have been laying in.

Answer 4

Potash isn't poisonous at all. It was used for baking before people switched to baking soda and is still an ingredient in gingerbread.

Answer 5

I didn't see anything about it being poisonous but this is what I found:

See potassium carbonate.
See potassium hydroxide.
Any of several compounds containing potassium, especially soluble compounds such as potassium oxide, potassium chloride, and various potassium sulfates, used chiefly in fertilizers.
[Sing. of obsolete pot ashes, translation of obsolete Dutch potaschen (from the fact that this substance was originally obtained by leaching wood ashes and evaporating the leach in a pot).]

Name used for various inorganic compounds of potassium, chiefly the carbonate (K2CO3), a white crystalline material formerly obtained from wood ashes. They are used to make special types of glass, potassium silicate (a dehydrating agent), pigments, printing inks, and soft soaps; for washing raw wool; and as a lab reagent and general-purpose food additive. Potassium hydroxide is frequently called caustic potash, and in the fertilizer industry, potassium oxide is called potash.

Good luck I hope this helps,
Mrs. Fuzz

Answer 6

What Is Potash

Answer 7

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Answer 8

2

Answer 9

What Is Pot Ash

Answer 10

Potassium
From Wikipedia, the free encyclopedia
Jump to: navigation, search
19 argon ← potassium → calcium
Na
↑
K
↓
Rb
Periodic table - Extended periodic table
General
Name, symbol, number potassium, K, 19
Chemical series alkali metals
Group, period, block 1, 4, s
Appearance silvery white
Standard atomic weight 39.0983(1) g·mol−1
Electron configuration [Ar] 4s1
Electrons per shell 2, 8, 8, 1
Physical properties
Phase solid
Density (near r.t.) 0.89 g·cm−3
Liquid density at m.p. 0.828 g·cm−3
Melting point 336.53 K
(63.38 °C, 146.08 °F)
Boiling point 1032 K
(759 °C, 1398 °F)
Atomic properties
Crystal structure cubic body centered
Oxidation states 1
(strongly basic oxide)
Ionization energies
(more) 1st: 418.8 kJ·mol−1
2nd: 3052 kJ·mol−1
3rd: 4420 kJ·mol−1
Atomic radius 220 pm
Atomic radius (calc.) 243 pm
Covalent radius 196 pm
Van der Waals radius 275 pm
Miscellaneous
Magnetic ordering paramagnetic
Thermal conductivity (300 K) 102.5 W·m−1·K−1
Thermal expansion (25 °C) 83.3 µm·m−1·K−1
Speed of sound (thin rod) (20 °C) 2000 m/s
Young's modulus 3.53 GPa
Shear modulus 1.3 GPa
Bulk modulus 3.1 GPa
Mohs hardness 0.4
Brinell hardness 0.363 MPa
CAS registry number 7440-09-7
Selected isotopes
Main article: Isotopes of potassium iso NA half-life DM DE (MeV) DP
39K 93.26% K is stable with 20 neutrons
40K 0.012% 1.277×109 y β- 1.311 40Ca
ε 1.505 40Ar
β+ 1.505 40Ar
41K 6.73% K is stable with 22 neutrons
References
This box: view • talk • edit

Potassium (pronounced /pəˈtæsiəm/) is a chemical element. It has the symbol K (Arabic: al qalja → Latin: kalium) and atomic number 19. The name "potassium" comes from the word "potash", as potassium was first isolated from potash. Potassium is a soft silvery-white metallic alkali metal that occurs naturally bound to other elements in seawater and many minerals. It oxidizes rapidly in air and is very reactive, especially towards water. In many respects, potassium and sodium are chemically similar, although organisms in general, and animal cells in particular, treat them very differently.
Contents
[hide]

* 1 Notable characteristics
o 1.1 Physical
o 1.2 Biochemical
* 2 Applications
o 2.1 Agriculture and health
o 2.2 Industrial
* 3 History
* 4 Occurrence
* 5 Isotopes
* 6 Precautions
* 7 Potassium in nutrition and medicine
* 8 High potassium food
* 9 See also
* 10 Notes
* 11 References
* 12 External links

[edit] Notable characteristics

[edit] Physical
The flame test
The flame test

Potassium is the second least dense metal; only lithium is less dense. It is a soft, low-melting solid that can easily be cut with a knife. Freshly cut potassium is silvery in appearance, but in air it begins to tarnish toward grey immediately. Potassium must be protected from air for storage to prevent disintegration of the metal from oxide and hydroxide corrosion. Often samples are maintained under a reducing medium such as kerosene.

Like the other alkali metals, potassium reacts violently with water producing hydrogen. The reaction is notably more violent than that of lithium or sodium with water, and is sufficiently exothermic that the evolved hydrogen gas ignites.

2K(s) + 2H2O(l) → H2(g) + 2KOH(aq)

Because potassium reacts quickly with even traces of water, and its reaction products are nonvolatile, it is sometimes used alone, or as NaK (an alloy with sodium which is liquid at room temperature) to dry solvents prior to distillation. In this role, it serves as a potent desiccant

Potassium and its compounds emit a violet color in a flame. This fact is the basis of the flame test for the presence of potassium in a sample.

Potassium compounds generally have excellent water solubility, due to the high hydration energy of the K+ ion. The potassium ion is colorless in water.

Potassium concentration in solution is commonly determined by flame photometry, atomic absorption spectrophotometry, inductively coupled plasma, or ion selective electrodes. Methods of separating potassium by precipitation, sometimes used for gravimetric analysis, include the use of sodium tetraphenyl boron, dihydrogen hexachloroplatinate (IV) hexahydrate, and sodium cobaltinitrite.

[edit] Biochemical

Potassium is important in nerve function and in influencing osmotic balance between cells and the interstitiual fluid.[1]

Potassium may be detected by taste because it triggers three of the five types of tastebuds, according to concentration. Dilute solutions of potassium ion taste sweet (allowing moderate concentrations in milk and juices), while higher concentrations become increasingly bitter/alkaline, and finally also salty to the taste. The combined bitterness and saltiness of high potassium content solutions makes high-dose potassium supplementation by liquid drinks a palatability challenge.[citation needed]

[edit] Applications

[edit] Agriculture and health

* It is primarily used in fertilizers as either the chloride, sulfate or carbonate - not as the oxide.
* Potassium is an essential component needed in plant growth and is found in most soil types.
* In animal cells, potassium ions are vital to keeping cells alive (see Na-K pump)
* Potassium chloride is used as a substitute for table salt and is also used to stop the heart, e.g. in cardiac surgery and in executions by lethal injection in a solution.
* Potassium bisulfite (KHSO3) is used as a food preservative (but not in meats), bleaching of textiles and straw, wine and beer-making and in the tanning of leathers.
* Potassium bromate (KBrO3) is used as a flour improver (E924).
* Potassium sodium tartrate, or Rochelle salt (KNaC4H4O6) is used in baking powder and medicine.
* Potassium pyrophosphate (K4P2O7) is used in soaps and detergents.
* Potassium fluorosilicate (K2SiF6) is used as an insecticide.

[edit] Industrial

* Potassium hydroxide is an important industrial chemical used as a strong base.
* Potassium nitrate is used in gunpowder (black powder). An older term for KNO3 is saltpeter.
* Potassium carbonate, known as potash, is used in glass manufacturing.
* Glass treated with liquid potassium is much stronger than regular glass.
* Potassium vapor is used in several types of magnetometers.
* NaK (usually pronounced "nack"), an alloy of sodium and potassium which is liquid at room temperature, is used as a heat-transfer medium. It can also be used as a desiccant for producing dry and air-free solvents.
* The superoxide KO2 is used as a portable source of oxygen and as a carbon dioxide absorber. It is useful in portable respiration systems.
* Potassium bromide (KBr) is used in photographic film and in engraving.
* Potassium chromate (K2CrO4) is used in dyes and stains (bright yellowish-red colour), in explosives and fireworks, in safety matches, in the tanning of leather and in fly paper.
* Potassium fluorosilicate (K2SiF6) is used in specialized glasses, ceramics, and enamels.
* Potassium sodium tartrate, or Rochelle salt (KNaC4H4O6) is used in the silvering of mirrors.

Many potassium salts are very important, and include: potassium bromide, potassium carbonate, potassium chlorate, potassium chloride, potassium chromate, potassium cyanide, potassium dichromate, potassium iodide, potassium nitrate, potassium sulfate.

[edit] History

Potassium was discovered in London England by Sir Humphry Davy. In 1807 he derived it from caustic potash (KOH). Potassium was the first metal that was isolated by electrolysis.

Potassium was not known in Roman times, and its names are not Classical Latin but rather neo-Latin.

* The name kalium was taken from the word "alkali", which came from Arabic al qalīy = "the calcined ashes".
* The name potassium was made from the word "potash", which is English, and originally meant an alkali extracted in a pot from the ash of burnt wood or tree leaves.

[edit] Occurrence
Potassium in feldspar
Potassium in feldspar

Potassium makes up about 1.5% of the weight of the Earth's crust and is the seventh most abundant element. As it is very electropositive, potassium metal is difficult to obtain from its minerals. It is never found free in nature, as it reacts violently with water. Potassium salts such as carnallite, langbeinite, polyhalite, and sylvite are found in ancient lake and sea beds. These minerals form extensive deposits in these environments, making extracting potassium and its salts more economical. The principle source of potassium, potash, is mined in Saskatchewan, California, Germany, New Mexico, Utah, and in other places around the world. 3000 feet below the surface of Saskatchewan are large deposits of potash which are important sources of this element and its salts, with several large mines in operation since the 1960s. Saskatchewan pioneered the use of freezing of wet sands (the Blairmore formation) in order to drive mine shafts through them. See Potash Corporation of Saskatchewan. The oceans are another source of potassium, but the quantity present in a given volume of seawater is relatively low compared with sodium.


Potassium can be isolated through electrolysis of its hydroxide in a process that has changed little since Davy. Thermal methods also are employed in potassium production, using potassium chloride.

See also potassium minerals.

[edit] Isotopes

Main article: isotopes of potassium

There are 24 known isotopes of potassium. Three isotopes occur naturally: 39K (93.3%), 40K (0.0117%) and 41K (6.7%). Naturally occurring 40K decays to stable 40Ar (11.2%) by electron capture and by positron emission, and decays to stable 40Ca (88.8%) by beta decay; 40K has a half-life of 1.250×109 years. The decay of 40K to 40Ar enables a commonly used method for dating rocks. The conventional K-Ar dating method depends on the assumption that the rocks contained no argon at the time of formation and that all the subsequent radiogenic argon (i.e., 40Ar) was quantitatively retained. Minerals are dated by measurement of the concentration of potassium and the amount of radiogenic 40Ar that has accumulated. The minerals that are best suited for dating include biotite, muscovite, plutonic/high grade metamorphic hornblende, and volcanic feldspar; whole rock samples from volcanic flows and shallow instrusives can also be dated if they are unaltered.

Outside of dating, potassium isotopes have been used extensively as tracers in studies of weathering. They have also been used for nutrient cycling studies because potassium is a macronutrient required for life.

40K occurs in natural potassium (and thus in some commercial salt substitutes) in sufficient quantity that large bags of those substitutes can be used as a radioactive source for classroom demonstrations. In healthy animals and people, 40K represents the largest source of radioactivity, greater even than 14C. In a human body of 70 kg mass, about 4,400 nuclei of 40K decay per second.[2]

The activity of natural potassium is 31 Bq/g.

[edit] Precautions
Peroxides (Yellow) and Ozonides (Red) on surface of potassium metal.
Peroxides (Yellow) and Ozonides (Red) on surface of potassium metal.

Solid potassium reacts violently with water, and should therefore be kept under a mineral oil such as kerosene and handled with care. Unlike lithium and sodium, however, potassium cannot be stored under oil indefinitely. If stored longer than 6 months to a year, dangerous shock-sensitive peroxides can form on the metal and under the lid of the container, which can detonate upon opening. It is recommended that potassium, rubidium or caesium not be stored for longer than three months unless stored in an inert (oxygen free) atmosphere, or under vacuum.[3]

The extremely alkaline potassium hydroxide (KOH) residue on the surface of potassium which has been exposed to moisture, is a caustic hazard. As with sodium metal, the "soapy" feel of potassium metal on skin is due to caustic breakdown of the fats in skin into crude soft potassium soap, and represents the beginning of an alkali burn. Potassium should obviously be handled with care, with full skin and eye protection.

Potassium fires are exacerbated by water, and only a few dry chemicals are effective for them. Potassium has also been discovered to react violently with iodine.

[edit] Potassium in nutrition and medicine

Potassium is an essential mineral macronutrient in human nutrition; it is the major cation (positive ion) inside animal cells, and it is thus important in maintaining fluid and electrolyte balance in the body. Sodium makes up most of the cations of blood plasma at about.145 milliequivalents per liter (3345 milligrams) and potassium makes up most of the cell fluid cations at about 150 millequivalents per liter (4800 milligrams). Plasma is filtered through the glomerulus of the kidneys in enormous amounts, about 180 liters per day [4]. Thus 602,000 milligrams of sodium and 33,000 milligrams of potassium are filtered each day. All but the 1000-10,000 milligrams of sodium and the 1000-4000 milligrams of potassium likely to be in the diet must be reabsorbed. Sodium must be reabsorbed in such a way as to keep the blood volume exactly right and the osmotic pressure correct; potassium must be reabsorbed in such a way as to keep serum concentration as close to 4.8 milliequivalents [5] (about 190 milligrams) per liter as possible. Therefore, the sodium pumps must always operate to conserve sodium. Potassium must sometimes be conserved also, but since the amount of potassium in the blood plasma is very small and the pool of potassium in the cells is about thirty times as large, the situation is not so critical for potassium. Since potassium is moved passively [6][7] in counter flow to sodium in response to an apparent (but not actual) Donnan equilibrium [8], the urine can never sink below the concentration of potassium in serum except sometimes by actively excreting water at the end of the processing. Potassium is secreted twice and reabsorbed three times before the urine reaches the collecting tubules.[9] At that point, it usually has about the same concentration as plasma with respect to potassium. If potassium were removed from the diet, there would remain a minimum obligatory kidney excretion of about 200 mg per day when the serum declines to 3.0-3.5 milliequiivalents per liter in about one week,[10] and can never be cut off completely. Because it cannot be cut off completely, death will result when the whole body potassium declines to the vicinity of one-half full capacity. At the end of the processing, potassium is secreted one more time if the serum potassium is too high.

The potassium moves passively through "gates" (pores in the cell wall) and probably through one of the cell wall pumps which also pumps out sodium, three sodium ions for each two potassium ions [11] Even so, the net apparent effect is active in the kidney tubules. When ions move through pumps there is a gate in the pumps on either side of the cell wall and only one gate can be open at once. As a result 100 ions are forced through per second. Pores have only one gate and there one kind of ion only can stream through at 10 million to 100 million ions per second.[12] The pores require calcium in order to open[13] although it is thought that the calcium works in reverse by blocking at least one of the pores. [14] Carbonyl groups inside the pore on the amino acids mimics the water hydration that takes place in water solution[15] by the nature of the electrostatic charges on four carbonyl groups inside the pore.[16]

Potassium is also important in allowing muscle contraction and the sending of all nerve impulses in animals through action potentials. Because of the interaction of the charge on a potassium ion and its surrounding water molecules, K+ ions are actually a little larger than Na+ ions, and ion channels and pumps in cell membranes can easily distinguish between the two types of ions, actively pumping or passively allowing one of the two ions to pass, while blocking the other.

A shortage of potassium in body fluids may cause a potentially fatal condition known as hypokalemia (see article for detail), typically resulting from diarrhea, increased diuresis and vomiting. Deficiency symptoms include muscle weakness, paralytic ileus, ECG abnormalities, decreased reflex response and (in severe cases) respiratory paralysis, alkalosis and arrhythmia.

Eating a variety of foods that contain potassium is the best way to get an adequate amount. Healthy individuals who eat a balanced diet rarely need supplements. Foods with high sources of potassium include in order from highest to lowest avocados, potatoes, bananas, broccoli, orange juice, soybeans and apricots, although pomegranates, parsnips, turnips and many other fruits, vegetables, and meats contain potassium. Research has indicated that diets high in potassium can reduce the risk of hypertension.

The 2004 guidelines of the Institute of Medicine specify an RDA of 4,000mg of potassium. However, it is thought that most Americans consume only half that amount per day . Similarly, in the European Union, particularly in Germany and Italy, insufficient potassium intake is somewhat common.[17]

Supplements of potassium in medicine are most widely used in conjunction with loop diuretics and thiazides, classes of diuretics which rid the body of sodium and water, but have the side effect of also causing potassium loss in urine. A variety of medical supplements are available.

Some people with kidney disease are advised to avoid large quantities of dietary potassium. End stage renal failure patients undergoing therapy by renal dialysis must observe strict dietary limits on potassium intake, since the kidneys control potassium excretion, and buildup of blood concentrations of potassium may trigger fatal cardiac arrhythmia.

[edit] High potassium food

These have more than 225 milligrams per 1/2 cup serving:

* Apricots (fresh more so than canned)
* Avocado
* Banana
* Cantaloupe
* Honeydew
* Kiwifruit
* Lima beans
* Milk
* Oranges and orange juice
* Potatoes (can be reduced to moderate by soaking peeled, sliced potatoes overnight before cooking)
* Prunes
* Spinach
* Tomatoes
* Winter squash

[edit] See also
[hide] v • d • e Alkali Metals

Lithium
Li
Atomic Number: 3
Atomic Weight: 6.941
Melting Point: 453.69
Boiling Point: 1615
Electronegativity: 0.98


|



Sodium
Na
Atomic Number: 11
Atomic Weight: 22.990
Melting Point: 370.87
Boiling Point: 1156
Electronegativity: 0.96


|



Potassium
K
Atomic Number: 19
Atomic Weight: 39.098
Melting Point: 336.58
Boiling Point: 1032
Electronegativity: 0.82


|



Rubidium
Rb
Atomic Number: 37
Atomic Weight: 85.468
Melting Point: 312.46
Boiling Point: 961
Electronegativity: 0.82


|



Caesium
Cs
Atomic Number: 55
Atomic Weight: 132.905
Melting Point: 301.59
Boiling Point: 944
Electronegativity: 0.79


|



Francium
Fr
Atomic Number: 87
Atomic Weight: (223)
Melting Point: ?295
Boiling Point: ?950
Electronegativity: 0.7




* Potassium compounds
* Potassium in biology

[edit] Notes

1. ^ Campbell, Neil (1987). Biology, 795. ISBN 0-8053-1840-2.
2. ^ background radiation - potassium-40 - γ radiation.
3. ^ Thomas K. Wray. DANGER: PEROXIDIZABLE CHEMICALS. Environmental Health & Public Safety (North Carolina State University).
4. ^ Potts WTW Perry G (1964) Osmotic and Ionic Regulation in Animals. MacMillan, NY, on p261.
5. ^ LANS HS, STEIN IF, MEYER KA (1952). "The relation of serum potassium to erythrocyte potassium in normal subjects and patients with potassium deficiency". Am. J. Med. Sci. 223 (1): 65–74. PMID 14902792.
6. ^ Bennett CM, Brenner BM, Berliner RW (1968). "Micropuncture study of nephron function in the rhesus monkey". J Clin Invest 47 (1): 203–216. PMID 16695942.
7. ^ SOLOMON AK (1962). "Pumps in the living cell". Sci. Am. 207: 100–8. PMID 13914986.
8. ^ Kernan RP (1980) Cell Potassium. John Wiley & Sons, NY. On p40 and 48
9. ^ Wright FS (1977). "Sites and mechanisms of potassium transport along the renal tubule". Kidney Int. 11 (6): 415–32. PMID 875263.
10. ^ SQUIRES RD, HUTH EJ (1959). "Experimental potassium depletion in normal human subjects. I. Relation of ionic intakes to the renal conservation of potassium". J. Clin. Invest. 38 (7): 1134–48. PMID 13664789.
11. ^ http://www.rockefeller.edu/research/abstract.php?id=45 Potassium and sodium pumps.
12. ^ Gadsby DC (2004). "Ion transport: spot the difference". Nature 427 (6977): 795–7. doi:10.1038/427795a. PMID 14985745. ; for a diagram of the potassium pores are viewed, see Miller C (2001). "See potassium run". Nature 414 (6859): 23–4. doi:10.1038/35102126. PMID 11689922.
13. ^ Jiang Y, Lee A, Chen J, Cadene M, Chait BT, MacKinnon R (2002). "Crystal structure and mechanism of a calcium-gated potassium channel". Nature 417 (6888): 515–22. doi:10.1038/417515a. PMID 12037559.
14. ^ Shi N, Ye S, Alam A, Chen L, Jiang Y (2006). "Atomic structure of a Na+- and K+-conducting channel". Nature 440 (7083): 570–4. doi:10.1038/nature04508. PMID 16467789. ; includes a detailed picture of atoms in the pump.
15. ^ Zhou Y, Morais-Cabral JH, Kaufman A, MacKinnon R (2001). "Chemistry of ion coordination and hydration revealed by a K+ channel-Fab complex at 2.0 A resolution". Nature 414 (6859): 43–8. doi:10.1038/35102009. PMID 11689936.
16. ^ Noskov SY, Bernèche S, Roux B (2004). "Control of ion selectivity in potassium channels by electrostatic and dynamic properties of carbonyl ligands". Nature 431 (7010): 830–4. doi:10.1038/nature02943. PMID 15483608.
17. ^ http://content.karger.com/ProdukteDB/produkte.asp?Aktion=ShowPDF&ProduktNr=223977&Ausgabe=230671&ArtikelNr=83312&filename=83312.pdf

[edit] References

* Los Alamos National Laboratory – Potassium

[edit] External links
Wikimedia Commons has media related to:
Potassium
Look up potassium in
Wiktionary, the free dictionary.

* WebElements.com – Potassium

Retrieved from "http://en.wikipedia.org/wiki/Potassium"

Categories: All articles with unsourced statements | Articles with unsourced statements | Alkali metals | Chemical elements | Desiccants | Dietary minerals | Potassium
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