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  1. › wiki › SodiumSodium - Wikipedia

    Sodium is a chemical element with the symbol Na (from Latin natrium) and atomic number 11. It is a soft, silvery-white, highly reactive metal. Sodium is an alkali metal, being in group 1 of the periodic table. Its only stable isotope is 23 Na. The free metal does not occur in nature, and must be prepared from compounds.

    • silvery white metallic
    • group 1: hydrogen and alkali metals
    • 11
    • Properties
    • Discovery and Name
    • Use as Element
    • Occurrence and Production
    • Use in Organisms
    • Related Pages

    Sodium is a light, silver-coloured metal. Sodium is so soft that it can be easily cut with a knife. When it is cut, the surface will become white over time. This is because it reacts with air to form sodium hydroxide and sodium carbonate. Sodium is a little lighter than water; when it reacts with water it floats. This reaction is very fast. Hydrogen and sodium hydroxide are produced. The hydrogen may ignite. Since sodium melts at a low temperature, it melts when it reacts with water. It has one valence electronwhich is removed easily, making it highly reactive. Compared with other alkali metals (metals in the first column of the periodic table), sodium is usually less reactive than potassium and more reactive than lithium.

    Sodium was discovered by Sir Humphrey Davy, an English scientist, back in 1807. He made it by the electrolysis of sodium hydroxide. It is named after soda, a name for sodium hydroxide or sodium carbonate.

    It is used in the preparation of organic compounds. It is also used in the street lights that are orange, and ultra violet lights.

    Sodium does not exist as an element in nature; its easily removed valence electron is too reactive. It exists as an ion in chemical compounds. Sodium ions are found in the ocean. It is also found as sodium chloride in the earth's crust, where it is mined. Sodium is normally made by electrolysis of very hot sodium chloridethat was melted.

    Sodium ion in the form of sodium chloride is needed in the human body, but large amounts of it cause problems, which is why one should not eat too much salt and other food items with huge sodium amount (such as biscuits with baking soda). Many organisms in the ocean depend on the proper concentration of ions in sea water to live.

    • silvery white metallic
    • 11
  2. Sodium chloride / ˌ s oʊ d i ə m ˈ k l ɔːr aɪ d /, commonly known as salt (although sea salt also contains other chemical salts), is an ionic compound with the chemical formula NaCl, representing a 1:1 ratio of sodium and chloride ions.

    • NaCl
    • 58.443 g/mol
    • 800.7 °C (1,473.3 °F; 1,073.8 K)
    • 360 g/1000 g pure water at T = 25 °C
    • Overview
    • Properties
    • Production
    • Uses
    • Safety
    • Storage

    Sodium hydroxide, also known as lye and caustic soda, is an inorganic compound with the formula NaOH. It is a white solid ionic compound consisting of sodium cations Na+ and hydroxide anions OH−. Sodium hydroxide is a highly caustic base and alkali that decomposes proteins at ordinary ambient temperatures and may cause severe chemical burns. It is highly soluble in water, and readily absorbs moisture and carbon dioxide from the air. It forms a series of hydrates NaOH·nH 2O. The...

    Pure sodium hydroxide is a colorless crystalline solid that melts at 318 °C without decomposition, and with a boiling point of 1,388 °C. It is highly soluble in water, with a lower solubility in polar solvents such as ethanol and methanol. NaOH is insoluble in ether and ...

    Sodium hydroxide is industrially produced as a 50% solution by variations of the electrolytic chloralkali process. Chlorine gas is also produced in this process. Solid sodium hydroxide is obtained from this solution by the evaporation of water. Solid sodium hydroxide is most commonly sold as flakes, prills, and cast blocks. In 2004, world production was estimated at 60 million dry tonnes of sodium hydroxide, and demand was estimated at 51 million tonnes. In 1998, total world production was aroun

    Sodium hydroxide is a popular strong base used in industry. Sodium hydroxide is used in the manufacture of sodium salts and detergents, pH regulation, and organic synthesis. In bulk, it is most often handled as an aqueous solution, since solutions are cheaper and easier to handle.

    Like other corrosive acids and alkalis, drops of sodium hydroxide solutions can readily decompose proteins and lipids in living tissues via amide hydrolysis and ester hydrolysis, which consequently cause chemical burns and may induce permanent blindness upon contact with eyes. Solid alkali can also express its corrosive nature if there is water, such as water vapor. Thus, protective equipment, like rubber gloves, safety clothing and eye protection, should always be used when handling this chemic

    Careful storage is needed when handling sodium hydroxide for use, especially bulk volumes. Following proper NaOH storage guidelines and maintaining worker/environment safety is always recommended given the chemical's burn hazard.

    • NaOH
    • 39.9971 g mol−1
    • 323 °C (613 °F; 596 K)
    • 418 g/L (0 °C), 1000 g/L (25 °C), 3370 g/L (100 °C)
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    • Overview
    • Nomenclature
    • Uses
    • Chemistry
    • Stability & Shelf Life
    • History

    Sodium bicarbonate, commonly known as baking soda or bicarbonate of soda, is a chemical compound with the formula NaHCO3. It is a salt composed of a sodium cation and a bicarbonate anion. Sodium bicarbonate is a white solid that is crystalline, but often appears as a fine powder. It has a slightly salty, alkaline taste resembling that of washing soda. The natural mineral form is nahcolite. It is a component of the mineral natron and is found dissolved in many mineral springs.

    Because it has long been known and widely used, the salt has many related names such as baking soda, bread soda, cooking soda, and bicarbonate of soda, and can often be found near baking powder in stores. The term baking soda is more common in the United States, while bicarbonate of soda is more common in Australia and Britain, and in many northern/central European countries it is called Natron. Abbreviated colloquial forms such as sodium bicarb, bicarb soda, bicarbonate, and bicarb are common.

    In cooking, baking soda is primarily used in baking as a leavening agent. When it reacts with acid, carbon dioxide is released, which causes expansion of the batter and forms the characteristic texture and grain in cakes, quick breads, soda bread, and other baked and fried foods.

    Sodium bicarbonate is one of the main components of the common "black snake" firework. The effect is caused by the thermal decomposition, which produces carbon dioxide gas to produce a long snake-like ash as a combustion product of the other main component, sucrose. Sodium bicarb

    It has weak disinfectant properties, and it may be an effective fungicide against some organisms. Because baking soda will absorb musty smells, it has become a reliable method for used book sellers when making books less malodorous.

    Sodium bicarbonate is an amphoteric compound. Aqueous solutions are mildly alkaline due to the formation of carbonic acid and hydroxide ion: HCO− 3 + H2O → H 2CO 3 + OH−

    If kept cool and dry, sodium bicarbonate can be kept without a significant amount of decomposition for at least two or three years.

    The word natron has been in use in many languages throughout modern times and originated via Arabic naṭrūn from Greek nítron, which can be traced back to ancient Egyptian ntr. The Greek nítron was also used in Latin nitrum and in German Salniter. In 1791, French chemist Nicolas Leblanc produced sodium carbonate, also known as soda ash. The pharmacist Valentin Rose the Younger is credited with the discovery of sodium bicarbonate 1801 in Berlin. In 1846, two American bakers, John Dwight ...

    • 144-55-8
    • 84.0066 g mol−1
    • NaHCO, ₃
    • (Decomposes to sodium carbonate starting at 50 °C)
  4. › wiki › SodiumSodium - Wikipedia

    Sodium is a chemical element wi the symbol Na (frae Laitin: natrium) an atomic nummer 11. It is a saft, siller-white, heichly reactive metal an is a member o the alkali metals; its anly stable isotope is 23 Na.

    • sillery white metallic
    • 22.98976928(2)
    • Na:
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