how are strontium and barium stored?
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(m)\n\nBarium is so reactive it is stored under oil.\n\nstrontium is typically stored under kerosene.
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According to a book I read some time back, "Mellor's Modern Inorganic Chemistry," fluorine is stored in copper lined cylinders.  The F reacts with the Cu, forming a layer of CuF2, which prevents further attack.  Here's a good document on everything you ever wanted to know about handling fluorine:\nhttp://www.llnl.gov/es_and_h/hsm/doc_14.06/doc14-06.html\nI couldn't find anything on cost.
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Spent nuclear fuel is transported in casks made of a combination of materials. Most designs include a lead, steel, and resin-shielded cylinder, within a stainless steel cask. The lead is the component that shields the most radiation, but the other components prevent physical damage to the container, and chemical reactions between the contents and the container.  The most sophisticated containers also contain a layer of water and depleted uranium to provide additional protection from radiation and heat generated by radioactive materials. The components in these casks will give you a good idea what container vessels should include, both for radiation reduction, and safety. \n\nSee this website, which lists specifications for many container vessels for radioactive material: http://www.trex-center.org/casks.asp\n\nThanks for asking this question. The above website is fascinating.
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A.  Iodine is being reduced from +5 in HIO3 to 0 in I2; oxygen is being oxidized from -1 in H2O2 to 0 in O2.\n\nB.  There is no oxidation/reduction going on; this is simple metathesis, producing the barium sulfate precipitate.
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The liquid oxygen goes in the smaller, top tank inside the external tank.  To provide better stability in rockets, one should always put the densest (and heaviest) fuel at the top.\n\nThe propellant mixture in each SRB motor consists of an ammonium perchlorate (oxidizer, 69.6 % by weight), aluminum (fuel, 16 %), iron oxide (a catalyst, 0.4 %), a polymer (such as PBAN or HTPB - a binder that holds the mixture together, 12.04 %), and an epoxy curing agent (1.96 %).
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Color Compound \nRed- strontium salts, lithium salts \nlithium carbonate, Li2CO3 = red \nstrontium carbonate, SrCO3 = bright red  \nOrange- calcium salts \ncalcium chloride, CaCl2 \ncalcium sulfate, CaSO4·xH2O, where x = 0,2,3,5 \nGold- incandescence of iron (with carbon), charcoal, or lampblack \nYellow- sodium compounds \nsodium nitrate, NaNO3 \ncryolite, Na3AlF6 \nElectric White- white-hot metal, such as magnesium or aluminum \nbarium oxide, BaO \nGreen- barium compounds + chlorine producer \nbarium chloride, BaCl+ = bright green \nBlue- copper compounds + chlorine producer \ncopper acetoarsenite (Paris Green), Cu3As2O3Cu(C2H3O2)2 = blue \ncopper (I) chloride, CuCl = turquoise blue \nPurple- mixture of strontium (red) and copper (blue) compounds \nSilver- burning aluminum, titanium, or magnesium powder or flakes
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I'd say the left-most column, the alkali metals. All of them, in the metallic state, explode in contact with water. This is why they must be stored in oil, so they don't come in contact with the water vapor in the air.
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barium: 1s22s22p63s23p64s23d104p65s24d105p66s2\n\nradium: 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s2\n\nsry if it looks a bit confusing without using exponetnts but im sure u could figure it out
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Barium sulfate will precipitate. The reaction is\n\nCuSO4(aq)+ BaCl2(aq)---> 2CuCl(aq)+ BaSO4(s)
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Radium\nI  INTRODUCTION \n\nRadium (Latin, radius,”ray”), symbol Ra, chemically reactive, silvery-white, radioactive metallic element. In group 2 (or IIa) of the periodic table, radium is one of the alkaline earth metals. The atomic number of radium is 88.\n\nRadium was discovered in the ore pitchblende by the French chemists Marie Curie and Pierre Curie in 1898. They discovered that the ore was more radioactive than its principal component, uranium, and they separated the ore into many chemical fractions in order to isolate the unknown sources of radioactivity. One fraction, isolated by use of bismuth sulphide, contained a strongly radioactive substance that the Curies showed was a new element, polonium. A highly radioactive barium chloride fraction was treated to remove the radioactive substance, which was discovered to be a new element, radium.\n\nII  PROPERTIES AND OCCURRENCE \n\nRadium-226 metal melts at about 700° C (about 1292° F), and has a relative density of 5.5. The element oxidizes immediately upon exposure to air. The element is used and handled in the form of radium chloride or radium bromide and practically never in the metallic state.\n\nRadium is formed by the radioactive disintegration of uranium and is consequently found in all uranium ores. Radium is present in uranium ore to the extent of one part of radium to three million of uranium. It is extracted from the ore by the addition of a compound of barium that acts as a “carrier”. The chemical properties of radium are similar to those of barium, and the two substances are removed from the other components of the ore by precipitation of barium and radium sulphate. The sulphates are converted into carbonates or sulphides, which are then dissolved in hydrochloric acid. The radium is separated from the barium as the end result of successive crystallizations of the chloride solutions.\n\nOf the isotopes of radium, ranging in mass number from 206 to 232, the most abundant and most stable is the isotope of mass 226. Radium-226 is formed by the radioactive disintegration of the thorium isotope of mass 230, which is the fourth successive isotope in the decay series starting with uranium-238. The half-life of radium-226 is 1,620 years. It emits alpha particles, forming the gas radon.\n\nIII  USES \n\nRadiation from radium has a harmful effect upon living cells, and radium burns are caused by overexposure to the rays. Cancerous cells, however, are often more sensitive to radiation than normal cells, and such cells may be killed without seriously injuring healthy tissue by controlling the intensity and direction of the radiation. Radium is now used in the treatment of only a few kinds of cancer; radium chloride or radium bromide is enclosed in a sealed tube and inserted in the diseased tissue. When a radium salt is mixed with a substance such as zinc sulphide, the substance is caused to luminesce by the bombardment of the alpha rays emitted by the radium. Small amounts of radium were once used in the production of luminous paint, which was applied to clock dials, doorknobs, and other objects, to make them glow in the dark.
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sodium sulfte is soluble, but barium sulfate would form as a precipitate. Thus\n\nBaNO3 + Na2SO4 -> BaSO4 + 2 NaNO3, or simply\n\nBa(2+) + SO4(2-) -> BaSO4
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The molar mass of Barium is 137.33 g/mol.\n\nDivide the mass of Barium reacted by the molar mass to obtain the number of moles of Barium reacted.\n\n2.74 grams / 137.33 g/mol = .01995 moles of Ba
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It has a 2 microsecond half life, so it is not abundant anywhere. You can hardly keep it in a jar.\n\nIt is made at supercolliders, such as CERN.
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Stored in the ovaries.
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Actually, this is pretty simple.  You have a saturated  solution of lead sulfate (PbSO4) and strontium sulfate (SrSO4).  Probably the biggest hurdle here is to realize that the concentration of sulfate ion will be the same for both salts!  Therefore, the concentration of sulfate ion will be the result of the most soluble of the two salts:\n\nKsp for PbSO4 = [Pb+2]*[SO4-2] = 1.6x10^-8\nKsp for SrSO4 = [Sr+2]*[SO4-2] = 2.8x10^-7\n\nStrontium sulfate is the more soluble of the two salts, so it will control the concentration of sulfate:\n\nSrSO4 ===> Sr+2  + SO4-2, thus [Sr+2] = [SO4-2]\n\nKsp for SrSO4 = 2.8x10^-7 = [SO4-2]^2 , so \n\n[SO4-2] = sqrt(2.8x10^-7) = 5.29x10^-4 = [Sr+2]\n\nNow, to find out the concentration of Pb+2, we use the value we have just calculated for [SO4-2] and the Ksp:\n\nKsp for PbSO4 = [Pb+2] * [SO4-2] = 1.6x10^-8\n\n[Pb+2] = 1.6x10^-8/[SO4-2] = (1.6x10^-8)/(5.29x10^-4)\n[Pb+2] = 3.02x10^-5\n\nand there we have your answers:\n[Sr+2] = [SO4-2] = 5.29x10^-4 moles/liter\n[Pb+2] = 3.02x10^-5 moles/liter
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The answers for your questions must be determined experimentally.  I can only give you some theory behind the answer below.\n\nCalcium chloride can react with ammonia gas to gaive a stable compound with the formula CaCl2*8NH3\n\nThis means one mole of Calcium chloride will adsorb 8 moles of Ammonia.  This means that about 111 grams of anhydrous (bone dry) calcium chloride will adsorb 8 (17) = 136 grams of Ammonia.\n\n136 g / 454 g/lb = 0.300 lb of Ammonia for about every 111 g / 454 g/lb = 0.25 pounds of dry Calcium chloride.\n\nI am sure that the electrical resistance would change but you would need to take experimental readings to see how much.\n\nA mixture of CaCl2 plus CaBr2 seem to be better for Ammonia storage, but may be more expensive.
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Potassium chloride, Chromium oxide, Barium chlorate, Ammonium chloride, Phosphorus trichloride