How copper sulphate inhibits the growth of bacteria.?
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Copper is an essential plant micronutrient with a wide range of other agricultural applications; however, as is the case with many plant nutrients, an excess of copper can be toxic to plants and other organisms. Fungi are particularly susceptible to copper and for this reason, copper is frequently used as a fungicide and wood preservative. Many invertebrates, algae, and bacteria are also sensitive to copper and it has can be used against these pests as well. Because copper is a mineral element, it can accumulate in soils. Low levels do not pose a risk to soil life and may even enhance plant growth if soil copper levels are deficient; however, higher levels can be detrimental to soil life, particularly earthworms. They can also be toxic to fish. Copper compounds must also be handled carefully since they can present a health risk for humans. \n\nCopper is a restricted input in organic systems. Its use must be monitored to avoid build up of copper in soil. Many certifying bodies, particularly in Europe, are beginning to re-assess its use in organic systems. \n\nThere are many forms of copper available for use. Copper sulphate, often referred to as "bluestone", is the most common form of copper allowed for use in organic systems. It is a finely ground powder that dissolves relatively quickly in water and should be stored in a dry place to avoid clumping. Copper sulphate is frequently combined with hydrated lime to make what is known as a Bordeaux Mixture. Because hydrated lime is not permitted under organic standards, Bordeaux mix is frequently prohibited for use in organic systems. Other approved forms are copper hydroxide and copper oxychloride. Prohibited forms of copper are copper ammonia base, copper ammonium carbonate, copper nitrate and cuprous chloride. \n\nAs a fungicide, copper is now being replaced by newer biological agents, such as Bacillus subtilis, which directly kill fungal pathogens, or by fish emulsions and compost teas, which act to stimulate a plant’s own defence against pathogens. \n\nCopper products are readily available at farm supply stores.
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they improve water holding capacity of sandy soil.\nthey also increase infiltration rates of water through clay soils.\nthey absorb, store and release soluble fertilizer and nutrients.\nso, they are used in farming and gardening (agricultural uses)\nan example is CuSO4.5H2O (pentahydrate copper sulfate)!
792118
As copper is more reactive than silver it will give up its two electrons to silver ions so when is really happening is:-\n\n2Ag+  + Cu → Cu++ + 2Ag\n\n(The nitrate ions (NO3‾) are passive)
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Nitric acid is a very strong oxidizing agent, so on reaction with metals, it gives salt (nitrate), nitrogen dioxode and oxygen.\n\nE.g: Cu + HNO3 ---> Cu(NO3)2 + NO2 + O2\n\nHNO3 self undergoes reduction to NO2 and metals reacting are oxidized.\n\nMetal with HCl give salt and hydrogen and with dilute sulphric acid give salt and hydrogen too, but if you use concentrated sulphuric acid with some metals, then SO2 can be released, because again with more concentration, sulphuric acid becomes a stronger oxidizing agent and gets reduced to SO2 in a redox reaction.\n\nEDIT: The reaction above for copper occurs with concentrated nitric acid; if dilute nitric acid is used, NO would be released instead of NO2.
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anhydrous copper sulphate is white in colour because it forms an ionic bond with the sulphate ions using the 4s shell electron.when water molecules form bond with copper sulphate as water has two free electron pairs and due to splitting in energy levels of copper atom these electons absorb white light and go to higher energy level and come back to lower level but higher than the initial one and emit blue colour photons.this means that hydrated copper sulphate is blue in colour and anhydrous one due to absence of water molecules is white in colour.
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there is none.  Silver was being used hundreds if not thousands of years before the concept of microbes was used.  That's like asking why does organic matter reak down to make oil for cars?
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CuSO4·5H2O(s) → CuSO4(s) + 5H2O(g)
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There are a vast number of water soluble corrosion inhibitors.\n\nAt the simple end of the scale - Sodium nitrite, sodium tolytriazole, zinc phosphate, borates, molybdates, vanadates and chromates all inhibit rust.\n\nThere are also proprietary organic compounds (some phosphate esters, ethanolamides, etc) also inhibit rust.\n\nIt all depends on whether you want the inhibition to be short lived or long lived (nothing is "permanent") and whether the inhibition is an "in use" inhibitor (like, say, a corrosion inhibitor in cooling water) or "static" (like phosphate "rust converters" used prior to painting.
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CuCl2 + 2NH4OH --> Cu(OH)2 + 2NH4Cl\n\nCu(OH)2 (s) + 4NH3 (aq)     ----->     Cu(NH3)4^2+
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Thiobacillous feroxidans, gains energy by oxidising sulfur to form sulfurous acid, (H2SO3), and sulfuric acid. (H2SO4)\nThose acidic byproducts attack the iron and steel of popes in the ground. Where iron Fe is converted to Fe2O3 (hematite, or red iron oxide). The reaction is even more efficient than normal in that the bacteria are probably a constituent of the biofilm slime that attaches to the pipe. Hence their byrduct acids are less likely to diffuse into the surrounding soil, but stay next to the pipe in a higher concentration. This reaction causes billions of dollars in damage to buried pipes yearly.\nDan the Answers-Man
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There are several ways in which salt and sugar inhibit microbial growth. The most notable is simple osmosis, or dehydration. The salt or sugar, whether in solid or aqueous form removes free water molecules in the food that is necessary for microbial survival and growth.\n\nThey may also inhibit enzymes activity directly or indirectly by helpng in the accumulation of antimicrobial produts from other organisms.
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Solid copper sulfate is a bluish crystal that is highly water soluble. It would therefore dissociate to form copper (II) and sulfate ions when placed in water. It DOES NOT react with water.
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Cu + 2H2S04 --> CuSO4 + SO2 + 2H20\n\nCu (copper) is oxidized, because it loses 2 electrons to enter into the +2 state.\n\nThe sulfuric acid is the oxidizing agent, because it oxidizes the copper and is itself reduced to form sulfur dioxide. (Compare the oxidation states. Half of it remains as SO4- because it takes 2 equivalents of H2SO4 to react with Cu, due to the mole to mole ratio.)\n\nI'd do this reaction in the fume hood, though. SO2 is an irritant to your lungs.
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Actually the copper doesn't come directly from the solution...\n\nNot sure how much detail you want, but it does use electroplating.  This means that it uses electricity to plate metal on an object.  The stainless steel object is put on the "positive end" and a lump of pure copper is placed on the "negative end."  A low voltage is used because a high voltage plates too fast, and the layer will peel off quickly.  If copper is the plating, then the solution must be a fairly low-concentration copper sulfate (CuSO4) solution, meaning that copper is the only metal present in the electrochemical cell.  The negative end is called the anode, and this decreases in mass as its copper ions are taken to the positive end -- the cathode.  \n\nThis method of plating multiple metals is actually fairly common, because the properties of each one can be combined.  Nickel can be used for farm equipment and engines because it can withstand a lot of force, silver is used for decoration, chromium is used to withstand a lot of use (like a spoon).  Copper is able to conduct heat and helps food cook evenly.
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definitely sulphate... lol...ne ways, u gotta mix those stuff n leave it over nite to crystalise..then break it to pieces..or, u can jus ask ur chemistry teacher..haha.. all i did in sch was crystalizing copper sulphate usin the solution itself..
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copper most easily interact with oxygen than the other metals\ncoins are made of
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It breaks down the cell wall of the bacteria.