how to  test and remeve nitrate?
460809
If you own a single family (domestic) well, it is recommended that you test your water every three years for nitrates; more often if you live in an area with a history of high nitrate levels or if someone in your home is at risk from nitrate contamination. \n\n Reverse osmosis, ion exchange and distillation units could conceivably provide home treatment for removing nitrates from water, but those processes can be complicated, expensive, and generally require routine maintenance. Activated carbon and other simple filters do not remove nitrates to any significant degree. Home treatment units are generally not recommended, particularly as a permanent solution to assure nitrate-free water for infant use.
724819
To determine the concentration of a reagent.
1112820
Please restate, nitrogen 4 oxide N4O is not a common species or do you mean NO2?  For that go to\n\nhttp://www.epa.gov/ttn/emc/promgate.html
699263
V=nRT/P\nn(O2)=3/2(0.0022mol of KClO3) =0.0033 gmol\nR=0.0826\nT=294 k\np = p (O2) + p (water vapour)\np(O2) = 0.926 Atm\nV=(0.0033)(0.0826)(294)/0.926=0.087 liter = 87 ml
566236
click on these links\nhttp://www.spartechsoftware.com/reeko/\nhttp://scifun.chem.wisc.edu/HOMEEXPTS/HOMEEXPTS.html\nhttp://www.hunkinsexperiments.com/\nhttp://www.reachoutmichigan.org/funexperiments/agesubject/lessons/nitrogen.html\nhope u r satisfied
967315
say u are going to perform a test for anion A in some sample. but you know that this test may also have a positive result with other anions B and C. \n\nyou then have to take into consideration that B and C might give you false positives as u test for A. if the background of the sample suggests it may contain B and C then find a way to remove these without affecting A.\n\nthen test for A using your originally proposed method.\n\n\nnow for the example:\nyou are to test for chloride ions. the reagent that comes to mind is aq silver nitrate which will result in white ppt of AgCl. then you realise that a ppt will form with any halide ion such as Br- and I-. you also know that AgBr and AgI solids will dissolve in ammonia while AgCl will not. so you first add ammonia to the sample, then test with silver nitrate. voila, now if a ppt forms, you will know it is AgCl only, and of course the conclusion that Cl- was present.
60733
simply use a hydrometer.
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acid and base\nget red cabbage boil it but don't let the juice go to waste.. collect it\nget  some paper towel and dip it in the juice  pull it out and let it dry... pick it up and cut it in strips... now use it to measure if somethign is acid or base ... blue or green if its a base... red or orange if it's acid... \nthe hypothesis can be on finding out if any liquid is acid or base and the above is the procedure\ngood luck\nbtw a+ in 8th grade with this
427444
Here is everything you need to know about Zinc Nitrate. http://www.jtbaker.com/msds/englishhtml/z3137.htm
765235
Here you are:\n1. multiply the first equation by -1 to get\nN2 + O2 ---> 2NO  H= 180 kJ   {1}\n2. Sum the above equation with the second one:\n2NO + O2 ---> 2NO2 H= -112 kJ   {2}\n\nThe sum is\nN2 + 2O2 ---> 2NO2  (This is what you need)\nSo now sum the Hs for the rearenged equation {1} and the second equation {2}.  This will be the H for the equation you need\n\n-112 + 180 = 68 kJ.
1030444
check if it has GAS !
381445
its ca(no3)2, calcium has a charge of positive 2 and nitrate is only negative 1, so you need 2 of them
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First of all, you need a chemical equation,\n\nNO + O2 ----> NO2\n\nThen, balance it,\n\nNO + 1/2 O2 -----> NO2\n\nNow, what this balanced equation tells you is that the mole ratio between NO and O2 is 2:1. i.e., you need 2 parts of NO to react with every 1 part of O2.\n\nNow, you need to calculate the total number of moles of NO and O2 respectively,\n\n# mole of NO = 17.26/(14+16) = 0.575 mole\n\n# mole of O2 = 13.15/(16+16) = 0.411 mole\n\nAs said before, for every 1 mole of O2, it takes 2 moles of NO to react. From the number of moles of NO and O2, it is clear to see that NO is the limiting reagent. Why? Because if you react all 0.575 mole of NO, it takes only 0.575/2 mole (0.2875 mole) of O2, which you have a lot more than that.\n\nThe limiting reagent is the substance that is NOT in excess, which then determines how much product will be produced (because once this substance is all gone, there will be no reactants to react and give product).\n\nNow, from the balanced equation, you know the mole ratio between NO and NO2 is 1:1. Therefore, the number of moles of NO2 that be formed will be 0.573 moles.\n\nMass of NO2 = # mole * molecular weight\n= 0.573 * (14 + 16 + 16) = 26.465 g
227627
Try a garden nursery. They will have soil testing kits that have test tubes in them.
358327
Nitrates are actually the substance in the nodules on a plant's roots that humans eat and take it the nitrogen because we need nitrogen to grow and change.
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In one experiment 32.40 g of NO is mixed with 19.20 g of O2.\n\n\nThe reaction goes: 2NO + O2 -> 2NO2\n\n\nFirst, you have to find out which is the limiting reactant.\n\nno of moles of NO\n= mass / molar mass\n= 32.40 / (14 + 16)\n= 32.40 / 30\n= 1.08\n\nno of moles of O2\n= mass / molar mass\n= 19.20 / (2 x 16)\n= 0.6\n\nGoing by the equation, there must be twice the no of moles of NO than O2. However, the no of moles of O2 supplied is more than half of the no of moles of NO. Thus, O2 is in excess and NO is the limiting reactant.\n\nWorking with the no of moles of NO,\nno of moles of NO2\n= no of moles of NO\n= 1.08\n\nmass of NO2\n= (no of moles) x (molar mass of NO2)\n= 1.08 x (14 + 2 x 16)\n= 1.08 x 46\n= 49.68g\n\nAnd there you have it! :D
326922
Another easy reaction:\n\nMg(s) + HNO3 ===========> Mg(NO3)2 + H2 (g)\n\nMagnesium reacts rapidly with nitric acid to make magnesium nitrate and hydrogen gas