Why do dillute solutions of heavy metal slats like silver nitrate AgNO3 effectivly kill bacteria?
958171
Protein damage through sulfydryl group interactions.  Proteins within the cell are damaged and the cell cannot proliferate (dies).
147418
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?
834819
Without knowing what reaction you're trying to get, or everything else present, thats a difficult question to answer.\n\nIn a sense. you're forming a silver nitrate solution, but you have to knw all the spectator ions to know what reaction will actually occur.  The silver cation in solution needs to have a anion associated with it.  \n\nThe purpose may also have something to do with the variable solubilities of the silver compound that may be formed.  \n\nAnother potential reaction involves the nitrate as an oxidizing agent.
284044
Try changing the pH of the system and lowering the voltage.  If those don't help go the other way.\n\nhttp://www.cehs.siu.edu/Chemical/silver_waste.htm\n\nhttp://www.p2pays.org/ref/01/00048.htm\n\nhttp://www.finishing.com/73/82.shtml
928716
1.What bacteria are we talking about (E.coli? Which strain?)\n2.There is no such standard solution for any type of bacteria.\n3.Why on earth would you need such a dilution? \n4.What type of facilites do you have access to (You can isolate single cells by FACs provided you have a proper marker and this expensive equipment)
921233
Colloidal Silver is harmful.  It can cause argyria; a condition which causes silver salts to be deposited in the skin giving the skin an ashen grey appearance.\n\nWhile collodial silver may be effective in the labratory against bacteria so is bleach.  And nobody is suggesting you injest bleach.\n\nSale of collodial silver has been banned in both the US and Australia (and probably other places, too.)\n\nMost often, as in the previous answer, the person using collodial silver simply gets better on his own--the silver had nothing to do with it--but credits the silver.\n\nIt does nothing; and is potentially harmful.
117885
its a disinfectant - kills bacteria (germs)\n\ncheck the label though...
434812
Looks like nasty stuff.\n\nSearch Google for \n\n"sodium azide" MSDS\n\nThat should turn up some MSDSs.  Also look for a Merck article on it.\n\nHere is the beginning of the Wikipedia article:\n\nSodium azide (NaN3) is a highly toxic chemical that exists as an odorless white solid. Its solution in water is slowly hydrolyzed into a very toxic gas, hydrogen azide (HN3), which also forms when NaN3 reacts with a strong acid. It may react with heavy metal ions such as copper, silver or lead to form metal azides which are very unstable, easily synthesized, and highly explosive. Care should be taken when disposing of this material down the sink as it may react with the plumbing material.
1185928
put your object in a concentrated solution of HCl (muriatic acid) , the silver will precipitate as silver chloride, you can now filter the solution and keep the silver chloride. Then add ammonia to the silver chloride to solubilise the AgCl. Then put a copper wire in the solution, the silver will precipitate on the copper, put copper until no silver is appering. you can now filter the liquid to obtain pure silver
823469
All nitrates are soluble.  You would need to consult a table of solubilities to see what other ions you could use to precipitate out the cations.\n\nEx:  If you had silver nitrate in a solution you could add something with a halide ion such as sodium chloride.  The silver ion would precipitate out with the chloride ion.  If no ppt forms with the sodium chloride you know it was not silver ions.\n\nThen look for other ions that you could test for.
874059
I think that isolating potassium is the wrong approach.  Potassium metal reacts with atmospheric water to form KOH and hydrogen gas.  If you accidentally get water on the metal the reaction is so vigourous that the metal will catch fire, which will be dangerous.  \n\nTry a different approach.  Dissolve KCl in water and add a molar equivalence of Silver iodide, AgI, also dissolved in water..  AgCl is nearly insoluble in water (~0.9 mg/L at 10C)  and will precipitate out, leaving KI in solution.  Filter out the AgCl and evaporate the water, leaving solid KI.  \n\nThe two biggest problems starting with KNO3 are:  It will be nearly impossible to salt out the nitrate because of its high solubility in salt form, and two, many nitrate salts, particularlyof metals, are highly explosive and dangerous.  KCl is cheap and plentiful, so why not just buy some?
701423
1] It is a bleaching agent\n\n 2] It is used in making Mortar,which is a building material ,is a  \n     mixture of slaked ,lime and water.\n\n 3]It neutralises the acidity of soil.Being an alkaline  \n   compound,slaked lime increases the fertility of soil by              neutralizing the harmful effects of acid rain.Also makes the soil porous.\n\n 4]as water softener:addition of slaked lime to hard water              removes hardness.\n\n 5] used in manufacture of bleaching powder,and in the purification ofsugar and coal gas.
76820
I agree with the previous answer; magnesium nitrate is probably more soluble, at 125 g/100 mL water versus magnesium chloride's 54.2 g/100 mL.  Nitrate's ionic bond (not "bound") is weaker probably because of its higher electron density pulling away from that bond.  \n\nSolubility rules tell us that all nitrates are soluble, but silver, mercury, and lead chlorides are insoluble.
706927
a. Silver nitrate\nb. isopropanol? methanol?\nc. Potassium chloride\nd. Benzene\ne. Carbon monoxide\nf. Sodium hydroxide
206939
OK ... I don't know about the heavy metals ... but I sure wouldn't want my vacuum cleaner "dust" to be in my compost bin, and I sure wouldn't want to use the compose on any gardens that might grow things I could eat!\n\nWhy?\n\nThink about it ... most DUST is actually dead skin and dust mites, and other little critters ... DUST is DISGUSTING.
238675
If the reactants are in aqueous solution, in high enough concentrations, then solid silver chloride (AgCl) will precipitate. Sodium nitrate wiill remain in solution as sodium and nitrate ions. No chloride ions should remain - they will all have reacted with the silver ions.\n\ni.e.   AgNO3 + NaCl  + NaNO3   ->    AgCl  +   NaNO3\n\nDon't forget to balance the equation.
564401
Silver Carbonate  - AgCO3 (3 being the small number on teh O)\nSilver Nitrate - AgNO3\nSilver Sulphate - Ag2SO4