will colloidal silver lose effect if mixed with ozonated water?
540901
No....because it doesn't have any effect to lose.....other than the toxicity of being a heavy metal like mercury that is.
444550
The difference in solubility of the components allows for separation.  I don't remember the specifics, but that is the reason.  Water will not have a big enough difference.
320284
It is not possible.  Observe the chemical equation:\nAg2SO4(s) + AgNO3(s) --> Ag2SO4(s) + AgNO3(s)\n\nIn order for a substance to dissolve, it must be in an aqueous solution.
545618
There's no chemical action. The AgI particles act as nucleation centers around which the moisture aggregates and thus falls as rain. It is more of Surface Chemistry.
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
554003
You can remove the tarnish with baking soda, metalic aluminum, and water. The aluminum combines with the sulphur compounds in tarnish (silver sulfide) to form aluminum sulfide, leaving the silver clean. \n\nSilver polishes buff the tarnish off of the silver, leaving a thinner layer on the object. This method keeps the original silver in place.\n\nhttp://scifun.chem.wisc.edu/HOMEEXPTS/TARNISH.html
1143443
Able to be dissolved by water.
559195
Now, THAT is what I call a challenging question! It requires some thinking in addition to the book-ish knowledge and I love it! But, before I continue with my answer, I'd just like to correct one statement:- "I know that peroxide reacts with metals and glass", It does NOT. Metals and glass act as catalysts i.e. they accelerate the reaction of conversion of Peroxide into Water and Oxygen but they don't participate in the reaction.\n\nNow coming to your question, the varying levels of fumes that you are observing have nothing to do with an organic reaction.\n\nLet's address all your situations one-by-one:\n======= ========== ============\n1- When you pour it around the faucet and it bubbles furiously around the crud and not on the spigot itself.\nThe reaction going on in there is the same ol' Peroxide converting to Water and Oxygen.\nOne molecule of Peroxide (liquid) ----> One molecule of Water (Liquid) + Half molecule of Oxygen (gaseous)\n\nWhich is Symbolically-\nH202 (l) -------> H2O (l) + (1/2)O2 (g)\n\nIt's just that the reaction takes place at a faster rate around the crud around the base! \n\nIn general, ANY rough surface acts as a CATALYST for this reaction. Try it yourself, put some peroxide on a smooth surface and then put some on a rough surface. You can easily see that it fumes and bubbles more on a rough surface. It is because on a rough surface there is more AMOUNT of surface on a given area due to all the unevenness of the surface. And more area accomodates more peroxide which leads to more reaction for a given area and hence a faster rate.\n\n======= ========== ============\n2. When you drop earings into peroxide, the whole earings don't bubble only the "gunk" does and when that's gone it stops!\n\nHmm.. This required a little bit of thought process: The "gunk" in your earrings can be two things-\na) Deposition of Dust or dead skin-\nIf this is the case, then the answer would be- "Rough surfaces and dust CATALYZE the reaction of conversion of Perxide into Water and Oxygen which I have already metioned."\n\nb) Deposition of METAL OXIDE because of rusting or corrosion  or tarnishing of your earring.\nNow, if THIS is the case, then the bubbles are coming out due to the REDUCTION reaction by peroxide in the acidic medium.\nLet's see what's happening in there-\nThe Metal Oxide on the surface of your metal earrings is an oxidising agent i.e. it releases Oxygen (Oxygen atom). In presence of an oxidising agent, the Peroxide acts as a reducing agent. It reacts with the oxygen atom like this-\n\nH2O2 (Peroxide) + [O] (Oxygen atom from the rust) -----> H20 (Water) + O2 (Oxygen molecule)\n\nYou can see that Oxygen is being released here, THAT CAUSES THE BUBBLES!\n\n======= ========== ============\n3- It bubbles on cuts but, not on normal skin!\nWhoa whoa whoa... Don't put it on your skin, the reaction of it's conversion to water is exothermic (gives out heat) and sometimes, explosive!\nNow, to answer the question, it might be the tiny dust particles in your abrasion that could be triggerin' off the decomposition reaction & causing the release of Oxygen gas bubbles \nOR as you might be knowing that the pH of the blood is MORE THAN 7, i.e. it is basic or alkaline in nature AND in alkaline solution, this reaction takes place-\nFerrous(Iron) Ions (Fe +3) + Peroxide (H2O2) + Hydroxyl Ions (OH-) ----------> Ferric (Iron) Ions (Fe 2+) + Water (H20) + OXygen Molecules\n\nDid you see that? One of the products in the reaction up there was Oxygen molecules!! Now, that means that we are gonna have some bubbles there as Oxygen gas is gonna bubble baby!\n\nP.S. This is perhaps the longest answer I have ever typed in my entire life!
1082457
Anode is a silver bar and cathode is iron spoon.Electrolyte used is aqueous silver nitrate (AgNO3)\n\nAgNO3 in water ionizes into Ag+  and NO3-\nPositively charged Ag+ ions are attracted by the spoon to be plated.Ag+ reach the spoon and electrons flow from the spoon to the Ag+ ions.Thus, at Cathode:\n[Ag+]  +  [e-] =Ag\nAt the anode, electrons are removed from the Silver metal bar, oxidizing it to the Ag+ state. Thus the silver metal dissolves as Ag+ into the solution, supplying replacement silver for that which has been plated out.\nThus at anode:\nAg - [e-]= [Ag+]\nThts all.
1018313
Silver is being oxidized, nitrogen from the nitrate is being reduced.\n\nOxidation half reaction:\nAg --> Ag+  +  e\n\nReduction half reaction:\nNO3- +  4H+ + 3e  -->  NO + 2H2O\n\nNet balanced and reduced equation:\n3Ag +  NO3- +  4H+ --> 3Ag+ + NO + 2H2O
636208
Lyophilic colloid - The colloidal particles are more attracted to the dispersing medium than to each other.  \n\nThe effect: This prevents the colloidal particles from coagulating (clumping) together to form large particles which will settle out.
832296
A) Ag2O (s) >>> 2 Ag(s) + 1/2 O2 (g)\nB) Nickel (II) Carbonate >>>>>Nickel (II) Oxide + [Carbon Dioxide], NiCO3 -> NiO + CO2\nC) Ammonium Nitrate >>>>> Dinitrogen monoxide + Water,  \nC does not balance as is... but this does:\nNH3NO3 -> N2O +  1.5 H2O + 0.5 O2\n\n48) A) 2 HCl (aq) + Ca (OH)2 (aq) >>>> 2 H2O + CaCl2 (aq)\nB) 3 Ag2 SO4 (aq) + 2 AlCl3 (aq) >>>> 6 AgCl (s) + Al2(SO4)3 (aq) (silver chloride is a precipitate)\nC) H2C2O4 (aq) + 2 KOH (aq)>>>> 2 H2O + K2C2O4 (aq)\nD) CdBr2 (aq) + Na2S (Aq)>>> CdS(s) + 2 NaBr (aq) (Cadium sulfide is a precipitate)\n50 Write a Balanced equation for the complete combustion of each compound:\nA) Butene (C4H8): C4H8 + 6 O2 -> 4 CO2 + 4 H2O\nB) Octane (C8H18): C8H18 + 12.5 O2 -> 8 CO2 + 9 H2O\nC) glycerol (C3H8O3): C3H8O3 + 3.5 O2 -> 3 CO2 + 4 H2O\nD) Acetone (C3H6O): C3H6O + 4 O2 -> 3 CO2 + 3 H2O\n52: Complete these:\nA) Al (s) + H2SO4 (aq)>>>> AlSO4(aq) + H2(g)\nB) 2 HCl (aq) + Ba (OH)2 (aq)>>>> BaCl2 (aq) + 2 H2O\nC) Au (s) + 3 HCl (aq) >>>>> AuCl3(aq) + 1.5 H2 (g)\n54) EACH IS BALANCED BUT "INCORRECT", so correct these:\nA) Cl-2 + NaI(aq) >>> NaCl2(aq) + I-\nB) NH3(aq) >>> N- + H+3\nC) Na (s) + O2(g) >>NaO2(s)\nD) 2Mg (s) + H2SO4(aq) >>Mg2SO4(aq) + H2(g)\nE) MgCl2(aq) + Ca(OH)2(s) >>> Mg(OH)2(s) + CaCl2(aq)\nF) H2 (g) + Cl2 (g) >> H2Cl2 (g)
265632
I'm not sure what the black silver salt you're talking about is, but yes, you can produce Ag(s), the metal, from a silver salt. You need something that will oxidize, so that silver will reduce to Ag(s).
976128
I believe the answer is conductive.  This is the process in which things are silver plated.  \n\nHere's how it goes.You fill a tray that has been lined with aluminum foil with salt water ( or is it plain water ? ).  You run a current through the aluminum foil.  The electrons in the the foil get excited due to the electrical current and start releasing aluminum ions ( Al-, I think )  Now, take your rusty, dull ' silver ' spoon.  Place it in the bath for about 2 hours.  Be careful,  electricity, water and living things don't mix well.  After 2 hours, remove the electrical current source and remove the spoon.  The free ions in the water would have coated the spoon, making it shining again.\n\nActually, toothpaste to clean the spoon is easier.
630717
All of the answers regarding the lack of oxygen to react with the silver are true, but another factor is that metals oxidize quicker when in the presence of an ionic solution, and the air on Mt. Everest has very few ions dissolved in it. So, then not only is there less reagents for the process of oxidizing silver, but there is also a lack of catalyst to speed the reaction up.
953082
Okay, it's been a looooooong time since I had to use my chemistry skills, so lets see what I have:\n\nCopper is more magnetic with electrons than silver is because it's electrons (with fewer of them) are close to the nucleus (or whatever you call it) of the element.  Silver is more apt to lose its electrons with them being so far away.  \n\nCopper is more often found in a +2 state.  So I'd say that's a safe bet to go with.  I'd only assume a +1 state if your teacher said so.\n\nSo therefore:  2AgNO3 + Cu -> Cu(NO3)2 + 2 Ag would probably be your best bet.\n\nBut once again, it's been a long time since I used this so I don't know how right I might be.
233095
Ag+ will react with free Cl- to form AgCl(s).  However, there is no free Cl- in chlorobenzene as it is covalently bound to carbon.\n\nAg+ is also used as a redox reagent (see: mirror test) for certain oxidizable organic molecules.  Chlorobenzene is aromatically stabilized, and therefore unreactive.