When Silver nitrate reacts w/ hydrochloric acid, what type of reaction takes place?
353745
Net ionic is\n\nAg+ + Cl- => AgCl\n\nThis is double replacement.
1002183
Concentrated Nitric Acid and copper.  Be careful.  Nasty stuff... really!
972791
HCl + NH4OH → H2O + NH4Cl.\nThere would be heat given off, so you could verify that a reaction took place.\n\n2HCl + Ca(OH)2 → 2H2O + CaCl2\n\nedit: The steps for balanacing the reaction:\n1)We know the salt produced is CaCl2, so an acid with Cl is HCl and a base with Ca is Ca(OH)2. \n2) write the skeleton reaction:\nHCl + Ca(OH)2 → H2O + CaCl2\n3) there are 2 Cl's on the right side, but only 1 on the left. To balance this, place a 2 in front of HCl\n2HCl + Ca(OH)2 → H2O + CaCl2\n4) Now there are 4 H on the left and only 2 on the right, so, place a 2 in front of H2O.\n2HCl + Ca(OH)2 → 2H2O + CaCl2\n5) check with the other elements, each side has one Ca, and 2 O. It all works out ☺
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
438197
This is sulfuric acid and is just as dangerous as hydrochloric acid. However, since you only have one reactant and there is no reaction, you do not have a chemical equation.
866145
HCl + AgNO3-----> AgCl +HNO3\nPb(OOC-CH3)2  + 2LiCl -------> PbCl2  + 2Li(OOC-CH3)\nNa3PO4 + CrCl3 -------> Cr(PO4) + 3NaCl\nH2SO4 + BaCl2 ----------> BaSO4 + 2HCl\nAl2(SO4)3  + 6NH4OH ------> 2Al(OH)3  + 3(NH4)2SO4\n2AgNO3 + H2S -------> Ag2S  + 2HNO3\nCaCl2   + Pb(NO3)2 -------> Ca(NO3)2  + PbCl2\nCa(NO3)2 + Na2CO3 ------>CaCO3  + 2 NaNO3
854318
One needs toluene and concentrated nitric and sulfuric acids, plus "fuming" sulfuric acid (H2SO4 + SO3). As the reaction proceeds, the first nitro groups usually go on either in the position next to the -CH3 (2-, ortho) or diametrically opposite (4-, para). All three mostly end up in the 2-, 4-, and 6-positions. The operator nitrates in three stages, with the temperature raised gradually during the three stages from 35degC to 110degC. However, there is also formation of small amounts of the 2,3,4- and 2,4,5-trinitro compounds. These unsymmetrical isomers make the product dangerously shock-sensitive to handle. The crude product is therefore stirred with 15% aqueous sodium sulfite solution at 100degC. This treatment converts the two impurities to sulfonic acids, which are water soluble and poured away from the oily product in the water.
896618
When calcium hypochlorite is added to water there are three reactions:\n\n     Ca(OCl)2 + H2O  =  Ca(OH)2 + Cl2\n\nChlorine is a reactive gas and will react with the water to form oxygen and hydrochloric acid.\n\n     2H2O   +   2Cl2  =   4HCl  +  O2\n\nThe hydrochloric acid reacts with the Ca(OH)2 to make calcium chloride\n\n    Ca(OH)2 +  2HCl  =  CaCl2  +   2H2O\n\nIt's the O2 that does the bleaching but the chlorine kills the bacteria.\n\nThe sunlight speeds up the reaction between the chlorine and water in two ways.(1) Photochemically - simply some of the energy in the light is used (it splits the chlorine molecules into even more reactive chlorine atoms)  and (2) the sunlight will warm up the water slightly. A 10 degree C rise in temperature will double the speed of reaction so even a 1 or 2 degree rise will have a significant effect.
327609
If I've understood what you're asking then:\nA\nCd(s) + Ag2+ -> Cd2+ + Ag(s) \n\nCadmium occurs at Anode and the Silver would deposit on the Cathode\n\nB (I hate Manganese equations and the partial above is incorrect)\n\nMnO2 + 4H+ + 2AgBr -> Mn2+ 2Br- + 2Ag + 2H2O\n\nMnO2 @ Anode\nAgBr @ Cathode\n\nC\n\n(PtCl4)2- + 4Ag -> Pt + 4AgCl \nAg @ anode\n(PtCl4)2- @ Cathode
928366
The first answer is, like, SO wrong. Gold is one of the least active metals. Check out the Activity Series of metals (you can Google it). The ones at the top of the list (lithium, calcuim, and barium, I think) are the most reactive. They'd react readily with air (they oxidize, releasing hydrogen gas from the water vapor in the atmosphere, forming an oxide or hydroxide). They'd definitely cause an explosion when reacted with acids. Even sodium metal (not salt, I'm talking pure sodium) will react with acids violently.\n\nAll metals react with acids to some degree. Even gold, the most unreactive metal, dissolves in selenic acid. Silver reacts best with nitric acid to form silver nitrate. The coinage metals (Au, Ag, Cu) are the most unreactive.
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
1087032
try Vogel's "Qualitative Inorganic Analysis", I'm pretty sure it has all the answers 4 u.\n\ndont care editions, but for 7th ed, ISBN is 0582218667\n\n****\nokey then, from Vogels\n\n1) when heated, lead nitrate decomposes to white solid lead oxide (PbO), brown gas (NO2) and oxygen gas. Brown gas decolorizes when contact with water. \n\n2) ammonia odur. ammonium compounds are all volatile towards heat and decomposes to ammonia and an acid but quickly recombine if the acid, in this case, hydrochloric acid, is a strong acid.\n\n3) anhydrate copper sulphate is white, hydrate copper sulphate is blue. I have no idea which one you actually heated. If it's anhydrate, no change; if hydrate, blue ---> white.\n\n4) blue precipitate forms initally, but resolve upon excess reagent, clear blue soln results due to the formation of copper complex [blue precipitate: Cu(OH)2*CuSO4, complex: [Cu(NH3)4]^2+]\n\n5) brown precipitates froms [Cu(OH)2], no change with excess reagents.\n\n6) metal-gray stipe (magnesium stipe) gains a redish brown color due to formation of copper metal. Possible decolorization of the soln (depends on how much magnesium u actually put in)\n\n7) volatile reaction, solid metal solves,ignitable gas is formed. (if phenolphthalein is added to water initally, soln becomes pink)
896646
"The final experiment was to observe the reaction when one small crystal of NH4SCN was added to 0.1 M FeCl3. The color of FeCl3 was yellow, but after NH4SCN was added, the color of contents changed to red.\nIn second experiment, when the Mg was ignited, the resulting flame was hot. Therefore, the release of thermal energy through the interaction of Mg and O was shown.\nFiguring out the type of the last two reactions was difficult, because the chemical equations were not given. However, the possibility that the type of both reactions were replacement reactions was high. The reason being that the chemical reactions were observed as a color change and this means that the composition of the substance is changed.\nThis experiment was very successful, and it was a good opportunity to observe chemical reactions directly."\n\nI would change your paragraph to that.  I would also expand on the other experiments if you know more about them.
136146
The 1st answer is wrong. The reaction is\n\nNa2CO3(aq) + SrCl2 (aq)--> 2NaCl (aq) +SrCO3 (s)
618961
6 moles of hydrochloric acid will react at a faster rate than 1 mole of hydrochloric acid because the solution will not dilute as fast as the smaller amount of acid- more acid to react with the Zinc.\n\nSounds good to me...
874441
AgNO3 + NaCl => AgCl(white ppt) + NaNO3\nAgNO3 + KI => AgI( yellow ppt) + KNO3\n\nthere is a change of color because AgI is produced
929088
Explain the reaction of Potassium Nitrate mixed with Amonia Sulfite,with a pinch of Magnesium powder,and a foot of Magnesium Ribbon,and last but not least Benzyl Chloride. It is very important you use Benzyl Chloride.