what salt gives a precipitate with silver ion in acid solution and also produces an ammoniacal odor with NaOH?
149740
Ammonium chloride. With silver ion, silver chloride (white) precipitates out. With NaOH, the proton in ammonium ion is donated to hydroxide and the ammonium ion now becomes ammonia, which is what you smell.
179839
It depends on the salt. A salt of calcium, magnesium, or iron will form an insoluble compound that will precipitate with a soap molecule that is known as soap scum.\n\nHere is a typical reaction:\nCa2+(aq)  + 2C17H35COO-(aq)  ==> (C17H35COO-)2Ca2+(s)\n\nSodium chloride will not form a precipitate with soap as long as the soap is a carboxylate.\nhttp://dl.clackamas.cc.or.us/ch106-04/structur1.htm
217892
Apart from the precipitation reactions (AgCl and BaCO3 form insoluble compounds, although HCl will dissolve BaCO3), there is flame colouring for identifying the alkali and earth alkali metals (Na yellowish orange, Li reddish, Ba green), there are pH measurements (HCl acidic, NaOH and Na2CO3 basic, rest neutral), and you need to test an oxidant to identify the sugar solution. This ought to give you a matrix which gives only one possible identification for each test (with deionized water failing all tests).
564401
Silver Carbonate  - AgCO3 (3 being the small number on teh O)\nSilver Nitrate - AgNO3\nSilver Sulphate - Ag2SO4
294143
add:\n\nH2S2O8(ag)+ NH3(aq) + ? -->(NH4)2S208(aq)  + ?\n\nAmmonia can be prepared in the laboratory by treating ammonium chloride with sodium hydroxide:\n\nthe net ionic equation to this reaction is:\n\n NH4+(aq) +  OH-(aq) ---> NH3(g) + H2O(l) in system 1\n \nand\n\n NH3(g)   = NH3(aq) in solution in system 2\n\nyou finish it ,if you need more help just e-mail me
355760
It's [Cu(NH3)6]2+ or hexaamine copper (II)
339232
Yes, the reaction would spontaneously occur because Sn is higher on the activity series than Ag.\n\nSn(s) + 2AgNO3(aq) => Sn(NO3)2(aq) + 2 Ag(s)\nThe net ionic is\nSn(s) + 2Ag+(aq) => Sn+2(aq) + 2 Ag(s)\n\nI don't remember the oxidation number for Sn.  2 sounds about right.\n\nIt would turn a silver nitrate solution to a tin nitrate solution, and you'd see metallic silver precipitate out.
521349
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.
324126
The salt that is formed is Barium sulphate, which simply has low solubility in water (or acid or bases - you need a chelating agent for the Barium to dissolve it again). There is  no other significant reaction (like redox or altering pH).
457812
Ammonia, baking soda.
51552
AgNO3 + NaCl -----> AgCl + NaNO3\n\ntotal ionic equation\n\nAg+  +  NO3-  +  Na+  +  Cl-\n\n                      ----->\n\n                            AgCl  +  Na+  +  NO3-\n\nnet ionic equation\n\n    Ag+  +  Cl-  ----->  AgCl
875003
Silver acetate (AgC2H3O2) is a photosensitive, white crystalline substance commonly used as a pesticide. It also produces a repulsive taste when combined with cigarette smoke, so it is used in chewing gum and lozenges to aid the cessation of smoking.\n\nOther names Acetic acid, silver (1+) salt\nMolecular formula AgC2H3O2\nMolar mass 166.91 g/mol\nAppearance white to slightly grayish powder\nslightly acidic odour\nCAS number [563-63-3]\n\nProperties\nDensity and phase 3.26 g/cm3, solid\nSolubility in water 1.02 g/100 g (20 °C)\nBoiling point decomposes
36586
Ag+ + SO4(2-) ---> Ag2SO4\nYeah, it's double replacement, and according to my solubility rules, AgSO4 is insoluble.
706927
a. Silver nitrate\nb. isopropanol? methanol?\nc. Potassium chloride\nd. Benzene\ne. Carbon monoxide\nf. Sodium hydroxide
225436
Here is one :\n\nAn aqueous solution of hydrazine can be prepared by reacting ammonia with a solution of sodium hypochorite:\n\nthe net ionic equation:\n\n2NH3(aq) + OCl-(aq) ---> N2H4(aq) +  H2O(l) + Cl-(aq)\n\n""" CAUTION""""\n\nMixing these chemicals together is very dangerous. Please on paper  analysis only .
747313
1) Zinc Chloride\n2) Copper (II) Sulphate\n3) there is no such thing as NH4OH, but oh well..\n    Ammonium Hydroxide\n4) Iron (III) Sulphide\n5) Aluminium Phosphate\n6) Lead (II) Nitrate\n7) Sulphur hexafluoride\n8) Sodium Sulphate\n9) Mercury (II) oxide\n10) Potassium Clorate (V)\n11) Tin (II) Choride\n12) Iron (II) hydroxide\n13) Mercury (II) Sulphate\n14) Carbon Dioxide
1002183
Concentrated Nitric Acid and copper.  Be careful.  Nasty stuff... really!