what soduim thiosulfate would do to silver bromide?
486640
Thiosulfate forms water-soluble complexes with many metals, making it useful in photoprocessing (where it dissolves excess silver bromide on the surface of exposed film, preventing excessive darkening). Thiosulfate is also useful in the extraction of silver from silver ore, in leather manufacture, and as a mordant in the textile industry.
611161
Silver carbonate, Ag2CO3.
831216
Cu (s) + Pb(NO3)2 (aq) ---------> No Reaction. \nCopper will not replace lead.\n\nreaction VI in the attached link.
636325
Photographic film is developed in a sodium thiosulfate solution, which reduces silver ions to silver metal.\n\nNot entirely sure I understand the entire question here . . .
748670
If the reaction goes to fast, i.e.the blue colour appears instantly, you can slow it down by adding more thiosulfate to the solution.\n\nI hope that helped, because otherwise the meaning of your question wasn't very clear to me.
422969
AgNO3(aq)+2Na2S2O3(aq)--> [Ag(S2O3)2]3-(aq) + 4Na+(aq)+ NO3-(aq)
564401
Silver Carbonate  - AgCO3 (3 being the small number on teh O)\nSilver Nitrate - AgNO3\nSilver Sulphate - Ag2SO4
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.
749219
a) Ag2S\nb) SnCl4\nc) Na3N\nd) SrI2\n\nDo us a favor and pay attention during class. That way you'd know how to do these.
958410
1.\nMn(s) + SnCl2(aq) --> MnCl2(aq) + Sn(s)\nCr(s) + 2HBr(aq) --> CrBr2(aq) + H2(g)\nCo(s) + CaBr2(aq) --> N.R\n2Al(s) + 3Ni(NO3)2(aq) --> 2Al(NO3)3(aq) + 3Ni(s)\n\n2.\nMg + 2AgNO3 --> Mg(NO3)2 + 2Ag\nmole of Ag = 3.580 / 108 = 0.033 mole\nmole of AgNO3 = 0.033 mole = 33 mmole\nmolarity of AgNO3 = 33 / 50 = 0.66 M\n\n3.\na.soluble\nb.soluble\nc.soluble\nd.insoluble\ne.soluble\nf.soluble\ng.insoluble in water, soluble in acid\nh.soluble\n\n4.\n3NaOH(aq) + Fe(ClO4)3(aq) --> Fe(OH)3(s) + 3NaClO4(aq)\n3Na+ + 3OH- + Fe3+ + 3ClO4- --> Fe(OH)3 + 3Na+ + 3ClO4-\nFe3+ + 3OH- --> Fe(OH)3\n(NH4)2SO4(aq) + Pb(NO3)2(aq) --> PbSO4(s) + 2NH4NO3(aq)\n2NH4+ + SO42- + Pb2+ + 2NO3- --> PbSO4 + 2NH4+ + 2NO3-\nPb2+ + SO42- --> PbSO4\n\nHope it helps\npeace\nvixklen
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
370859
Presuming that bromine is getting reduced to Br(-) and bisulfite is getting oxidized to sulfate (not including the spectator sodium ion):\n\nReduction half-reaction\nBr2 + 2e ---->  2Br(-)\n\nOxidation half reaction\nHSO3(-) + H2O ----->  SO4(2-) + 2e + 3H(+)\n\nOverall Reaction:\nBr2 + HSO3(-) + H2O ---->  SO4(2-) + 2Br(-) + 3H(+)
482555
AgBr-------->Ag+ + Br-\n(a) Ksp=[Ag][Br] solubility=s=[Ag]=[Br]=Ksp^0.5\ns=(6*10^-7)^0.5\n(b) [Br]=0.01 (because all of kBr was dissuciated)\ns=Ksp/[Br]=(6*10^-7)/0.01 mol/lit
903130
Na2SO4(aq)+ 2 AgNO3(aq)-->Ag2SO4(s)+ 2 NaNO3(aq).
576167
The thiosulfate anion is S2O3--.  It forms salts with various cations.  Sodium thiosulfate is used in photography (as "fixer", or "hypo").  Thiosulfate salts are also used as reagents to determine iodine concentrations, and to dechlorinate tap water.
956142
2Rb(s)+Cl2(g)--2RbCl(s)
854997
CuS + H2SO4 ===> H2S + CuSO4