Which compound will precipitate?
962694
Tehe answer is:\nAg + HNO3 -> AgNO3 + H\nAgNO3 + KBr -> AgBr + KNO3
712818
more soluble in what solution?
341863
ammonium nitrate and aluminum hydroxide\n\nNH4NO3 + Al(OH)3\n\nThe aluminum hydroxide is insoluble when formed and will precipitate out of the solution as a solid powder.
429906
Never trust materials science majors ...\n\n1. NaCl (s) --> Na+ (aq) + Cl- (aq)\n2. Ca (s) + 2H2O (l) --> Ca(OH)2 (s) + H2 (g)\n3. Ca(OH)2 (s) --> H2O (g) + CaO (s)
778796
bcd\n\n\n\nSolution:\nCaCN2 + 3H2O ---> 2NH3 + CaCO3
741136
(a): Si+, P2+\n\n(b) Ar+, S-\n\n(c) Ca+, Cl2-\n\nBut the other answers that you gave are also correct.
361037
It is a mixture. A solution has ions in it and is possible only in liquid phase. A compound is a solid material that is formed when the materials react with each other. Even after they react they form mixed compounds. It is not suspension.
829175
AB + CD ---> AD + CB\nlogic doesn't work here as Si doesn't react/bond with Ca or Phosphorus.and Ca(PO) should be Ca3(PO4)2\nand SiO should be in the form of SiO2. \nso unless you want hypothetical compounds SiO2 won't form with either of the two other reactants.\nbased on the forumlae from an SI data book, the above reaction would not balance.\ngood luck solving this one. :-)
1187925
You have two ionic substances, it will undergo a double displacement reaction.\nPb(C2H3O2)2 + 2 NaCl --> PbCl2 + 2 NaC2H3O2\n\nNow since Lead(II) acetate, Sodium chloride, and sodium acetate are soluble, they break up in water, and the net ionic equation is\nPb2+ + 2 Cl- --> PbCl2\n\nPbCl2 or Lead (II) chloride, is the precipitate formed, and it's generally yellowish.
65886
Synthesis - a compound forms from simpler reactants
872523
You need to specify a compound before we can tell you what its molecular geometry is!
82586
It has a cation or anion that isn't soluble. Stuff like NaCl won't work, because Na and Cl are always soluble. KBr has the same problem. But stuff like NaOH (the OH forms insoluble metal hydroxides) works well.\n\nBasically, you have to look at the solution and the precipitating agent and see if they'll form an insoluble compound.
457655
Iron (II) SulfIDE\n\nSodium ChlorIDE\n\nSodium HydroxIDE\n\nand Lead...umm...something. *lol*\n\nThe answer is evidently (A). =D\n\n\n\nPS okay, so yea, someone already wrote what i wrote when i was typing it. sorry!
906746
a)silver bromide\nb) tricalcium phosphate\nc)Lithum Hydride\nd)Radium Chloride
479476
You need to know concentrations to determine the amount of substance that precipitates out by using solubility products. In this case the precipitate will be CaSO4, so the solubility product will be given by:\n\nk=[Ca(+2)]*[SO4(-2)]\n\nWhere k is the equilibrium constant (probably a given), and [Ca(+2)] & [SO4(-2)] are the concentrations of Ca(+2) and SO4(-2) in the solution. Any amounts greater than the equilbrium concentration will precipitate out as a solid.
837848
Precipitate if it settles to the bottom of the reaction vessel or flask or a product if it remains in solution.
791597
You will get Silver Chromate as the precipitate.  It is red in color.\n2AgNO3(aqueous) + K2CrO4(aqueous) -> Ag2CrO4(solid) + 2KNO3(aqueous)