The tin ion, Sn2+, and the nitrate ion, NO3-.
This compound is called strontium nitrate.
Tin Nitrate.
Tin (II) Nitrate
Sn(NO3)4 is Tin (IV) sulfate
This compound is strontium nitrate.
The compound is tin(II) nitrate.
Zinc is most reactive of the three. So if you put a piece of zinc metal to the three solution you will observe, In the Zinc nitrate solution there is no reaction while others have. As zinc is most reactive of three, in will displace the respective metals out of their solution. If the zinc is coated with reddish covering, it is Copper nitrate. If is coated with silvery needles, the solution is Tin nitrate.Zn + Cu(NO3)2 ----> Cu + Zn(NO3)2Zn + Sn(NO3)2 ----> Sn + Zn(NO3)2Zn + Zn(NO3)2 ----> [No reaction]
Tin (ii) Nitrite also called Stannous Nitrite, has the formula Sn(NO2)2 and a molar mass of 210.721
Formula: Sn(NO3)2
Sn (s) + 2HNO3(aq)-> H2O(l) + 2NO2(g)+SnO(s) If the product formed is Tin (II) oxide, then the above should be the balanced equation. Tin (II) oxide can be blue black or red, depending upon the stability.
-1 for each Cl, +2 for Sn
Formulas are: Sn(NO3)2 and Sn(NO3)4.
Zinc is most reactive of the three. So if you put a piece of zinc metal to the three solution you will observe, In the Zinc nitrate solution there is no reaction while others have. As zinc is most reactive of three, in will displace the respective metals out of their solution. If the zinc is coated with reddish covering, it is Copper nitrate. If is coated with silvery needles, the solution is Tin nitrate.Zn + Cu(NO3)2 ----> Cu + Zn(NO3)2Zn + Sn(NO3)2 ----> Sn + Zn(NO3)2Zn + Zn(NO3)2 ----> [No reaction]
Tin (ii) Nitrite also called Stannous Nitrite, has the formula Sn(NO2)2 and a molar mass of 210.721
The chemical formula of stannous nitrate is Sn(NO3)2.
It is Sn(NO3)4
Sn(NO3)2
Formula: Sn(NO3)2
POSSIBLE ANSWER: nickel (Ni) EXPLANATION: all metals dissolve in water more or less and there is an equilibrium point at which the dissolving rate and the condensing rate are the same. If the solution already has enough nickel ions (in other words it is a saturated solution), then the solid nickel you put in will not dissolve.
Sn (s) + 2HNO3(aq)-> H2O(l) + 2NO2(g)+SnO(s) If the product formed is Tin (II) oxide, then the above should be the balanced equation. Tin (II) oxide can be blue black or red, depending upon the stability.
The reaction is:Pb2+ (aq) + 2NO3- (aq) + 2H+(aq) + 2Cl- (aq) --> PbCl2 (s) + 2H+ (aq) + 2NO3- (aq)The italicized items cancel out leaving just the reactants and the precipitate.Pb2+ (aq) + 2Cl- (aq) --> PbCl2 (s)
Tin(IV)cyanide is Sn(CN)4 and will dissociate into five ions.
previous answer-> "tin(II)nitride --> SnN" what?? I'm pretty sure it's Sn3N2 Nitrogen (nitride) has -3 charge