Determine net ionic equations, if any, occuring when aqueous solutions of the following reactants are mixed.
Select "True" or "False" to indicate whether or not the stated reaction (or "no reaction") correctly corresponds to the expected observation in each case.
Sodium phosphate and potassium nitrate; No reaction occurs.
Copper(II) sulfate and ammonium carbonate; Cu2+(aq) + CO32-(aq) CuCO3(s)
Nickel(II) chloride and lead(II) nitrate; No reaction occurs.
Ammonium sulfate and barium nitrate; Ba2+(aq) + SO42-(aq) BaSO4(s)
Lead(II) nitrate and sodium chloride; Pb2+(aq) + 2Cl-(aq) PbCl2(s)
2006-10-09 08:22:59 · 2 answers · asked by Magnitudex 2 in Science & Mathematics ➔ Chemistry
Now I need to figure out whether the following equations are true or false...for example whether Copper(II) Sulfate + Ammonium Carbonate actually do yield Cu2+(aq) + CO3 2-(aq) --> CuCO3 (s)
2006-10-09 08:34:06 · update #1
And your question is...?
If you're asking what the net ionic equations are...then you just split apart your compounds into their ions and cancel them out on either side until you're left with the components that react. The ones that are the same on both sides are spectator ions. To be ions, the compounds have to be in aqeous solutions(aq). If all ions cancel then there is no reaction, just a solution.
2006-10-09 08:30:08 · answer #1 · answered by Shaun 4 · 0⤊ 0⤋
Have looked through and amended accordingly.
Sodium phosphate and potassium nitrate; No visible change
Copper(II) sulfate and ammonium carbonate; Cu2+(aq) + CO32-(aq)
CuCO3(s) - green precipitate
Nickel(II) chloride and lead(II) nitrate; Pb2+(aq) + 2Cl-(aq)
PbCl2(s) - white precipitate .
Ammonium sulfate and barium nitrate; Ba2+(aq) + SO42-(aq)
BaSO4(s) - white precipitate
Lead(II) nitrate and sodium chloride; Pb2+(aq) + 2Cl-(aq)
PbCl2(s) - white precipitate
2006-10-10 00:27:44 · answer #2 · answered by Anonymous · 0⤊ 0⤋