Net ionic question, please help!!!?

Question

Write the balanced net ionic equations for each of the following reactions:
1) A soluition of sodium thiocyanate id added dropwise to a solution of nickel chloride
2) Solid calcium oxide is heated in the presense of sulfur trioxide gas
3) Equal volumes of .1 M sulfuric acid and .1 M potassium hydroxide are mixed.
4) Calcium metal is heated strongly in nitrogen gas.
5) Solutions of .1 M ammonia and .1 M acetic acid are mixed to the equivalence point.
6) Iron metal is immersed in a solution of silver chloride.
7) A concentrated solution of ammonia is added to a solution of zinc iodide.
8) A solution of copper (II) sulfate is added to a solution of barium nitrate.

Thank you so much! I just don't get these net ionic things!

Answer 1

1) Ni2+ + 2 SCN- ---> Ni(SCN)2
2) CaO + SO3 ---> CaSO4
3) H+ + OH- ----> H2O
4) 3 Ca + N2 ----> Ca3N2
5) NH4OH + CH3CO2H ---> NH4+ + CH3CO2- + H2O
6) Fe + 2 Ag+ ---> Fe2+ + 2 Ag
7) Zn2+ + 4 NH3 ---> Zn(NH3)4(2+)
8) Ba2+ + SO42- ---> BaSO4

Only include the species that actually react. In the case of #5, because ammonia and acetic acid are weak, the whole species plays a role in the reaction. In the case of #3, sulfuric acid and potassium hydroxide are both strong, so the counterions are truly spectators. Unlike what was said above, there is a net ionic equation for that reaction, and it is the combination of hydrogen ion and hydroxide ion to form water.

Answer 2

I'll do 1,2, and 3.
To find net ionic equations, all you do is first make the molecular equation and break the ionic compounds into their separate components. For #1:
2NaSCN + Ni(II)Cl2 ---> 2NaCl + NiSCN2
= 2Na + 2SCN + Ni + 2Cl -----> 2Na + 2Cl + Ni + 2SCN
Now look up which of the compounds is soluble: the ions are Na and Cl. So you eliminate the two because they are not the precipitate (the point of the net ionic is to get the precipitates, or the insoluble compounds) and get:
= 2SCN + Ni ----> Ni(SCN)2
By the way, you have to show the superscript charges for each of them.
For #2:
CaO + SO3 ----> CaSO4
The only ion is CaO, and there is no real net ionic reaction that can be written because this isn't a replacement reaction.
For #3:
H2SO4 + KOH -----> K2SO4 + H2O
Ok, this is interesting. There is no net ionic equation that can be written because all the products are soluble in water, or aqueous. Therefore, you will not get a solid or gas that precipitates from the reaction at the end. Thus, there is no net ionic reaction that can be written here.
Ok, try this with the next four:
1)write out molecular equation
2)break it into separate ions (CaH becomes Ca + H, for example; Ba(NO3)2 becomes Ba + 2NO3)
3)drop any ions that are aqueous, or soluble in water (research online or in book to find this info)
drop any that do not change from reactant to product
4) check to see that the equation is a replacement reaction; that is, ions get switched around. If not, then there is no net ionic reaction (like in #2)
Ok, good luck!

Answer 3

Ionic Equation: Ba2+(aq) + 2 Cl-(aq) + 2 NH4+(aq) + CO32-(aq) --> 2 NH4+(aq) + 2 Cl-(aq) + BaCO3(s) To produce the net ionic equation, you cancel out anything that does not change forms or states on the two sides of the equation--that is, you remove anything that is exactly the same on both sides: Net Ionic Equation: Ba2+(aq) + CO32-(aq) --> BaCO3(s)

Answer 4

a)2 Na(CNS) + NiCl2 -> Ni(CNS)2 + NaCl
b) CaO + SO3 -> CaSO4
c) H+ + OH- -> H2O
d) 3Ca + N2 -> Ca3N2
e) NH3 + CH3COOH -> CH3COONH2 + H2O
f) Fe + 2AgCl -> FeCl2 + 2Ag
g) 2NH4OH + ZnI2 -> [Zn(NH3)2]I2 + 2H2O
h) Ba2+ + SO4 2- -> BaSO4 (ppt)

Answer 5

here you are with my try:

1) 2SCN(-) + Ni(++) -----> NiSCN(s)
2) CaO(s) + SO3 (g)-----> CaSO4 (s)
3) 2H+ 2OH -------> 2H2O
4) 3Ca(s) + N2(g) ----> Ca3N2(s)
5) NH3(aq)+ CH3COOH(aq) -----> NH4(+) + CH3COO(-)
6) Fe(s) -----> Fe(s)
7) ------
8) SO4(2-) + Ba(2+) -----> BaSO4(s)

Hope it helps!