For each of the following situations, identify those for which a reaction likely to occur. For those that do occur, white a net ionic equation.
a) Chromium dipped into silver nitrate.
b) Gold immersed in hydrochloric acid
c) Nickel pellets dropped into calcium acetate, Ca(C2H3O2)2.
d) Aluminum dropped into a bath of sulphuric acid.
e) Zinc dipped into a solution of lead(II) nitrate.
The Attempt at a Solution
This is what I got:
a)Cr(s) + 2AgNO3(aq) --> Cr(NO3)2 + 2Ag(s)
Separate the aqueous ions:
Cr(s) + 2Ag(aq) + 2NO3(aq) --> Cr(aq) + 2NO3(aq) + 2Ag(s)
Then I'm supposed to remove the ions common to both sides...but
then I end up with none at all b/c each one is on both sides...???
b) no reaction
c) no reaction
d) 2Al(s) + 3H2SO4(aq) --> Al2(SO4)3(aq) + 3H2(g)
Here I get the same problem as in (a) when I separate them.
e) Zn(s) + Pb(NO3)2(aq) --> Zn(NO3)2(aq) + Pb(s)
Again, same problem....if I separate the aqueous ions and get rid of the common ones I end up with nothing.
What am I doing wrong? If someone can show me how to do this that would be great, thanks!