# Help with Metal reactions in solutions.

my class did a metal activity series lab where we added calcium to 8 different solutions. We have to write the net ionic equations for each reaction but im stuck getting started on them.
Ca(s) + Ca(NO3)2(aq) = ?

my guess

Ca(s) + Ca(NO3)2(aq) + 2H2O(l) --> Ca(OH)2 + H2(g) + Ca(NO3)(aq)

This one reacted in the lab. I also remember gas being formed so do I have to include water in the equation?? but i dont know what the equation is. Another one is

Ca(s) + FeSO4(aq) = im guessing its CaSO4(aq) + Fe(s) ?

again there was gas formation but there is no gas in the equation?

Would really appreciate the help.

AGNuke
Gold Member
Since both solutions are aqueous solution, Calcium can simply react with water to form Calcium Hydroxide and Hydrogen Gas.

In the first one, no overall displacement takes place as the displacing metal and displaced metals, both are the same. In the second one, iron will be displaced by calcium and Calcium Sulphate will be formed. In the second equation, you must include water because Calcium can react with water at room temperature. That too, vigorously. If warm water is taken, the hydrogen gas evolved can catch fire too, giving you Brick-red flame.

Last edited:
Borek
Mentor
we added calcium to 8 different solutions
And the first step was always the same. Depending on the solution composition something else could happen afterwards, but the next stage would be almost the same if you were to add dissolved Ca(OH)2.