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Part I: Changes in Reactant or Product Concentrations
A. Copper and Nickel Ions
Observed colors of the solutions:
Copper (II) Ions
Nickel (II) Ions
CuSO4(aq):
clear, light blue
NiCl2(aq):
clear, light teal
[Cu(NH3)4]2+(aq):
clear, dark blue
[Ni(NH3)6]2+(aq):
cloudy (precip), dark blue/green
After HCl addition:
produced heat and formed water vapor
After HCl addition:
produced heat, water vapor, cleared the color, and removed the precipitate
a.) Explain your observations upon addition of NH3(aq) to the CuSO4 and NiCl2 solutions. Include balanced net ionic equations (2) and explain what happens in the reactions in terms of LeChâtelier’s principle as more NH3(aq) is added.
b.) Explain your observations upon addition of HCl(aq) on the solutions. Include the balanced net ionic equation for the reaction that occurs. Explain which way the equilibria in (a) shift and why in terms of LeChatlier’s principle as HCl is added.
c.) What initially forms as pale blue and pale green precipitates when NH3(aq) is added to [Cu(H2O)4]2+ and [Ni(H2O)6]2+ solutions, respectively? Why do these precipitates form?
B. Cobalt Ions
Color of original CoCl2 solution:
Clear, see through red, no precipitate
Color after adding HCl(aq):
Dark purple, clear, formed water vapor
Color after adding H2O:
Cleared changes, returned to red, see through.
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