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When a piece of nickel is placed in a solution of copper(II) nitrate:
a. Solid copper would form on the surface of the nickel metal.
c. Nickel atoms are converted to nickel ions in solution.
d. The blue color of the solution would become lighter.
Let's consider what happens when a piece of nickel is placed in a solution of copper(II) nitrate. Cu has a higher reduction potential than Ni, thus Cu will reduce and Ni will oxidize. This will be a single displacement redox reaction. The corresponding balanced molecular equation is:
Ni(s) + Cu(NO₃)₂(aq) ⇒ Ni(NO₃)₂(aq) + Cu(s)
The net ionic equation is:
Ni(s) + Cu²⁺(aq) ⇒ Ni²⁺(aq) + Cu(s)
<em>Describe what you would expect to observe, if anything, when a piece of nickel is placed in a solution of copper(II) nitrate.</em>
<em>a. Solid copper would form on the surface of the nickel metal.</em> YES. Solid copper will deposit on the surface of nickel metal.
<em>b. The blue color of the solution would become darker.</em> NO. The blue color, caused by Cu²⁺ ions, will become lighter, as their concentration decreases.
<em>c. Nickel atoms are converted to nickel ions in solution.</em> YES. Ni is oxidized to Ni²⁺.
<em>d. The blue color of the solution would become lighter.</em> YES. Due to the decrease in the concentration of Cu²⁺ ions.
<em>e. No reaction would occur.</em> NO.
When a piece of nickel is placed in a solution of copper(II) nitrate:
a. Solid copper would form on the surface of the nickel metal.
c. Nickel atoms are converted to nickel ions in solution.
d. The blue color of the solution would become lighter.
You can learn more about redox reactions here: brainly.com/question/13978139
