Question

Solid nickel reacts with aqueous lead (II) nitrate to form solid lead. What is the net ionic equation for this reaction? • Hint: In this reaction, nickel exhibits its most common oxidation state of +2. • Be sure to include the charge for each ion in the net ionic equation. Provide your answer below: (s) + (aq) → *(n)

Answer 1

Ni(s)+Pb2+(aq)→Ni2+(aq)+Pb(s)

Step-by-step explanation:

The complete ionic equation of this reaction is

Ni(s)+Pb2+(aq)+2 NO−3(aq)→Ni2+(aq)+2 NO−3(aq)+Pb(s)

The nitrate ions are spectator ions and can be removed from the equation, giving us

Ni(s)+Pb2+(aq)→Ni2+(aq)+Pb(s)

Answer 2

Pb²⁺(aq) --> Ni²⁺(aq)

Step-by-step explanation:

The equation of the reaction is given as;

Ni(s) + Pb(NO₃)₂(aq) --> Pb(s) + Ni(NO₃)₂(aq)

In writing the ionic equation, we break the aqueous compound into ions. The solid and liquid compounds are ignored.

We have;

Pb²⁺(aq) + NO₃²⁻(aq) --> Ni²⁺(aq) + NO₃²⁻(aq)

Canceling the spectator ions;

Pb²⁺(aq) --> Ni²⁺(aq)