Would you store a solution of zinc nitrate in an aluminum container? Use half-reactions to explain your answer.
Al ==> Al^+3 + 3e
Zn ==> Zn^+2 + 2e
Look up the above half reactions and you will see that the Al will go into solution and the Zn+2 will come out. Eventually, enough of the Al container will dissolve to cause a leak in the container.
Therefore, it is not recommended to store a solution of zinc nitrate in an aluminum container.
No, it is not advisable to store a solution of zinc nitrate in an aluminum container. This is because of a reaction called galvanic corrosion that can occur between the aluminum container and the zinc ions present in the solution.
The half-reactions provided are as follows:
Al(s) → Al^3+ + 3e^-
Zn(s) → Zn^2+ + 2e^-
Based on these half-reactions, it is evident that aluminum (Al) will dissolve into the solution as aluminum ions (Al^3+), while zinc (Zn) ions in the solution will be reduced to zinc metal (Zn).
In this scenario, the aluminum container will act as the anode, meaning it will undergo oxidation by losing electrons (Al → Al^3+ + 3e^-). On the other hand, the solution containing zinc nitrate will act as the cathode, where zinc ions (Zn^2+) will be reduced and deposited as zinc metal (Zn).
Over time, this ongoing corrosion process will lead to the gradual dissolution of the aluminum container, as the aluminum ions are continuously being removed from the container and entering the solution. Eventually, enough of the aluminum container may dissolve to cause a leak or compromise the integrity of the container.
Therefore, it is recommended to use a container made of a material that is compatible with zinc nitrate, such as glass or other materials that are resistant to corrosion by the solution.
No, it is not recommended to store a solution of zinc nitrate in an aluminum container. This is because zinc is more reactive than aluminum, as evidenced by their respective half-reactions.
The half-reaction for aluminum is Al -> Al^3+ + 3e^-. This reaction shows that aluminum loses electrons to form aluminum ions with a positive charge. On the other hand, the half-reaction for zinc is Zn -> Zn^2+ + 2e^-, indicating that zinc also loses electrons to form zinc ions with a positive charge.
When the two metals come into contact with each other in the presence of an electrolyte, such as the zinc nitrate solution, a galvanic cell is formed. In this cell, the more reactive metal - in this case, zinc - becomes the anode and undergoes oxidation (loses electrons). The less reactive metal - aluminum - becomes the cathode and undergoes reduction (gains electrons).
As a result of this galvanic cell, the aluminum container would dissolve as aluminum ions are formed, leading to a gradual degradation or even catastrophic failure of the container. This is because the reaction between zinc and aluminum is highly exothermic and results in the formation of corrosion products.
To store a solution of zinc nitrate, it is recommended to use containers made of materials that are not reactive with the solution, such as glass or certain types of plastics.