Would it be feasible to store a solution of copper sulfate in a container made of metallic zinc? Of metallic silver?
No way. The Zn container will go into solution which will eventually lead to a leak in the container. The reaction is
Zn(s) + CuSO4(aq) ==> ZnSO4(aq) + Cu(s)
For storing CuSO4 in a contain of metallic Ag, that will be OK.
There is no reaction for Ag(s) + CuSO4(aq) ==> no reaction
Storing a solution of copper sulfate in a metallic zinc container is not feasible, as the combination of copper sulfate and zinc would undergo a chemical reaction known as displacement. In this reaction, zinc would displace copper from the copper sulfate solution, resulting in the formation of zinc sulfate and copper precipitates. This reaction would consume both the copper sulfate and the zinc container, leading to the degradation of the container.
On the other hand, storing the solution in a container made of metallic silver is feasible. Silver is not reactive with copper sulfate, so there would be no significant chemical reaction taking place. However, it is worth noting that silver containers may not be the most cost-effective option due to the high price of silver.
To determine the feasibility of storing a solution of copper sulfate in a container made of metallic zinc or metallic silver, we need to consider the reactivity between the metals and the solution.
First, let's look at the reaction between copper sulfate solution and metallic zinc. Copper sulfate is an electrolyte solution, meaning it contains positive and negative ions. When metallic zinc comes into contact with the copper sulfate solution, a displacement reaction occurs. Zinc is more reactive than copper, so it will displace copper from the copper sulfate solution and form zinc sulfate, while copper will undergo deposition.
The reaction can be represented as follows:
Zn(s) + CuSO4(aq) -> Cu(s) + ZnSO4(aq)
Based on this reaction, it is feasible to store a copper sulfate solution in a container made of metallic zinc, as zinc will not dissolve or react with copper sulfate significantly. Instead, it will protect the solution from contamination by forming a layer of zinc sulfate on its surface.
Now let's consider metallic silver. Silver is less reactive than copper, so it will not displace copper from the copper sulfate solution. Thus, storing a copper sulfate solution in a container made of metallic silver would also be feasible. Silver will not react with copper sulfate and will not contaminate the solution.
In summary, both metallic zinc and metallic silver are suitable for storing a solution of copper sulfate, as they will not react significantly with the solution.