Step-by-step explanation:
In this scenario, we can use the reactivity series of metals to predict which pots will get damaged when they come into contact with solutions of certain metal salts. The reactivity series for these metals, from most reactive to least reactive, is:
1. Magnesium (Mg)
2. Zinc (Zn)
3. Iron (Fe)
4. Copper (Cu)
Now, let's analyze each situation:
(i) A solution of magnesium sulfate is kept in a copper pot:
In this case, magnesium is more reactive than copper. When magnesium sulfate comes into contact with copper, a displacement reaction can occur:
Mg + CuSO4 → MgSO4 + Cu
Magnesium will displace copper from copper sulfate, resulting in the formation of magnesium sulfate and copper. The copper pot will not get damaged because magnesium is displacing copper, not the other way around.
(ii) A solution of copper sulfate is kept in an iron pot:
Iron is more reactive than copper. When copper sulfate comes into contact with iron, a displacement reaction can occur:
Fe + CuSO4 → FeSO4 + Cu
Iron will displace copper from copper sulfate, resulting in the formation of iron sulfate and copper. In this case, the iron pot will get damaged because iron is displacing copper, causing the iron to corrode.
(iii) A solution of magnesium sulfate is kept in an iron pot:
Magnesium is more reactive than iron. When magnesium sulfate comes into contact with iron, a displacement reaction can occur:
Mg + FeSO4 → MgSO4 + Fe
Magnesium will displace iron from iron sulfate, resulting in the formation of magnesium sulfate and iron. In this case, the iron pot will get damaged because magnesium is displacing iron, causing the iron to corrode.
So, pots (ii) and (iii) will get damaged in the respective situations because a more reactive metal is displacing a less reactive metal in the salt solutions, leading to corrosion of the pot material.