Four metal A, B, C and D are added to the following aqueous solutions one by one. The observations made are tabulated below:
Answer the following questions based on the above observations:
(a) Which is the most active metal and why?
(b) What would be observed if B is added to a solution of copper (II) sulphate and why?
(c) Arrange the metal A, B, C and D in order of increasing reactivity.
(d) The container of which metal can be used to store both zinc sulphate solution and silver nitrate solution?
(e) Which of the above solutions can be easily stored in a container made up of any of these metals?
Answers
Answer:
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Explanation:
i) B is the most active metal as it displaces iron from its salt solution.
(ii) B will displace Cu from CuSO4 solution because B is more reactive than copper.
(iii) D < C <A < B
(iv) Container of metal D can be used to store both $ZnSO_{4}$ and $AgNO_{3}$ solutions, because it cannot displace Zn and Ag from their salt solutions.
(v) $ZnSO_{4}$ can be stored in a container made up of any of these metals.
(i) B metal is most active
(ii) B is more reactive than Cu, and hence will displace it from CuSO4
(iii) B is most reactive.
(iv) Metal D
(v) ZnSO4
Explanation:
From the given table, we infer:
(i) B is the most active metal as it displaces iron from Iron sulphate.
(ii) When B is added to CuSO4 solution, B will displace copper from copper sulphate as B is more reactive than copper.
(iii) B > A > C > D. B is the most reactive and D is least reactive.
(iv) Container of metal D can be used to store both ZnSO4 and AgNO solutions, as it does not react with both the solutions.
(v) ZnSO4 can be stored in a container made up of any of these metals.