On the basis of the reactivity series of metals, predict how these metals will react with each of the following salt solutions:

Metals: magnesium, zinc, copper, iron, and potassium

Salt solutions: magnesium sulphate, zinc sulphate, copper sulphate, iron sulphate,and potassium sulphate

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Solution

Magnesium will replace metals from Copper sulfate, Zinc sulfate, and Iron sulfate.
$M g + {C u S O}_{4} ⟶ M g {S O}_{4} + C u$
$M g + Z n S O_{4} ⟶ M g S O_{4} + Z n$
$M g + F e S O_{4} ⟶ M g S O_{4} + F e$
$M g + K_{2} S O_{4} ⟶ N o R e a c t i o n$
$M g + M g S O_{4} ⟶ N o R e a c t i o n$
$M g$ + $C u S O_{4}$ $⟶$ $M g S O_{4}$ + $C u$

Zinc will replace metals from Copper sulfate and Iron sulfate.
$Z n + C u S O_{4} ⟶ Z n S O_{4} + C u$
$Z n + F e S O_{4} ⟶ Z n S O_{4} + F e$
$Z n + M g S O_{4} ⟶ N o R e a c t i o n$
$Z n + Z n S O_{4} ⟶ N o R e a c t i o n$
$Z n + K_{2} S O_{4} ⟶ N o R e a c t i o n$

Copper is less reactive and will not replace metals from their solution.
$C u + C u S O_{4} ⟶ N o R e a c t i o n$
$C u + F e S O_{4} ⟶ N o R e a c t i o n$
$C u + M g S O_{4} ⟶ N o R e a c t i o n$
$C u + Z n S O_{4} ⟶ N o R e a c t i o n$
$C u + K_{2} S O_{4} ⟶ N o R e a c t i o n$

Iron will replace Copper sulfate solution.
$F e + C u S O_{4} ⟶ F e S O_{4} + C u$
$F e + F e S O_{4} ⟶ N o R e a c t i o n$
$F e + M g S O_{4} ⟶ N o R e a c t i o n$
$F e + Z n S O_{4} ⟶ N o R e a c t i o n$
$F e + K_{2} S O_{4} ⟶ N o R e a c t i o n$

Potassium is the most reactive and will replace all metals from their solution
$2 K + C u S O_{4} ⟶ K_{2} S O_{4} + C u$
$2 K + M g S O_{4} ⟶ K_{2} S O_{4} + M g$
$2 K + Z n S O_{4} ⟶ K_{2} S O_{4} + Z n$
$2 K + F e S O_{4} ⟶ K_{2} S O_{4} + F e$
$2 K + K_{2} S O_{4} ⟶ N o R e a c t i o n$

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Similar questions

Which of the following pairs cannot undergo displacement reaction?

(a) iron sulphate solution and magnesium

(b) zinc sulphate solution and iron

(d) silver nitrate solution and copper

Zinc granules were added to zinc sulphate, copper sulphate, aluminium sulphate and iron sulphate solutions as shown below. You would observe the deposition of metal on zinc in beakers:

Q. Choose the reactions which are not feasible.
I. Iron + Zinc sulphate

\to

Iron sulphate + Zinc
II. Magnesium + Silver nitrate

\to

Magnesium nitrate + Silver
III. Copper + dil. sulphuric acid

\to

Copper sulphate +

H_{2}

IV. Zinc + Ferrous sulphate

\to

Iron + Zinc sulphate

Q. Write the formula of the following compounds.
calcium hydroxide, copper chloride, iron sulphate, sodium carbonate, copper nitrate, copper oxide, lead sulphide, magnesium chloride, zinc sulphate, potassium hydroxide.

Q. Assertion :Zinc can easily displace copper on reacting with a solution of copper sulphate Reason: Zinc is more reactive metal as compared to copper therefore zinc displaces copper from coper sulphate solution.

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On the basis of the reactivity series of metals, predict how these metals will react with each of the following salt solutions: Metals: magnesium, zinc, copper, iron, and potassium Salt solutions: magnesium sulphate, zinc sulphate, copper sulphate, iron sulphate,and potassium sulphate

On the basis of the reactivity series of metals, predict how these metals will react with each of the following salt solutions:

Metals: magnesium, zinc, copper, iron, and potassium

Salt solutions: magnesium sulphate, zinc sulphate, copper sulphate, iron sulphate,and potassium sulphate