${Ca}^{2 +}$ The following table shows the test students performed on four different aqueous solutions which are X, Y, Z and W. Based on the observation provided, identify the cations present.
Chemical test Observation Conclusion
To solution X, ammonium hydroxide is added in minimum quantity first and then excess. A dirty white precipitate is formed which dissolves in excess to form a clear solution. (i)
To solution Y, ammonium hydroxide is added in minimum quantity first and then excess. A pale blue precipitate is formed which dissolves in excess to form a clear inky blue solution. (ii)
To solution W, a small quantity of ammonium hydroxide is added first and then in excess. A white precipitate is formed which remain insoluble. (iii)
To a salt Z, Calcium hydroxide solution is added and then heated. A pungent smelling gas turning moist red litmus paper blue is obtained. (iv)

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Solution

Chemical Test-1: To solution X, ammonium hydroxide is added in minimum quantity first and then excess.
When Ammonium hydroxide $(N H_{4} O H)$ is added to zinc salt, a white precipitate of Zinc hydroxide $(Z n {(O H)}_{2})$ is formed which dissolves in excess Ammonium hydroxide and forms a clear solution. Thus, the cation present in zinc nitrate salt is ${Zn}^{2 +}$ ion.
The chemical reaction is as follows.
$\underset{Zinc nitrate}{Zn {({NO}_{3})}_{2} (s)} + \underset{Ammonium hydroxide}{2 {NH}_{4} OH (aq)} \to \underset{Zinc hydroxide}{Zn {(OH)}_{2} (s)} + \underset{Ammonium nitrate}{2 {NH}_{4} {NO}_{3} (s)} \underset{Zinc hydroxide}{Zn {(OH)}_{2} (s)} + \underset{Ammonium hydroxide}{4 {NH}_{4} OH (aq)} \to \underset{Tetraamine zinc hydroxide}{[Zn {({NH}_{3})}_{4}] {(OH)}_{2} (s)} + \underset{Water}{4 H_{2} O (l)}$

Chemical Test-2: To solution Y, ammonium hydroxide is added in minimum quantity first and then in excess.
When ammonium hydroxide is added to Copper sulphate $(C u S O_{4})$ solution, pale blue precipitate is formed which dissolves in excess ammonium hydroxide to form a clear inky blue solution.
Thus, the cation present in Copper sulphate solution salt is ${Cu}^{2 +}$ ion.
The chemical reaction is as follows.
$\underset{Copper sulphate}{{CuSO}_{4} (s)} + \underset{Ammonium hydroxide}{2 {NH}_{4} OH (aq)} \to \underset{Copper hydroxide}{Cu {(OH)}_{2} (s)} (Blue white ppt .) + \underset{Ammonium sulphate}{{({NH}_{4})}_{2} {SO}_{4} (s)} \underset{Copper hydroxide}{Cu {(OH)}_{2} (s)} + \underset{Ammonium hydroxide}{4 {NH}_{4} OH} \to \underset{Tetraamine copper hydroxide}{[Cu {({NH}_{3})}_{4}] {(OH)}_{2} (aq) (Prussian blue solution)} + \underset{Water}{4 H_{2} O (l)}$
Chemical Test-3:To solution W, a small quantity of sodium hydroxide solution is added and then in excess.
When Sodium hydroxide solution is added to Calcium nitrate $(C a {(N O_{3})}_{2})$ solution, a white precipitate is formed which remains insoluble in excess Sodium hydroxide.
Thus, the cation present in calcium nitrate salt is ${Ca}^{2 +}$ ion.
The chemical reaction is as follows.
$\underset{Sodium hydroxide}{2 NaOH (s)} + \underset{Calcium nitrate}{Ca {({NO}_{3})}_{2} (s)} \to \underset{Calcium hydroxide}{Ca {(OH)}_{2} (s)} + \underset{Sodium nitrate}{2 {NaNO}_{3} (s)}$

Chemical Test-4: To a salt Z, calcium hydroxide solution is added and then heated.
When Sodium hydroxide is added to Ammonium chloride salt, Ammonia gas $({NH}_{3})$ having a pungent-smellingthe is evolved.
Ammonia is alkaline in nature and thus, turns moist red litmus paper blue. Thus, the cation present is the ammonium ${NH}_{4}^{+}$ ion.
The chemical reaction is as follows.
$\underset{Ammonium chloride}{{NH}_{4} Cl (s)} + \underset{Sodium hydroxide}{NaOH (s)} \overset{∆}{\to} \underset{Sodium chloride}{NaCl (s)} + \underset{Ammonia gas}{{NH}_{3} (g)} + \underset{Water}{H_{2} O (l)}$
Chemical test
Observation
Conclusion
To solution X, ammonium hydroxide is added in minimum quantity first and then in excess.
A dirty white precipitate is formed which dissolves in excess to form a clear solution.

(i) ${Zn}^{2 +}$ cation
To solution Y, ammonium hydroxide is added in minimum quantity first and then in excess. A pale blue precipitate is formed which dissolves in excess to form a clear inky blue solution. (ii) ${Cu}^{2 +}$ cation
To solution W, a small quantity of sodium hydroxide solution is added and then in excess. A white precipitate is formed which remains insoluble. (iii) ${Ca}^{2 +}$ cation
To a salt Z, calcium hydroxide solution is added and then heated. A pungent smelling gas turning moist red litmus paper blue is obtained. (iv) ${NH}_{4}^{+}$ cation

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Similar questions

Q. (a) Sodium hydroxide solution is added to solution A. A white precipitate is formed which is insoluble in excess sodium hydroxide solution. Name the metal ion present in solution A.
(b) When ammonium hydroxide is added to solution B, a pale blue precipitate is formed. This pale blue precipitate dissolves in excess ammonium hydroxide to give an inky blue solution. Name the cation present in solution B. What is the probable colour of solution B?

Q. When ammonium hydroxide is added to solution B, a pale blue precipitate is formed. This pale blue precipitate dissolves in excess ammonium hydroxide to give an inky blue solution. What is the cation [positive ion] present in solution B? What is the probable colour of solution B?

Q. When ammonium hydroxide is added to solution B, a pale blue precipitate is formed. This pale blue precipitate dissolves in excess ammonium hydroxide giving an inky blue solution. What is the cation [positive ion] present in solution B? What is the probable colur of solution B.

Q. The following table shows the test a student performed on four different aqueous solution which are X, Y, Z and W. Based on the observations provided, identify the action present.

Chemical test	Observation	Conclusion
To solution X, ammonium hydroxide is added in minimum quantity first and then in excess.	A dirty white precipitate is formed which dissolves in excess to form a clear solution.
To solution Y ammonium hydroxide is added in minimum quantity first and then in excess.	A pale blue precipitate is formed which dissolves in excess to form a clear inky blue solution.
To solution W a small quantity of sodium hydroxide solution hydroxide solution is added and then in excess.	A white precipitate is formed which remains insoluble.
To a salt Z calcium hydroxide solution is added and then heated.	A pungent smelling gas turning moist red litmus paper blue is obtained.

The following table shows the tests a student performed on four different aqueous solutions which are X, Y, Z and W. Based on the observations provided, identify the cation present:

Chemical Test	Observations	Conclusions
To solution X, ammonium hydroxide is added in minimum quantity first and then in excess.	A dirty white precipitate is formed which dissolves in excess to form a clear solution.	(i)
To solution Y, ammonium hydroxide is added in minimum quantity first and then in excess.	A pale blue precipitate is formed which dissolves in excess to form a clear inky blue solution.	(ii)
To solution W, a small quantity of sodium hydroxide solution is added and then in excess.	A white precipitate is formed which remains insoluble.	(iii)
To a salt Z, calcium hydroxide solution is added and then heated.	A pungent smelling gas turning moist red litmus paper blue is obtained.	(iv)

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Chemical test	Observation	Conclusion
To solution X, ammonium hydroxide is added in minimum quantity first and then excess.	A dirty white precipitate is formed which dissolves in excess to form a clear solution.	(i)
To solution Y, ammonium hydroxide is added in minimum quantity first and then excess.	A pale blue precipitate is formed which dissolves in excess to form a clear inky blue solution.	(ii)
To solution W, a small quantity of ammonium hydroxide is added first and then in excess.	A white precipitate is formed which remain insoluble.	(iii)
To a salt Z, Calcium hydroxide solution is added and then heated.	A pungent smelling gas turning moist red litmus paper blue is obtained.	(iv)