Assertion :As such the group reagent to separate 1st group cations is hydrochloric acid usually used at a concentration of 12 M. Reason: Concentrated $H C l$ must not be used because it forms a soluble complex ion of $P b C l_{4}$ with ${P b}^{2 +}$ .

Both Assertion and Reason are correct and Reason is the correct explanation for Assertion

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Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion

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Assertion is correct but Reason is incorrect

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Both Assertion and Reason are incorrect

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Solution

The correct option is A Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
An assertion is True: Group I metals are precipitated with the use of dilute hydrochloric acid rather than a dilute one.
${A g}^{+} + {C l}^{-} ⇌ A g C l (w h i t e p r e c i p i t a t e)$
${P b}^{2 +} + 2 {C l}^{-} ⇌ P b {C l}_{2} (w h i t e c r y s t a l l i n e p r e c i p i t a t e)$
The reason is the true and correct explanation of Assertion: The dilute hydrochloric acid is enough to precipitate the cations of the group I as insoluble chlorides. Using concentrated hydrochloric acid allows the formation of soluble chlorine complex in our salts. As the concentration of $C l^{-}$ raises the soluble complexes to form. These complexes are soluble because they are charged molecule and therefore effectively solvated by water.
Hence, the answer is $A$ .

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Assertion :As such the group reagent to separate 1st group cations is hydrochloric acid usually used at a concentration of 12 M. Reason: Concentrated HCl must not be used because it forms a soluble complex ion of PbCl4 with Pb2+.

Assertion :As such the group reagent to separate 1st group cations is hydrochloric acid usually used at a concentration of 12 M. Reason: Concentrated $H C l$ must not be used because it forms a soluble complex ion of $P b C l_{4}$ with ${P b}^{2 +}$ .