Assume that a given solution contains Ag^+ or Ba^2+ or a mixture of both. A reas

Question

Assume that a given solution contains Ag^+ or Ba^2+ or a mixture of both. A reasonable method for doing a qualitative analysis on this solution might be sketched out as follows (Remember || means a precipitate forms and | means a solution remains. It is always assumed that solutions are separated from precipitates before adding the next reagent.) What is the precipitate formed at X in the above scheme? What is the identity of cation at Y in the above scheme? What are two other solutions that could be used in the above scheme rather than Na_2SO_4? Explain

Explanation / Answer

The solution contain

Ag+ and Ba+2

The solution added is Na2SO4 '

a) It will precipitate out Ba+2 ion as BaSO4 So X : BaSO4

b) the cation in Y = Ag+

c) the two other solutions which can be used here are

NaCl : It will precipitate out Ag+ as AgCl while BaCl2 is soluble in water

NaI : it wil precipitate out Ag+ as pale yellow AgCl while BaI2 is soluble in water

TIt

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