Ba(CN) 2 = BaI 2 = 1.0 x 10 -10 M Ba(CN) 2 ---------> Ba 2+ + 2CN - 1 mole of Ba

Question

Ba(CN)2 = BaI2 = 1.0 x 10-10M

Ba(CN)2 ---------> Ba2+ + 2CN-

1 mole of Ba(CN)2 produces 1 mole of Ba2+ and 2 mole of CN- ions

[Ba2+] = 1.0 x 10-10 M [CN-] = 2.0 x 10-10M

BaI2 ---------> Ba2+ + 2I-

1 mole of BaI2 produces 1 mole of Ba2+ and 2 mole of I- ions

[Ba2+] = 1.0 x 10-10 M [I-] = 2.0 x 10-10M

Concentration of AgNO3 = moles/ vol in litres = 3.5 x 10-9 /0.01 = 3.5 x 10-7M

AgNO3 ---------> Ag+ + NO3-

[Ag+] = 3.5 x 10-7M   [NO3-] = 3.5 x 10-7M

Chances of forming AgCN precipitate

[Ag+][CN-] =3.5 x 10-7 x 2.0 x 10-10M = 7.0 x 10-17 > given Ksp of AgCN (6.0 x 10-17)

Hence, AgCN precipitate is formed in the solution

Chances of forming AgI precipitate

[Ag+][I-] =3.5 x 10-7 x 2.0 x 10-10M = 7.0 x 10-17 < given Ksp of AgI (8.5 x 10-17)

Hence, AgI precipitate is not formed in the solution

The correct answer is 'b'

Explanation / Answer

Consider a 10.0 mL solution containing 1.0 x 10-10 M each of Ba(CN)2 and Bal2. If 3.5 x 10° mol of AgNO, () is added to this solution, will any precipitate(s) form? If yes, what compound(s) will precipitate? Useful data: All barium salts and nitrate salts in this ques tion fully dissociate in water Kg for AgCN = 6.0 x 10-17 Ksp for AgI -8.5 × 10-17 No precipitates will be formed. Only AgCNwill precipitate. correct an swer Only AgI will precipitate. Both AgCN and AgI will precipitate. a. c. d.

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