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Ionic Equilibrum question

2011 · Q76
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Ionic Equilibrum question

2011 · Q76

NEETChemistryIonic EquilibrumMCQ+4 / −1
In qualitative analysis, the metals of group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains Ag+ and pb2+ at a concentration of 0.10 M. Aqueous HCl is added to this solution until the Cl−-− concentration is 0.10 M. What will the concentrations of Ag+ and Pb2+ be at equilibrium ?

(Ksp for AgCl = 1.8 ×\times× 10−-−10, Ksp for PbCl2 = 1.7 ×\times× 10−-−5)
  1. A
    [Ag+] = 1.8 ×\times× 10−-−7 M, [Pb2+] = 1.7 ×\times× 10−-−6 M
  2. B
    [Ag+] = 1.8 ×\times× 10−-−11 M, [Pb2+] = 8.5 ×\times× 10−-−5 M
  3. C
    [Ag+] = 1.8 ×\times× 10−-−9 M, [Pb2+] = 1.7 ×\times× 10−-−3 M
  4. D
    [Ag+] = 1.8 ×\times× 10−-−11 M, [Pb2+] = 1.7 ×\times× 10−-−4 M
View written solutionFree

Correct answer: C

Ksp[AgCl] = [Ag+][Cl-]

⇒\Rightarrow⇒ [Ag+] = 1.8×10−1010−1{{1.8 \times {{10}^{ - 10}}} \over {{{10}^{ - 1}}}}10−11.8×10−10​ = 1.8 ×\times× 10−-−9 M

Ksp[PbCl2] = [Pb2+][Cl-]2

⇒\Rightarrow⇒ [Pb2+] = 1.7×10−510−1×10−1{{1.7 \times {{10}^{ - 5}}} \over {{{10}^{ - 1}} \times {{10}^{ - 1}}}}10−1×10−11.7×10−5​ = 1.7 ×\times× 10−-−3 M

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