Determine if a precipitate of PbCl2 will form 5.0 mL of 0.02 M KCl is mixed with 5.5 mL of 0.02 M Pb(NO3)2? Ksp is 1.6 × 10^-5?
回答 (2)
2016-06-16 5:53 pm
PbCl₂(s) ⇌ Pb²⁺(aq) + 2Cl⁻(aq)
After the two solutions are mixed :
[Pb²⁺] = (0.02 M) × [5.5/(5.0 + 5.5)] = (0.11/10.5) M
[Cl⁻] = (0.02 M) × [5.0/(5.0 + 5.5)] = (0.10/10.5) M
Q = [Pb²⁺] [Cl⁻]² = (0.11/10.5) ×(0.10/10.5)² = 9.5 × 10⁻⁷ < Ksp
Hence, no precipitate of PbCl₂ is formed.
After the two solutions are mixed :
[Pb²⁺] = (0.02 M) × [5.5/(5.0 + 5.5)] = (0.11/10.5) M
[Cl⁻] = (0.02 M) × [5.0/(5.0 + 5.5)] = (0.10/10.5) M
Q = [Pb²⁺] [Cl⁻]² = (0.11/10.5) ×(0.10/10.5)² = 9.5 × 10⁻⁷ < Ksp
Hence, no precipitate of PbCl₂ is formed.
2016-06-16 5:33 pm
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