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Q14. A solution is 0.025 M in Pb2+. What minimum concentration of Cl is required to begin to precipitate PbCl2? For PbCl2, Ksp = 1.17 x 10-5. a) 1.17 X 10 M b) 0.0108 M c) 0.0216 M d) 5.41 X 10M

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A solution is prepared by mixing 50.0 mL of 0.30 M Pb(NO₃)₂ with 50.0 mL of 1.4 M KCl. Calculate the concentrations of Pb²⁺ and Cl ^- at equilibrium. K_sp for PbCl₂(s) is 1.6 â 10^-5.
Pb²⁺

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1) calculate the activity coefficient and the activity of SO42- in each of the following solutions
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2) the equilibrium constant for the dissociation of PbCl2 into it's ions is 1.7x10^-5. calculate the following:
a) the concentration of Pb2+ in a solution where such an equilibrium has been established
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c)percentage decrease in the concentration of Pb2+ caused by the addition of the Cl-

what is the molar solubility of pbcl2 in a solution containing 0.020 M cl-(aq)? the ksp for pbcl2 is 1.6*10^-5

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Q14. A solution is 0.025 M in Pb2+. What minimum concentration of Cl is required to begin to precipitate PbCl2? For PbCl2, Ksp = 1.17 x 10-5. a) 1.17 X 10 M b) 0.0108 M c) 0.0216 M d) 5.41 X 10M

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