Ksp of lead iodide

1/ The molar solubility of PbI2 is 1.5 x 10-3 M. a/ What is the molar concentration of iodide ion in a saturated PbI2 solution? b/ Determine the solubility constant, Ksp, for lead(II) iodide 2/ Calculate the molar solubility of PBI2 in the presence of 0.10 M NaI 3/ Compare the molar solubility given in problem 1 and the molar solubility ... The solubility-product constant for lead iodide (PbI2 ⇔ Pb2 + + 2I-) is Ksp = 7.1 × 10 − 9. Calculate the molar solubility of lead iodide in otherwise pure water. Calculate the molar solubility of lead iodide (PbI2 ⇔ Pb2 + + 2I-, Ksp = 7.1 × 10 − 9) in a solution containing 0.10 M potassium iodide (KI), a very soluble salt. 0.97 ml of 0.001 M AgNO3(aq) is required to just precipitate the iodide ion from 0.80 ml of the saturated lead iodide solution. With this information, we can find the Ksp and solubility of lead iodide. NOTE: Ag+(aq) + I-(aq) = AgI(s), Ksp = [Ag+][I-] = 8.3 x 10-17 Ksp will then be stated as a range of values at room temperature, and the precipitate test tubes will be heated until the precipitate is dissolved so that Ksp may be observed and determined at different levels. In this experiment various solutions of lead nitrate and potassium iodide were mixed at a number of different dilutions. Solution Ksp = [Pb2+][I-]2 7.1x10-9 = s x (2s)2 7.1x10-9 = 4s3 s = 1.2x10-3 M If we compare the molar solubilities of PbSO4 and PbI2 we find that the solubility of lead iodide is larger than that of lead sulfate although lead iodide has smaller ksp.

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Ksp will then be stated as a range of values at room temperature, and the precipitate test tubes will be heated until the precipitate is dissolved so that Ksp may be observed and determined at different levels. In this experiment various solutions of lead nitrate and potassium iodide were mixed at a number of different dilutions.

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Jul 27, 2016 · 00:07 Solubility of lead (II) iodide 01:24 Kₛₚ expression for PbI₂ 04:08 Let x = [Pb⁺² (aq)] 04:58 Let 2x = [I⁻ (aq)], charge balance 05:29 Substitute x and 2x into Kₛₚ expression ... Lead (II) iodide precipitates when potassium iodide is mixed with lead (II) nitrate. Graphic: Wikimedia Commons user PRHaney. Slide 2. Ksp Values for Some Salts at 25 C. Slide 3. Solving Solubility Problems. For the salt AgI at 25 C, Ksp = 1.5 x 10-16. AgI(s) Ag+(aq) + I-(aq) O. O +x +x. x. x. 1.5 x 10-16 = x2. x = solubility of AgI in mol/L ...


3. The Ksp for lead iodide (PbI2) is 1.4x10-8. Calculate the solubility of lead iodide in a. Water PbI2 (s) ==> PbI2(aq) ==> Pb 2+ + 2I-S S 2S Ksp = S(2S) 2 = 4S3 = 1.4 x10-8 S=0.0015 moles/liter b. 0.1M Pb(NO3)2 PbI2 (s) ==> PbI2(aq) ==>Pb 2+ + 2I-Initial: 0.1M OM Eq. 0.1 +x 2x Ksp = 1.4 x 10 – potassium iodide and lead nitrate – sodium sulfate and barium nitrate (ACSCH065) derive equilibrium expressions for saturated solutions in terms of Ksp and calculate the solubility of an ionic substance from its Ksp value predict the formation of a precipitate given the standard reference values for Ksp

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