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Post-Lab Questions: In a different experiment, a precipitation reaction was used to determine the solubility and solubility product constant of lead(II) chloride. The equilibrium equation is: PbCl2(s) Pb²+ (aq) + 2 Cl(aq) The dissolved chloride in the filtered solution was quantitatively precipitated as AgCl by the addition of excess AgNO3 solution. The solid AgCl was filtered from solution, dried, and weighted. The following data were obtained for three samples of the filtered, saturated solution. Temperature of filtered saturated solution (°C) Volume of PbCl2 saturated solution analyzed (mL) Mass of dry AgCl (g) Calculate the following: Number of moles of: AgCl(s) Cl(aq) Pb²+ (aq) 1 20.2 25.00 0.2543 Trial 2 20.4 22.00 0.2276 3 20.1 20.10 0.2051

Post-Lab Questions: In a different experiment, a precipitation reaction was used to determine the solubility and solubility product constant of lead(II) chloride. The equilibrium equation is: PbCl2(s) Pb²+ (aq) + 2 Cl(aq) The dissolved chloride in the filtered solution was quantitatively precipitated as AgCl by the addition of excess AgNO3 solution. The solid AgCl was filtered from solution, dried, and weighted. The following data were obtained for three samples of the filtered, saturated solution. Temperature of filtered saturated solution (°C) Volume of PbCl2 saturated solution analyzed (mL) Mass of dry AgCl (g) Calculate the following: Number of moles of: AgCl(s) Cl(aq) Pb²+ (aq) 1 20.2 25.00 0.2543 Trial 2 20.4 22.00 0.2276 3 20.1 20.10 0.2051

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter17: Solubility And Complex-ion Equilibria
Section: Chapter Questions
Problem 17.117QP
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can you help me calculate the number of moles for the first three substances? 

Post-Lab Questions: In a different experiment, a precipitation reaction was used to determine the solubility and solubility product constant of lead(II) chloride. The equilibrium equation is: PbCl2(s) → Pb2+ (aq) + 2 Cl(aq) The dissolved chloride in the filtered solution was quantitatively precipitated as AgCl by the addition of excess AgNO3 solution. The solid AgCl was filtered from solution, dried, and weighted. The following data were obtained for three samples of the filtered, saturated solution. Temperature of filtered saturated solution (°C) Volume of PbCl2 saturated solution analyzed (mL) Mass of dry AgCl (g) Calculate the following: Number of moles of: AgCl(s) 421 Cl(aq) 2+ Pb²+ (aq) [Cl] in PbCl2 solution (mol/L) [Pb²+] in PbCl2 solution (mol/L) Ksp Average Ksp Solubility of PbCl2, in g per 100 mL 1 20.2 25.00 0.2543 Trial 2 20.4 22.00 0.2276 3 20.1 20.10 0.2051 (literature value is 0.994 g/100 mL at 20 °C)
Transcribed Image Text:Post-Lab Questions: In a different experiment, a precipitation reaction was used to determine the solubility and solubility product constant of lead(II) chloride. The equilibrium equation is: PbCl2(s) → Pb2+ (aq) + 2 Cl(aq) The dissolved chloride in the filtered solution was quantitatively precipitated as AgCl by the addition of excess AgNO3 solution. The solid AgCl was filtered from solution, dried, and weighted. The following data were obtained for three samples of the filtered, saturated solution. Temperature of filtered saturated solution (°C) Volume of PbCl2 saturated solution analyzed (mL) Mass of dry AgCl (g) Calculate the following: Number of moles of: AgCl(s) 421 Cl(aq) 2+ Pb²+ (aq) [Cl] in PbCl2 solution (mol/L) [Pb²+] in PbCl2 solution (mol/L) Ksp Average Ksp Solubility of PbCl2, in g per 100 mL 1 20.2 25.00 0.2543 Trial 2 20.4 22.00 0.2276 3 20.1 20.10 0.2051 (literature value is 0.994 g/100 mL at 20 °C)
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