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The Solubility Product of PbCl2 from Electrochemical Measurements
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Abstract
A new experiment suited for an undergraduate physical chemistry laboratory is presented. The students obtain the solubility product, Ksp, of PbCl2 at various temperatures from practically simultaneous emf measurements on two electrochemical cells. One half-cell is common to both cells. Each of the three half-cells is enclosed in a jacket of circulating water where the temperatures are controlled to better than ±0.05 K and measured to ±0.1 K. A 1 M KNO3 salt bridge is used in the two cells. At each temperature the difference between the two cells' emf values is directly related to the concentration of the Cl- ions in the saturated PbCl2 solution, which in turn yields the solubility product of PbCl2. The variation of ln Kspwith T-1 yields the standard enthalpy and entropy of the solubility equilibrium of PbCl2(s). Use of two cells to cancel out the temperature dependencies of the standard reference electrodes and junction potentials across the salt bridge is novel. This experiment is not found in physical chemistry laboratory textbooks. It works well and can be completed by the students within three hours.
Keywords (Audience):
Second-Year UndergraduateKeywords (Domain):
Laboratory InstructionKeywords (Pedagogy):
Hands-On Learning / ManipulativesKeywords (Subject):
ElectrochemistryCiting Articles
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This article has been cited by 4 ACS Journal articles (4 most recent appear below).
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- Received: August 03, 2009
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