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The solubility of PbCl2 increases with an increase in temperature. Is the dissolution of PbCl2 (s) in water exothermic or endothermic? Explain

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Robert Kubara
Robert KubaraLv10
20 Nov 2020

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Related questions

The Ksp for PbCl2 = 1.7x10^-5

a. Calculate the molar solubility of PbCl2 in pure water.

b. Calculate the molar solubility of PbCl2 in a solution that is 0.1M of the soluble salt MgCl2.


Calculate the molar solubility, S, of PbCl2 (Ksp, at 25ºC is 1.7 x 10-5) (Consider only the equilibria associated with the dissolution of PbCl2, i.e., ignore the reaction of Pb2+ with H2O).

a) In pure water

b) In 0.10 M NaCl. For this problem, assume activity coefficients are equal to 1.

c) In 2.0 x 10-6 M Pb(NO3)2 For this problem, assume activity coefficients are equal to 1.

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