A 4.2 g mixture of the solid salts Na2S04 (molar mass = 142.04 g/mol) and Pb(NO3)2 (molar mass =331.20 g/mol) forms an aqueous solution with the precipitation of PbS04 (molar mass =303.26 g/mol). The precipitate was filtered and dried, and its mass was determined to be 3.9 g. What is the total mass in (g) of the reacted Na2s04 and Pb(NO3)2?
A 4.2 g mixture of the solid salts Na2S04 (molar mass = 142.04 g/mol) and Pb(NO3)2 (molar mass =331.20 g/mol) forms an aqueous solution with the precipitation of PbS04 (molar mass =303.26 g/mol). The precipitate was filtered and dried, and its mass was determined to be 3.9 g. What is the total mass in (g) of the reacted Na2s04 and Pb(NO3)2?
Chemistry by OpenStax (2015-05-04)
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Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter19: Transition Metals And Coordination Chemistry
Section: Chapter Questions
Problem 14E: A 2.5624-g sample of a pure solid alkali metal chloride is dissolved in water and treated with...
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