- Given Mw Aacl 143 3212 G Mol Mw Pbcl2 278 1054 G Mol Mw Ag2so4 311 799 G Mol Aaci Mass 4 999819 Ag 0 000013303 1 (47.46 KiB) Viewed 93 times
Given: MW AaCl = 143.3212 g/mol MW PbCl2 = 278.1054 g/mol MW Ag2SO4 = 311.799 g/mol Aaci Mass 4.999819 [Ag*] 0.000013303
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answerhappygod
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Given: MW AaCl = 143.3212 g/mol MW PbCl2 = 278.1054 g/mol MW Ag2SO4 = 311.799 g/mol Aaci Mass 4.999819 [Ag*] 0.000013303
Given: MW AaCl = 143.3212 g/mol MW PbCl2 = 278.1054 g/mol MW Ag2SO4 = 311.799 g/mol Aaci Mass 4.999819 [Ag*] 0.0000133038 [CH] 0.0000133038 PbCl2 Mass 0.460227g [Pb2+] 0.0143013 [CH] 0.0286026 Ag2SO4 Mass 4.525369 [Ag*] 0.0304380 [SO42-10.0152190 A. Write solubility product constant expression and calculate numerical value (Ksp) of each ionic compound I. AgCI II. PbCl2 III. Ag2SO4 B. Use ICE Method for each addition of common ions Common ion CF (AgCl and PbCl2) » Common ion Ag* (AaCl and Ag2SO4) C. Looking at your solubility results, did the solubility increase, decrease, or stay about the same in the original solutions? Does this confirm the common ion effect? If not, can you explain why it does not?