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Solubility Product
Sep 19, 1996 Name ____________________________
1. 0.5143 g of Ag2CrO4 is placed in 104.3 mL of water. Ksp of silver chromate is 1.2x10-12.
A. Write the dissociation reaction for silver chromate, then write the Ksp expression for silver chromate.
B. Calculate the concentrations of Ag+ and of CrO42-.
2. A solution known to have [Ag+] = 0.045 M has a pile of silver chromate in the bottom of it. Compute the concentration of chromate [CrO42-] in the solution.
3. 100.0 mL of 0.100 M AgNO3 and 50.0 mL of 0.300 M NaCl are mixed together. Complete the following Initial/Final Spreadsheet, finally calculating the concentrations of all species in solution after reaction has taken place. Ksp AgCl is 1.82x10-10.
Balanced Reaction: _________________________________________________
millimoles
Ag+
|
millimoles
NO3-
|
millimoles
Na+
|
millimoles
Cl-
|
millimoles
AgCl(s)
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Volumes
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| Initial
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Final
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Molar
Conc.
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