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Chemistry problem... help please???

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Calculate the molar solubility of AgCl in a solution made by dissolving 10.0 g of CaCl2 in 5.50 L of solution.

Ksp AgCl = 1.6*10^-10

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  1. Ksp = 1.6x10^-10 = [Ag+][Cl-]

    [Cl-] = (10.0 g CaCl2/ 111 g/mol)*2/5.50 liter = 0.0328 M

    1.6x10^-10 = [Ag+]*0.0328

    [Ag+] = 4.9x10^-9 moles/liter

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