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00 g mixture of NaCl and CaCl2, which was completely dissolved in an aqueous solution, is treated with excess AgNO3 to precipitate all of the Cl-...

A 1.00 g mixture of NaCl and CaCl2, which was completely dissolved in an aqueous solution, is treated with excess AgNO3 to precipitate all of the Cl- ions present in solution as AgCl. A mass of 3.02 g of AgNO3 was consumed in the precipitation process. What is the percentage by weight of NaCl in the original mixture?

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Solution@011212 Solubility product.docx

Solution
Moles of AgNO3 = 3.02g/ 169.87 g/mol = 0.01778
Let us assume X gm of NaCl and (1-X) gm of CaCl2 reacts with 0.01778 mol of AgNO3
Moles of NaCl = Xgm / 58.44 gm/mol
Moles of CaCl2 = (1-X)gm...

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