Asked by Jared
10.0 g of KCl and 18.5 g of CaCl2 were dissolved in 500 mL of water. How many mL of 1.57 M AgNO3 solution would be required to precipitate all Cl- from the solution?
Answers
Answered by
Steve
first, identify the reactions:
KCl + AgNO3 = KNO3 + AgCl
CaCl2 + 2AgNO3 = Ca(NO3)2 + 2AgCl
convert grams to moles for KCl and CaCl2 to get total moles of Cl involved
Each mole of Cl requires one mole of AgNO3 to react.
divide that no. of moles by 1.57 to get liters of AgNO3 needed
KCl + AgNO3 = KNO3 + AgCl
CaCl2 + 2AgNO3 = Ca(NO3)2 + 2AgCl
convert grams to moles for KCl and CaCl2 to get total moles of Cl involved
Each mole of Cl requires one mole of AgNO3 to react.
divide that no. of moles by 1.57 to get liters of AgNO3 needed
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