What is the approximate mass of the precipitate formed when 50 mL of 16.9\% solution of AgNO _3 is mixed with 50 mL of 7.45\% KCl solution? (Molar mass of AgNO _3 = 169 g/mol, KCl = 74.5 g/mol, AgCl = 143.3 g/mol)

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Correct answer: B. 7 g

Mass of AgNO _3 in 50 mL of 16.9\% (w/v) solution = 16.9 100 50 = 8.45 g Moles of AgNO _3 = 8.45 169 = 0.05 mol Mass of KCl in 50 mL of 7.45\% (w/v) solution = 7.45 100 50 = 3.725 g Moles of KCl = 3.725 74.5 = 0.05 mol The balanced chemical equation is: AgNO _3 + KCl AgCl + KNO _3 Since 1 mole of AgNO _3 reacts with 1 mole of KCl to give 1 mole of AgCl, 0.05 mol of AgNO _3 will react completely with 0.05 mol of KCl to form 0.05 mol of AgCl. Mass of AgCl precipitate = 0.05 143.3 = 7.165 g 7 g Answer: 7 g

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