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)

Step-by-step solution

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