Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride: Ag⁺(aq) + Cl^-(aq) → AgCl(s)
Silver chloride is virtually insoluble in water so that the reaction appears to go to completion.How many grams of solid NaCl must be added to 25.0 mL of 0.125 M AgNO₃ solution to completely precipitate the silver?

Question

Quizplus · Accepted Answer

To completely precipitate the silver ions, the moles of NaCl needed must equal the moles of AgNO₃. Calculate moles of AgNO₃: 0.125 M × 0.025 L = 0.003125 moles. The molar mass of NaCl is 58.44 g/mol. Therefore, 0.003125 moles × 58.44 g/mol = 0.183 g of NaCl is needed.

Silver Ions Can Be Precipitated from Aqueous Solutions by the Addition