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 0.149 M AgNO₃ solution to completely precipitate the silver?

Question

Quizplus · Accepted Answer

To find the grams of NaCl needed, first calculate the moles of AgNO₃ in the solution: 0.149 M × 0.025 L = 0.003725 moles. Since the reaction is 1:1, 0.003725 moles of NaCl are needed. The molar mass of NaCl is 58.44 g/mol, so 0.003725 moles × 58.44 g/mol = 0.218 grams of NaCl.

Silver Ions Can Be Precipitated from Aqueous Solutions by the Addition