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 0.366 M AgNO₃ solution to completely precipitate the silver?

Question

Quizplus · Accepted Answer

1. Write the balanced chemical equation for the reaction:

AgNO3 (aq)+ NaCl (aq) → AgCl (s) + NaNO3 (aq)

2. Identify the number of moles of AgNO3:

Moles of AgNO3 = (25.0 mL) x (0.366 mol/L) x (1 L/1000 mL) = 0.00915 mol

3. Determine the limiting reactant based on stoichiometry. The coefficients of AgNO3 and NaCl in the balanced equation are both 1, so the moles of AgNO3 and NaCl required for complete reaction are equal.

4. Calculate the mass of NaCl required:

Mass of NaCl = (0.00915 mol) x (1 mol NaCl / 1 mol AgNO3) x (58.44 g NaCl / 1 mol NaCl) = 0.535 g

Therefore, the answer is C, 0.535.

Silver Ions Can Be Precipitated from Aqueous Solutions by the Addition