Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride: (aq) + (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 mol L^-1 (aq) solution to completely precipitate the silver?

Question

Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride:

(aq) +

(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 mol L^-1

(aq) solution to completely precipitate the silver?

Quizplus · Accepted Answer

First, we need to determine how many moles of Ag+ are present in 25.0 mL of the solution:

0.366 mol/L x 0.0250 L = 0.00915 mol Ag+

According to the balanced equation, 1 mole of Ag+ reacts with 1 mole of Cl-, so we need 0.00915 mol of Cl- to completely precipitate the silver ions.

Since NaCl dissociates into Na+ and Cl-, we only need to consider the moles of Cl- provided by NaCl. The molar mass of NaCl is 58.44 g/mol, so we can calculate the mass of NaCl required:

0.00915 mol Cl- x 1 mol NaCl/1 mol Cl- x 58.44 g/mol = 0.535 g NaCl

Therefore, the correct answer is (C).

Silver Ions Can Be Precipitated from Aqueous Solutions by the Addition