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 0.175 M solution to completely precipitate the silver? A) 4.38 × g B) 7.49 × 10^-5 g C) 0.256 g D) 0.0749 g E) 1.34 × 10⁴ g

Question

Quizplus · Accepted Answer

First, we need to determine the amount of Ag+ ions present in the solution:

0.175 mol/L x 0.025 L = 0.004375 mol Ag+

According to the balanced equation, 1 mole of Ag+ requires 1 mole of Cl- to precipitate. Therefore, we need to add 0.004375 moles of Cl- to the solution.

Next, we can use the molar mass of NaCl to determine the mass required to provide 0.004375 moles of Cl-:

0.004375 mol Cl- x 1 mol NaCl / 1 mol Cl- x 58.44 g/mol NaCl = 0.256 g NaCl

Therefore, the answer is C) 0.256 g.

Silver Ions Can Be Precipitated from Aqueous Solutions by the Addition