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CHM 101 CHM 101 Past Questions Objective Question
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Question

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 Ag⁺ solution to completely precipitate the silver? [Ag=108; Cl=35.5]
Options
A 9.15 × 10⁻³
B 1.57 × 10⁻¹
C 0.535
Correct Answer
D 0.157
Correct Answer

Option C is the correct answer.

Detailed Explanation

Moles Ag⁺ = 0.0250 L × 0.366 M = 0.00915 mol. Reaction is 1:1, so moles NaCl needed = 0.00915 mol. Molar mass NaCl = 58.44 g/mol. Mass = 0.00915 × 58.44 = 0.535 g.

Hint

Use the stoichiometry of the precipitation reaction: 1:1 mole ratio between Ag⁺ and Cl⁻.

Question Info

Course: CHM 101
Topic: CHM 101 Past Questions
Type: Objective
Difficulty: Not specified
Question 1153 of 1872
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