Problem: Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride per the following net ionic equation:                 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 solutions to completely precipitate the silver?A. 9.81B. 6.37 x 10-5C. 0.218D. 0.102E. 0.633

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FREE Expert Solution

We are asked how many grams of solid NaCl must be added to 25.0 mL of 0.149 M AgNO3 solutions to completely precipitate the silver.


Step 1. Calculate the moles of Ag+ (aq) in AgNO3. 

Dissociation reaction: AgNO3 →  Ag+ (aq) + NO3 (aq) 

This means : 1 mole AgNO3 → 1 mole Ag+ (aq)

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Problem Details

Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride per the following net ionic equation: 

                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 solutions to completely precipitate the silver?

A. 9.81
B. 6.37 x 10-5
C. 0.218
D. 0.102
E. 0.633