Problem: You want to analyze a silver nitrate solution.You could add HCl(aq) to the solution to precipitate out AgCl(s). What volume of a 0.160 M HCl(aq) solution is needed to precipitate the silver ions from 16.0 mL of a 0.210 M AgNO3 solution?

FREE Expert Solution

We’re being asked to calculate the volume of a 0.160 M HCl(aq) solution is needed to precipitate the silver ions from 20.0 mL of a 0.210 M AgNO3 solution.


For this problem, we need to do the following steps:

Step 1: Write and balance a chemical equation for the given reaction.

Step 2: Determine the volume of HCl needed.



Step 1: Since HCl and AgNO3 are ionic compounds, they form ions when dissociating in water. 

The dissociation of the two compounds is as follows:

For KCl: Hydrogen has a charge of +1. This means Cl- has a charge of –1:

HCl(aq)  K+(aq) + Cl(aq)


For AgNO3: Silver has a charge of +1. The nitrate ion has a charge of –1:

AgNO3(aq)  Ag+(aq) + NO3(aq)


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Problem Details

You want to analyze a silver nitrate solution.

You could add HCl(aq) to the solution to precipitate out AgCl(s). What volume of a 0.160 M HCl(aq) solution is needed to precipitate the silver ions from 16.0 mL of a 0.210 M AgNO3 solution?

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Our tutors have indicated that to solve this problem you will need to apply the Solution Stoichiometry concept. You can view video lessons to learn Solution Stoichiometry. Or if you need more Solution Stoichiometry practice, you can also practice Solution Stoichiometry practice problems.