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)
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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What scientific concept do you need to know in order to solve this problem?
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