We’re being asked to calculate the mass of KCl required to react with 20.0 mL of 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 mass of KCl needed.
Step 1: Since KCl and AgNO3 are ionic compounds, they form ions when dissociating in water.
The dissociation of the two compounds is as follows:
For KCl: Potassium is from Group 1 so it has a charge of +1. This means Cl- has a charge of –1:
KCl(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 solid KCl to the solution to precipitate out AgCl(s). What mass of KCl is needed to precipitate the silver ions from 20.0 mL of 0.210 M AgNO3 solution?
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What scientific concept do you need to know in order to solve this problem?
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.