To measure the amount of chlorine in a well-boring fluid, an analytical chemist adds 0.210M silver nitrate (AgNO,) solution to a 49.0 g sample of the fluid and collects the solid silver chloride (AgCl) product. When no more AgCl is produced, she filters, washes and weighs it, and finds that 2.21 g has been produced. The balanced chemical equation for the reaction is: CI (aq) + AgNO, (aq) → AGCI (s) + NO, (aq) .

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# Solving a Redox Titration Problem

To measure the amount of chlorine in a well-boring fluid, an analytical chemist adds 0.210M silver nitrate (\( \text{AgNO}_3 \)) solution to a 49.0 g sample of the fluid and collects the solid silver chloride (\( \text{AgCl} \)) product. When no more \( \text{AgCl} \) is produced, she filters, washes and weighs it, and finds that 2.21 g has been produced.

The balanced chemical equation for the reaction is:
\[
\text{Cl}^-_{(aq)} + \text{AgNO}_3 (aq) \rightarrow \text{AgCl} (s) + \text{NO}_3^- (aq)
\]

---

**Question:** What kind of reaction is this?

- [ ] precipitation
- [ ] acid-base
- [ ] redox

**Instructions:**

1. **If you said this was a _precipitation_ reaction, enter the chemical formula of the precipitate.**

2. **If you said this was an _acid-base_ reaction, enter the chemical formula of the reactant that is acting as the base.**

3. **If you said this was a _redox_ reaction, enter the chemical symbol of the element that is oxidized.**

4. **Calculate the mass percent of Cl in the sample. Be sure your answer has 3 significant digits.**

---

**Interface:** 

- There are options to select the type of reaction and fields for input based on the choice made. 
- The solution can be checked using the "Check" button. 
- Additional help can be accessed with the "Explanation" button. 

**Note:** The questions encourage understanding of chemical reaction types and require calculations for compositional analysis.
Transcribed Image Text:# Solving a Redox Titration Problem To measure the amount of chlorine in a well-boring fluid, an analytical chemist adds 0.210M silver nitrate (\( \text{AgNO}_3 \)) solution to a 49.0 g sample of the fluid and collects the solid silver chloride (\( \text{AgCl} \)) product. When no more \( \text{AgCl} \) is produced, she filters, washes and weighs it, and finds that 2.21 g has been produced. The balanced chemical equation for the reaction is: \[ \text{Cl}^-_{(aq)} + \text{AgNO}_3 (aq) \rightarrow \text{AgCl} (s) + \text{NO}_3^- (aq) \] --- **Question:** What kind of reaction is this? - [ ] precipitation - [ ] acid-base - [ ] redox **Instructions:** 1. **If you said this was a _precipitation_ reaction, enter the chemical formula of the precipitate.** 2. **If you said this was an _acid-base_ reaction, enter the chemical formula of the reactant that is acting as the base.** 3. **If you said this was a _redox_ reaction, enter the chemical symbol of the element that is oxidized.** 4. **Calculate the mass percent of Cl in the sample. Be sure your answer has 3 significant digits.** --- **Interface:** - There are options to select the type of reaction and fields for input based on the choice made. - The solution can be checked using the "Check" button. - Additional help can be accessed with the "Explanation" button. **Note:** The questions encourage understanding of chemical reaction types and require calculations for compositional analysis.
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