6. A sample of a chloride salt weighing 484.6 mg is titrated with AGNO, using K,Cro, as indicator. To reach the end point a 52.3 mL of 0.1475 M of AGNO, solution is required. The net ionic equation for the reaction of titration is: Ag+ (aq) + Cl- (aq) – Agce (s) 1. How many moles of Ag+ (aq) ions are used to reach the end point? 2. How many moles of Ct- (aq) have reacted in the titration? 3. How many grams of chloride are present in the sample? 4. What is the mass percent of chloride in the sample?
6. A sample of a chloride salt weighing 484.6 mg is titrated with AGNO, using K,Cro, as indicator. To reach the end point a 52.3 mL of 0.1475 M of AGNO, solution is required. The net ionic equation for the reaction of titration is: Ag+ (aq) + Cl- (aq) – Agce (s) 1. How many moles of Ag+ (aq) ions are used to reach the end point? 2. How many moles of Ct- (aq) have reacted in the titration? 3. How many grams of chloride are present in the sample? 4. What is the mass percent of chloride in the sample?
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Titration Analysis of a Chloride Salt Sample**
A sample of a chloride salt weighing 484.6 mg is titrated with silver nitrate (\( \text{AgNO}_3 \)), using potassium chromate (\( \text{K}_2\text{CrO}_4 \)) as an indicator. To reach the endpoint, 52.3 mL of a 0.1475 M \( \text{AgNO}_3 \) solution is required.
**Net Ionic Equation for the Reaction of Titration:**
\[
\text{Ag}^+ (\text{aq}) + \text{Cl}^- (\text{aq}) \rightarrow \text{AgCl} (\text{s})
\]
**Questions:**
1. How many moles of \( \text{Ag}^+ \) (aq) ions are used to reach the endpoint?
2. How many moles of \( \text{Cl}^- \) (aq) have reacted in the titration?
3. How many grams of chloride are present in the sample?
4. What is the mass percent of chloride in the sample?
**Explanation:**
This problem involves a typical titration procedure used to determine the concentration of chloride ions in a given salt sample. The reaction involves the formation of a precipitate, silver chloride (\( \text{AgCl} \)), through the mixing of silver ions (\( \text{Ag}^+ \)) and chloride ions (\( \text{Cl}^- \)) in the solution. The goal is to calculate the moles of reagents used, the mass of chloride, and its percentage in the sample.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb3f91dc4-b37e-4d99-b70a-878366312169%2F5deb9ad0-4a2c-4a9c-90f1-0366dc308c71%2Fpw4k4m_processed.png&w=3840&q=75)
Transcribed Image Text:**Titration Analysis of a Chloride Salt Sample**
A sample of a chloride salt weighing 484.6 mg is titrated with silver nitrate (\( \text{AgNO}_3 \)), using potassium chromate (\( \text{K}_2\text{CrO}_4 \)) as an indicator. To reach the endpoint, 52.3 mL of a 0.1475 M \( \text{AgNO}_3 \) solution is required.
**Net Ionic Equation for the Reaction of Titration:**
\[
\text{Ag}^+ (\text{aq}) + \text{Cl}^- (\text{aq}) \rightarrow \text{AgCl} (\text{s})
\]
**Questions:**
1. How many moles of \( \text{Ag}^+ \) (aq) ions are used to reach the endpoint?
2. How many moles of \( \text{Cl}^- \) (aq) have reacted in the titration?
3. How many grams of chloride are present in the sample?
4. What is the mass percent of chloride in the sample?
**Explanation:**
This problem involves a typical titration procedure used to determine the concentration of chloride ions in a given salt sample. The reaction involves the formation of a precipitate, silver chloride (\( \text{AgCl} \)), through the mixing of silver ions (\( \text{Ag}^+ \)) and chloride ions (\( \text{Cl}^- \)) in the solution. The goal is to calculate the moles of reagents used, the mass of chloride, and its percentage in the sample.
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