Exercise Precipitation titration is a volumetric method based upon the formation of slightly soluble Precipitate: AgNO3(aq) + NaCl(aq) AgCl(s) Construct a titration curve by plotting pAg vs. VAgNO3 added VAgNO3 (ml) [Ag¹] pAg* 0.0 5 10.0 15 20 25 30 Ag (aq) 35 40 45 50 + CF (aq) Ksp = 1.6*10-10 a.1.30 b.1.43 c.4.90 d.7.00 e.7.65 titrant: AgNO3, 0.1M analyte: NaC1, 0.05M, 50 ml. Question1) What is pAg at the equivalence point of titration?

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**Exercise: Precipitation Titration**

Precipitation titration is a volumetric method based upon the formation of a slightly soluble precipitate:

\[ \text{AgNO}_3(aq) + \text{NaCl}(aq) \rightarrow \text{AgCl}(s) \leftarrow \text{Ag}^+(aq) + \text{Cl}^-(aq) \]

\[ k_{sp} = 1.6 \times 10^{-10} \]

**Construct a titration curve by plotting pAg\(^+\) vs. \( V_{\text{AgNO}_3} \) added**

| \( V_{\text{AgNO}_3} \) (ml) | [Ag\(^+\)] | pAg\(^+\) |
|-------------------------------|-----------|-----------|
| 0.0                           |           |           |
| 5                             |           |           |
| 10                            |           |           |
| 15                            |           |           |
| 20                            |           |           |
| 25                            |           |           |
| 30                            |           |           |
| 50                            |           |           |

**Setup Diagram:**

The image includes a diagram showing a typical titration setup. This setup involves:

- A burette filled with the titrant, AgNO\(_3\), with a concentration of 0.1 M.
- The analyte, NaCl, with a concentration of 0.05 M, is placed in a 50 mL Erlenmeyer flask or beaker below the burette.
- The setup is ready for the titration process where AgNO\(_3\) is gradually added to the NaCl solution.

**Question 1:**

What is pAg at the equivalence point of titration?

a. 1.30  
b. 1.43  
c. 4.90  
d. 7.00  
e. 7.65
Transcribed Image Text:**Exercise: Precipitation Titration** Precipitation titration is a volumetric method based upon the formation of a slightly soluble precipitate: \[ \text{AgNO}_3(aq) + \text{NaCl}(aq) \rightarrow \text{AgCl}(s) \leftarrow \text{Ag}^+(aq) + \text{Cl}^-(aq) \] \[ k_{sp} = 1.6 \times 10^{-10} \] **Construct a titration curve by plotting pAg\(^+\) vs. \( V_{\text{AgNO}_3} \) added** | \( V_{\text{AgNO}_3} \) (ml) | [Ag\(^+\)] | pAg\(^+\) | |-------------------------------|-----------|-----------| | 0.0 | | | | 5 | | | | 10 | | | | 15 | | | | 20 | | | | 25 | | | | 30 | | | | 50 | | | **Setup Diagram:** The image includes a diagram showing a typical titration setup. This setup involves: - A burette filled with the titrant, AgNO\(_3\), with a concentration of 0.1 M. - The analyte, NaCl, with a concentration of 0.05 M, is placed in a 50 mL Erlenmeyer flask or beaker below the burette. - The setup is ready for the titration process where AgNO\(_3\) is gradually added to the NaCl solution. **Question 1:** What is pAg at the equivalence point of titration? a. 1.30 b. 1.43 c. 4.90 d. 7.00 e. 7.65
**Exercise: Precipitation Titration**

Precipitation titration is a volumetric method based upon the formation of a slightly soluble precipitate.

**Reaction:**

\[ \text{AgNO}_3(\text{aq}) + \text{NaCl}(\text{aq}) \rightarrow \text{AgCl}(\text{s}) \leftrightarrow \text{Ag}^+(\text{aq}) + \text{Cl}^-(\text{aq}) \]

\[ k_{sp} = 1.6 \times 10^{-10} \]

**Instructions:**

Construct a titration curve by plotting \( \text{pAg}^+ \) vs. \( V_{\text{AgNO}_3} \) added.

**Data Table:**

| \( V_{\text{AgNO}_3} \) (ml) | \([ \text{Ag}^+ ]\) | \( \text{pAg}^+ \) |
|------------------------------|---------------------|-------------------|
| 0.0                          |                     |                   |
| 5.0                          |                     |                   |
| 10.0                         |                     |                   |
| 15.0                         |                     |                   |
| 20.0                         |                     |                   |
| 25.0                         |                     |                   |
| 30.0                         |                     |                   |
| 35.0                         |                     |                   |
| 40.0                         |                     |                   |
| 50.0                         |                     |                   |

**Diagram Explanation:**

The diagram shows a titration setup with a burette filled with 0.1 M \( \text{AgNO}_3 \) as the titrant. The analyte in the flask below is a 50 mL solution of 0.05 M \( \text{NaCl} \).

**Question 1:**

What is \( \text{pAg} \) at the equivalence point of titration?

a. 1.30  
b. 1.43  
c. 4.90  
d. 7.00  
e. 7.65
Transcribed Image Text:**Exercise: Precipitation Titration** Precipitation titration is a volumetric method based upon the formation of a slightly soluble precipitate. **Reaction:** \[ \text{AgNO}_3(\text{aq}) + \text{NaCl}(\text{aq}) \rightarrow \text{AgCl}(\text{s}) \leftrightarrow \text{Ag}^+(\text{aq}) + \text{Cl}^-(\text{aq}) \] \[ k_{sp} = 1.6 \times 10^{-10} \] **Instructions:** Construct a titration curve by plotting \( \text{pAg}^+ \) vs. \( V_{\text{AgNO}_3} \) added. **Data Table:** | \( V_{\text{AgNO}_3} \) (ml) | \([ \text{Ag}^+ ]\) | \( \text{pAg}^+ \) | |------------------------------|---------------------|-------------------| | 0.0 | | | | 5.0 | | | | 10.0 | | | | 15.0 | | | | 20.0 | | | | 25.0 | | | | 30.0 | | | | 35.0 | | | | 40.0 | | | | 50.0 | | | **Diagram Explanation:** The diagram shows a titration setup with a burette filled with 0.1 M \( \text{AgNO}_3 \) as the titrant. The analyte in the flask below is a 50 mL solution of 0.05 M \( \text{NaCl} \). **Question 1:** What is \( \text{pAg} \) at the equivalence point of titration? a. 1.30 b. 1.43 c. 4.90 d. 7.00 e. 7.65
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