In titration we are interested in the equivalence point. Chemically this is when enough of the base has been added to completely neutralize the acid. Graphically this is when the reaction rate begins to decrease. How do we determine the equivalence point from P? Next, how do we determine the equivalence point from P'? What does the data suggest? Estimate the equivalence point with these two approaches using your data and graph.

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In titration we are interested in the equivalence point. Chemically this is when enough of the base has been added to completely neutralize the acid. Graphically this is when the reaction rate begins to decrease. How do we determine the equivalence point from P? Next, how do we determine the equivalence point from P'? What does the data suggest? Estimate the equivalence point with these two approaches using your data and graph.

This dataset shows the pH changes in a solution as sodium hydroxide (NaOH) is added. The table consists of two columns: "mL of NaOH" and "pH."

### Data Table

- **mL of NaOH**
  - 0
  - 5
  - 8
  - 10
  - 13
  - 15
  - 18
  - 20
  - 25
  - 27
  - 28
  - 29
  - 30
  - 31
  - 33
  - 35
  - 40

- **pH**
  - 2.22
  - 2.83
  - 3.09
  - 3.23
  - 3.41
  - 3.53
  - 3.71
  - 3.83
  - 4.24
  - 4.51
  - 4.72
  - 5.1
  - 10.66
  - 11.37
  - 11.77
  - 11.96
  - 12.22

### Analysis

- **Initial Stage (0-20 mL):** The pH gradually increases from 2.22 to 3.83, indicating a weak acidic solution being neutralized.

- **Buffer Region (20-29 mL):** The pH continues to rise slowly, from 3.83 to 5.1, suggesting the presence of a buffering system.

- **Equivalence Point and Beyond (30-40 mL):** A rapid increase in pH occurs, reaching alkalinity with values from 10.66 to 12.22. This suggests the neutralization of acidic components and the dominance of NaOH.

This pattern is typical in titration, where a solution transitions from acidic to basic as a strong base is added. The dramatic rise in pH around 30 mL indicates the point where the acid is fully neutralized.
Transcribed Image Text:This dataset shows the pH changes in a solution as sodium hydroxide (NaOH) is added. The table consists of two columns: "mL of NaOH" and "pH." ### Data Table - **mL of NaOH** - 0 - 5 - 8 - 10 - 13 - 15 - 18 - 20 - 25 - 27 - 28 - 29 - 30 - 31 - 33 - 35 - 40 - **pH** - 2.22 - 2.83 - 3.09 - 3.23 - 3.41 - 3.53 - 3.71 - 3.83 - 4.24 - 4.51 - 4.72 - 5.1 - 10.66 - 11.37 - 11.77 - 11.96 - 12.22 ### Analysis - **Initial Stage (0-20 mL):** The pH gradually increases from 2.22 to 3.83, indicating a weak acidic solution being neutralized. - **Buffer Region (20-29 mL):** The pH continues to rise slowly, from 3.83 to 5.1, suggesting the presence of a buffering system. - **Equivalence Point and Beyond (30-40 mL):** A rapid increase in pH occurs, reaching alkalinity with values from 10.66 to 12.22. This suggests the neutralization of acidic components and the dominance of NaOH. This pattern is typical in titration, where a solution transitions from acidic to basic as a strong base is added. The dramatic rise in pH around 30 mL indicates the point where the acid is fully neutralized.
Titration is a method of chemical analysis in which a reactive substance is slowly added to another substance, and some property of the combined substance is measured. This procedure is taught in CHM 116, General Chemistry II.

We will be looking at an example of acid-base titration. Specifically, 25 mL of an unknown monoprotic weak acid is titrated against 0.105M NaOH (which is a strong base). This means we are adding the base to the acid using a burette in a slow and precisely controlled manner. We measure the pH after each addition. (A pH of less than 7 is an acid, and a pH of more than 7 is a base.)
Transcribed Image Text:Titration is a method of chemical analysis in which a reactive substance is slowly added to another substance, and some property of the combined substance is measured. This procedure is taught in CHM 116, General Chemistry II. We will be looking at an example of acid-base titration. Specifically, 25 mL of an unknown monoprotic weak acid is titrated against 0.105M NaOH (which is a strong base). This means we are adding the base to the acid using a burette in a slow and precisely controlled manner. We measure the pH after each addition. (A pH of less than 7 is an acid, and a pH of more than 7 is a base.)
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