Determine the pH during the titration of 14.9 mL of 0.149 M nitric acid by 7.12x10-2 M potassium hydroxide at the following points: (1) Before the addition of any potassium hydroxide (2) After the addition of 15.6 mL of potassium hydroxide (3) At the equivalence point (4) After adding 38.4 mL of potassium hydroxide

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**Titration of Nitric Acid by Potassium Hydroxide: pH Determination**

Determine the pH during the titration of 14.9 mL of 0.149 M nitric acid by \(7.12 \times 10^{-2}\) M potassium hydroxide at the following points:

1. Before the addition of any potassium hydroxide: ____

2. After the addition of 15.6 mL of potassium hydroxide: ____

3. At the equivalence point: ____

4. After adding 38.4 mL of potassium hydroxide: ____

**Explanation:**

This exercise involves a titration process, where a solution of known concentration (titrant) is used to determine the concentration of an unknown solution. Here, potassium hydroxide (KOH) is the titrant added to nitric acid (HNO₃), a strong acid, to determine various pH levels during the chemical reaction. The reaction leads to the formation of water and potassium nitrate (KNO₃).
Transcribed Image Text:**Titration of Nitric Acid by Potassium Hydroxide: pH Determination** Determine the pH during the titration of 14.9 mL of 0.149 M nitric acid by \(7.12 \times 10^{-2}\) M potassium hydroxide at the following points: 1. Before the addition of any potassium hydroxide: ____ 2. After the addition of 15.6 mL of potassium hydroxide: ____ 3. At the equivalence point: ____ 4. After adding 38.4 mL of potassium hydroxide: ____ **Explanation:** This exercise involves a titration process, where a solution of known concentration (titrant) is used to determine the concentration of an unknown solution. Here, potassium hydroxide (KOH) is the titrant added to nitric acid (HNO₃), a strong acid, to determine various pH levels during the chemical reaction. The reaction leads to the formation of water and potassium nitrate (KNO₃).
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