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Determine the pH during the titration of 18.9 mL of 0.253 M hydrobromic acid by 0.205 M potassium hydroxide at the following points: (1) Before the addition of any potassium hydroxide (2) After the addition of 11.7 mL of potassium hydroxide (3) At the equivalence point (4) After adding 28.7 mL of potassium hydroxide

Determine the pH during the titration of 18.9 mL of 0.253 M hydrobromic acid by 0.205 M potassium hydroxide at the following points: (1) Before the addition of any potassium hydroxide (2) After the addition of 11.7 mL of potassium hydroxide (3) At the equivalence point (4) After adding 28.7 mL of potassium hydroxide

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Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Titration of Hydrobromic Acid with Potassium Hydroxide:** Determine the pH during the titration of 18.9 mL of 0.253 M hydrobromic acid by 0.205 M potassium hydroxide at the following points: 1. Before the addition of any potassium hydroxide: ______ 2. After the addition of 11.7 mL of potassium hydroxide: ______ 3. At the equivalence point: ______ 4. After adding 28.7 mL of potassium hydroxide: ______ --- This information will help you understand the changes in pH during the titration process, which is essential for analyzing the acidity and neutralization reactions.
Transcribed Image Text:**Titration of Hydrobromic Acid with Potassium Hydroxide:** Determine the pH during the titration of 18.9 mL of 0.253 M hydrobromic acid by 0.205 M potassium hydroxide at the following points: 1. Before the addition of any potassium hydroxide: ______ 2. After the addition of 11.7 mL of potassium hydroxide: ______ 3. At the equivalence point: ______ 4. After adding 28.7 mL of potassium hydroxide: ______ --- This information will help you understand the changes in pH during the titration process, which is essential for analyzing the acidity and neutralization reactions.
Expert Solution
Step 1

In strong acid and strong base titrations, the pH of the solution depends on the concentration of acid or base which is present in excess.

The neutralization reaction between HBr and KOH is

HBr(aq) + KOH(aq) ------> KBr(aq) + H2O (l) 

=> 1 mole of HBr = 1 mole of KOH 

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