Problem: Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after each of the following additions of acid:(b) 15.00 mL

FREE Expert Solution

Step 1

total volume = 30.00 mL + 15.00 mL = 45.00 mL


[HBr] = (15.00 mL)(0.1000 M)(45.00 mL) = 0.0333 M


[KOH] = (30.00 mL)(0.1000 M)(45.00 mL) = 0.0666 M


Step 2

[HBr] = 0.0333 M - 0.0333 M = 0

[KOH] = 0.0666 M - 0.0333 M = 0.0333 M


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Problem Details

Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after each of the following additions of acid:

(b) 15.00 mL

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Our tutors have indicated that to solve this problem you will need to apply the Strong Acid Strong Base Titrations concept. You can view video lessons to learn Strong Acid Strong Base Titrations. Or if you need more Strong Acid Strong Base Titrations practice, you can also practice Strong Acid Strong Base Titrations practice problems.

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Based on our data, we think this problem is relevant for Professor Keyes' class at BU.

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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.