# 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

= 0.0333 M

= 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

What scientific concept do you need to know in order to solve this problem?

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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