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**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

$\left[\mathrm{HBr}\right]\mathbf{}\mathbf{=}\mathbf{}\frac{(15.00\overline{)\mathrm{mL}})(0.1000M)}{(45.00\overline{)\mathrm{mL}})}$** = 0.0333 M**

$\mathbf{\left[}\mathbf{KOH}\mathbf{\right]}\mathbf{}\mathbf{=}\mathbf{}\frac{\mathbf{(}\mathbf{30}\mathbf{.}\mathbf{00}\mathbf{}\overline{)\mathbf{mL}}\mathbf{)}\mathbf{(}\mathbf{0}\mathbf{.}\mathbf{1000}\mathbf{}\mathbf{M}\mathbf{)}}{(45.00\overline{)\mathrm{mL}})}$** = 0.0666 M**

Step 2

[HBr] = 0.0333 M - 0.0333 M = 0

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

###### 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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