# A 25.0 mL sample of 0.100 M acetic acid is titrated with0.125 M NaOH at 25°C. What is the pH of the solutionafter 10.0, 20.0, and 30.0 mL of the base have been added?

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A 25.0 mL sample of 0.100 M acetic acid is titrated with
0.125 M NaOH at 25°C. What is the pH of the solution
after 10.0, 20.0, and 30.0 mL of the base have been added?

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Step 1

Given

Volume of the acetic acid =25ml

Molarity of the acetic acid= 0.1M

Volume of the NaOH solution = ?

Molarity of the NaOH solution= 0.125M

Step 2

We estimate the end point for the titration help_outlineImage TranscriptioncloseVS,=V,S, where V is the volume of the two solutions S is the strength of the two solutions fullscreen
Step 3 help_outlineImage Transcriptionclose25 moles of acetic acid= 0.1x- 1000 -0.0025 end point of titration S2 0.1Mx 0.025L 0.125M 0.02L = fullscreen

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### Chemistry 