What volume of 2.00 M NaOH must be added to 150.0 mL of 1.50 M lactic acid to produce a buffer solution having a pH of 4.00? (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLV2 References' Tables to answer this question as the values will not match.) Volume = mL

What volume of 2.00 M NaOH must be added to 150.0 mL of 1.50 M lactic acid to produce a buffer solution having a pH of 4.00? (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLV2 References' Tables to answer this question as the values will not match.) Volume = mL

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.7QE

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The course is specifically quantitative analysis, I figured that would just fall under chemistry. The issue I'm having with this one is that I have absolutely no idea how to even begin. I figure benzoic acid wouldn't affect the pH of NaOH that much since it's a weak acid and NaOH is a strong base, but I don't think it'd be right to just take the pH using solely the concentration of NaOH. What approach should I take to solve this? 220 mL of 0.03 M NaOH were added to 200 mL of 0.03 M benzoic acid (pKa = 4.2). What is the pH of the resulting solution?
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lets do Calculations System I * 0.010 M HCl * 0.0010 NaOH System II * 0.010 M ( HA ) * 0.0010 M ( B ) System IV * Buffer
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