A beaker with 1.40x102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. Thetotal molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 7.00 mL of a0.490 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is4.740.Express your answer numerically to two decimal places. Use a minus ( - ) sign if the pHhas decreased.View Available Hint(s)ΑΣφApH =

Answered: Image /qna-images/answer/166adb3d-f96a-4592-9568-3fc89c385d51.jpg

Answered: A beaker with 1.40x102 mL of an acetic…

Aquaculture Science

3rd Edition

ISBN:9781133558347

Author:Parker

Publisher:Parker

Chapter11: Health Of Aquatic Animals

Section: Chapter Questions

Problem 3KA

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The pH probe/meter uses following equations: Ecell = L + 0.0592 log a1 = L - 0.0592 pH Where L = L1 + EAg/AgCI + Easy= constants L1 = - 0.0592 log a2 a1 = activity of analyte solution a2 = activity of internal solution How will measured pH value be affected vs “real” pH if HCl in pH electrode, became 0.15M instead of 0.1M ? a.impact can not be determined b.measured pH is higher than "real" pH. c.measured pH is lower than "real" pH. d.measured pH is same as "real" pH.
The pH probe/meter uses following equations: Ecell = L + 0.0592 log a1 = L - 0.0592 pH Where L = L1 + EAg/AgCI + Easy= constants L1 = - 0.0592 log a2 a1 = activity of analyte solution a2 = activity of internal solution How will measured pH value be affected vs “real” pH if the temperature of the sample is 30C when pH was measured ? a.measured pH is lower than real pH b.impact can not be determined c.measured pH is higher than real pH d.measured pH is same as real pH

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