Titration of a weak acid Calculate the pH during the titration of 10.00 mL of 0.400 M hypochlorous acid with 0.500 M NaOH. First what is the initial pH (before any NaOH is added)? - The K, for HOCI is 3.0 x 10-8 M. Need help? Hint, given in general feedback. Answer: How many mL of NaOH are added to reach the equivalence point? Answer: What is the pH after 1.80 mL of NaOH are added? Hint given in general feedback. Answer:

Titration of a weak acid Calculate the pH during the titration of 10.00 mL of 0.400 M hypochlorous acid with 0.500 M NaOH. First what is the initial pH (before any NaOH is added)? - The K, for HOCI is 3.0 x 10-8 M. Need help? Hint, given in general feedback. Answer: How many mL of NaOH are added to reach the equivalence point? Answer: What is the pH after 1.80 mL of NaOH are added? Hint given in general feedback. Answer:

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 34QRT

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Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?
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