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When a 17.3 mL sample of a 0.439 M aqueous hypochlorous acid solution is titrated with a 0.388 M aqueous sodium hydroxide solution, what is the pH after 29.4 mL of sodium hydroxide have been added? pH =

When a 17.3 mL sample of a 0.439 M aqueous hypochlorous acid solution is titrated with a 0.388 M aqueous sodium hydroxide solution, what is the pH after 29.4 mL of sodium hydroxide have been added? pH =

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Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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When a 17.3 mL sample of a 0.439 M aqueous hypochlorous acid solution is titrated with a 0.388 M aqueous sodium hydroxide solution, what is the pH after 29.4 mL of sodium hydroxide have been added? pH = [ ]
Transcribed Image Text:When a 17.3 mL sample of a 0.439 M aqueous hypochlorous acid solution is titrated with a 0.388 M aqueous sodium hydroxide solution, what is the pH after 29.4 mL of sodium hydroxide have been added? pH = [ ]
**Titration Problem: Calculating the pH at the Midpoint** When a 16.9 mL sample of a 0.334 M aqueous hypochlorous acid solution is titrated with a 0.475 M aqueous sodium hydroxide solution, what is the pH at the midpoint in the titration? **pH =** [Input box]
Transcribed Image Text:**Titration Problem: Calculating the pH at the Midpoint** When a 16.9 mL sample of a 0.334 M aqueous hypochlorous acid solution is titrated with a 0.475 M aqueous sodium hydroxide solution, what is the pH at the midpoint in the titration? **pH =** [Input box]
Expert Solution
Step 1

#Q.1:

Hypochlorous acid, HOCl is a monoprotic weak acid with pKa = 7.53

sodium hydroxide, NaOH is a monoacidic strong base.

The balanced neutralization reaction is:

HOCl(aq) + NaOH(aq) → NaOCl(aq) + H2O(l) 

Since all the coefficients are 1, the mole ratio is 1/1.

Hence moles of NaOH required to reach equivalence point = moles of HOCl taken

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