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13 Dec 2019
Consider the titration of 40.0 mL of 0.210 M hypochlorous acid (HClO) with 0.09459 M KOH.
a) Calculate the moles of hypochlorous acid is present in the sample before titration (do not include dissociation).
b) What volume of KOH is required to reach the end point?
c) Calculate the pH after 8.08 mL KOH has been added
d) Calculate the pH after 44.4 mL KOH has been added
e) Calculate the pH after the addition of 88.80mL KOH.
f) Calculate the pH after the addition of 89.00mL
Consider the titration of 40.0 mL of 0.210 M hypochlorous acid (HClO) with 0.09459 M KOH.
a) Calculate the moles of hypochlorous acid is present in the sample before titration (do not include dissociation).
b) What volume of KOH is required to reach the end point?
c) Calculate the pH after 8.08 mL KOH has been added
d) Calculate the pH after 44.4 mL KOH has been added
e) Calculate the pH after the addition of 88.80mL KOH.
f) Calculate the pH after the addition of 89.00mL
Keith LeannonLv2
17 Dec 2019
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Related questions
| Hypochlorous | HClO | 4.0Ã10â8 |
Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.240 M HCIO(aq) with 0.240 M KOH(aq). The ionization constant for HCIO can be found here. Number (a) before addition of any KOH Number (b) after addition of 25.0 mL of KOH Number (c) after addition of 30.0 mL of KOH Number (d) after addition of 50.0 mL of KOH Number (e) after addition of 60.0 mL of KOH
