Question

A 25.00 mL sample of a diprotic weak acid, H2A, is being titrated with 0.0469 M KOH such that the acid is fully deprotonated. The student runs three titrations and finds the average volume of base used to be 16.09 mL. Using the average of the titration volumes, determine the concentration of the acid solution in mol/L.

Name: a 2500 ml sample of a diprotic weak acid h2a is being titrated with 00469 m koh such that the acid is fully deprotonated the student runs three titrations and finds the average volume of bas 08524
Uploaded: 2022-04-17T05:00:12-08:00
Duration: 5 min 50 s
Channel: Adedamola Opalade
Description: a 2500 ml sample of a diprotic weak acid h2a is being titrated with 00469 m koh such that the acid is fully deprotonated the student runs three titrations and finds the average volume of bas 08524

          A 25.00 mL sample of a diprotic weak acid, H2A, is being titrated with 0.0469 M KOH such that the acid is fully deprotonated. The student runs three titrations and finds the average volume of base used to be 16.09 mL. Using the average of the titration volumes, determine the concentration of the acid solution in mol/L.

Added by Guillermo R.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adedamola Opalade

04/17/2022

Step 1

To find the number of moles of KOH, use the formula: \[ \text{moles of KOH} = \text{concentration of KOH} \times \text{volume of KOH in liters} \] The average volume of KOH used is 16.09 mL, which needs to be converted to liters: \[ 16.09 \, \text{mL} = Show more…

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A 25.00 mL sample of a diprotic weak acid, H2A, is being titrated with 0.0469 M KOH such that the acid is fully deprotonated. The student runs three titrations and finds the average volume of base used to be 16.09 mL. Using the average of the titration volumes, determine the concentration of the acid solution in mol/L.