### Titration of Diprotic Acid with KOH**Problem Statement:**A 100 mL solution containing 0.10 M of a diprotic acid, \( \text{H}_2\text{A} \), is titrated using 1.0 M KOH. The dissociation constants for the diprotic acid are given as \( K_{a1} = 1.0 \times 10^{-4} \) and \( K_{a2} = 1.0 \times 10^{-8} \).**Task:**Calculate the pH of the solution after the addition of 0, 5, 15, and 20 millimoles of KOH. Assume there is no change in volume upon adding KOH.

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1. A 100 mL volume of 0.10 M H₂A, a diprotic acid, is titrated with 1.0 M KOH. The diprotic acid has Ka1 = 1.0 x 10-4 and Ka2 = 1.0 x 10-8 a) Calculate the pH after the addition of 0, 5, 15 and 20 mmoles of the KOH. Assume no volume change on addition of the KOH.

1. A 100 mL volume of 0.10 M H₂A, a diprotic acid, is titrated with 1.0 M KOH. The diprotic acid has Ka1 = 1.0 x 10-4 and Ka2 = 1.0 x 10-8 a) Calculate the pH after the addition of 0, 5, 15 and 20 mmoles of the KOH. Assume no volume change on addition of the KOH.

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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### Titration of Diprotic Acid with KOH

**Problem Statement:**

A 100 mL solution containing 0.10 M of a diprotic acid, \( \text{H}_2\text{A} \), is titrated using 1.0 M KOH. The dissociation constants for the diprotic acid are given as \( K_{a1} = 1.0 \times 10^{-4} \) and \( K_{a2} = 1.0 \times 10^{-8} \).

**Task:**

Calculate the pH of the solution after the addition of 0, 5, 15, and 20 millimoles of KOH. Assume there is no change in volume upon adding KOH.

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