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0.1 M HA is tritrated against 0.1 M ...

0.1 M HA is tritrated against 0.1 M NaOH . Find the pH the end point . Dissociation constant for the end acid HA is `5 xx 10^(-6)` and degree of hydrolysis , `h lt 1 `

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To find the pH at the endpoint of the titration of 0.1 M HA with 0.1 M NaOH, we can follow these steps: ### Step 1: Understand the Reaction The reaction between the weak acid (HA) and the strong base (NaOH) can be represented as: \[ \text{HA} + \text{NaOH} \rightarrow \text{NaA} + \text{H}_2\text{O} \] At the endpoint, all the acid (HA) has reacted with the base (NaOH) to form the salt (NaA). ### Step 2: Calculate the Concentration of the Salt ...
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