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A 0.1M solution of weak acid HA is 1% di...

A `0.1M `solution of weak acid `HA` is `1%` dissociated at `298k`. what is its `K_(a)`? what will be the new degree of dissociation of `HA` and `pH` when `0.2M` of `NaA` is added to it.

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To solve the problem step by step, we will first calculate the dissociation constant \( K_a \) of the weak acid \( HA \) and then determine the new degree of dissociation and pH when \( 0.2M \) of \( NaA \) is added. ### Step 1: Calculate \( K_a \) 1. **Given Information:** - Concentration of weak acid \( [HA] = 0.1M \) - Degree of dissociation \( \alpha = 1\% = 0.01 \) ...
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