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Calculate pH(1),[HS^(-)],[S^(2-)],[Cl^(-...

Calculate `pH_(1),[HS^(-)],[S^(2-)],[Cl^(-)]` in a solution which is `0.1M` in `HCl& 0.1M in H_(2)S`.Given that `K_(a_(1))(H_(2)S)=10^(-7),K_(a_(2))(H_(2)S)=10^(-14)`.Also calculate degree of dissociation of `H_(2)S` &`HS^(-)` in solution.

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To solve the problem, we need to calculate the pH, concentrations of \( [HS^-] \), \( [S^{2-}] \), and \( [Cl^-] \) in a solution that is \( 0.1M \) in \( HCl \) and \( 0.1M \) in \( H_2S \). We are also given the dissociation constants \( K_{a1} \) and \( K_{a2} \) for \( H_2S \). ### Step 1: Calculate the pH of the solution 1. **Determine the contribution of \( HCl \)**: - Since \( HCl \) is a strong acid, it will completely dissociate in solution: \[ HCl \rightarrow H^+ + Cl^- ...
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