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Equal volumes of 0.02M AgNO(3) and 0.01M...

Equal volumes of `0.02M AgNO_(3)` and `0.01M HCN` are mixed. Calculate `[Ag^(o+)]` in solution after attaining equilibrium. `K_(a) HCN = 6.2 xx 10^(-10)` and `K_(sp)` of `AgCN = 2.2 xx 10^(-16)`.

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To solve the problem, we need to find the concentration of silver ions \([Ag^+]\) in a solution after mixing equal volumes of \(0.02M \, AgNO_3\) and \(0.01M \, HCN\). The equilibrium constants given are \(K_a\) for HCN and \(K_{sp}\) for \(AgCN\). ### Step-by-Step Solution: 1. **Initial Concentrations**: - When equal volumes of \(0.02M \, AgNO_3\) and \(0.01M \, HCN\) are mixed, the concentrations will change due to dilution. - The final concentration of \(Ag^+\) from \(AgNO_3\): \[ ...
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