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Calculate the pH of a solution obtained ...

Calculate the `pH` of a solution obtained by mixing equal volume of `0.02MHOCl &0.2MCH_(3)COOH` solutions
Given that `K_(a)(HOCl)=2xx10^(-4),K_(a)(CH_(3)COOH)=2xx10^(-5)`
Also calculate `[OH^(-)],[OCl^(-)],[CH_(3)COOH]` at equilibrium .Take `log2=0.3`

Text Solution

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To solve the problem, we need to calculate the pH of a solution obtained by mixing equal volumes of 0.02 M HOCl and 0.2 M CH₃COOH. We will also find the concentrations of OH⁻, OCl⁻, and CH₃COOH at equilibrium. ### Step 1: Determine the final concentrations after mixing When equal volumes of two solutions are mixed, the concentrations of the solutes are halved because the total volume doubles. - Initial concentration of HOCl = 0.02 M - Initial concentration of CH₃COOH = 0.2 M ...
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