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At equilibrium, a 1.00 M OCl− solution has an [OH−] of 5.75 × 10−4 M. Which of the following is the correct pH of the solution? 3.24 3.3 × 10−7 14.00 10.76

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Below is the solution:

pOH = - log (5.75 × 10^−4) = 3.24 
pH = 14 - 3.24 = 10.76

pOH = - log (5.75 × 10^−4) = 3.24

pH = 14 - 3.24 = 10.76

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