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The henderson hasselbalch equation

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A solution has [C6H5COOH] = 0.100 M and [Ca(C6H5COO)2] = 0.200 M. Ka = 6.3 × 10^-5 for C6H5COOH. The solution volume is 5.00 L. What is the pH of the solution after 10.00 ml of 5.00 M NaOH is added? How would I do this using the Henderson Hasselbalch equation?

Reference no: EM131025238

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