For a titration of NaOH with a unknown diatomic acid, the phenolphthalein turns

Question

For a titration of NaOH with a unknown diatomic acid, the phenolphthalein turns pink when added 39.72 mL NaOH (pH =8.82)
Help me to calculate the first and second equivalence point, the first and second half equivalence point, and the pH at each point.
For a titration of NaOH with a unknown diatomic acid, the phenolphthalein turns pink when added 39.72 mL NaOH (pH =8.82)
Help me to calculate the first and second equivalence point, the first and second half equivalence point, and the pH at each point.

Help me to calculate the first and second equivalence point, the first and second half equivalence point, and the pH at each point.

Explanation / Answer

Total equivalence point = 39.72 mL

then

2nd equivalence point =  39.72 mL , pH = 8.82

first equivalence point --> 1/2*Total equivalence point = 1/2* 39.72 mL = 19.86 mL will be the 1st equivalence point

pH --> can't be obtained with the given data, but will be approx 3< pKa < 5

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