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A certain weak acid, HA, with a Ka value of 5.61×10−6, is titrated with NaOH. A...

A certain weak acid, HA, with a Ka value of 5.61×10−6, is titrated with NaOH.

A solution is made by titrating 8.00 mmol (millimoles) of HA and 1.00 mmol of the strong base. What is the resulting pH?

More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 46.0 mL ?

No idea how to do this! Please explain..thanks!

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queen_honey_blossom answered 7 months ago
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