Explain ph of the new solution at equivalence point

Reference no: EM13533902

A certain weak acid, HA, with a Ka value of 5.61*10 raised to negative 6 is titrated with NaOH. A solution is made by mixing 7.00 mmol (millimoles) of HA and 1.00 mmol of strong base. What is the pH? I figured out the pH was 4.47. But a more strong base is added until equivalence point is reached. What is pH of this new solution at equivalence point if total volume is 35.0 mL?

Reference no: EM13533902

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