A certain weak acid, HA, with a Ka value of 5.61×10−6, is titrated with NaOH. A solution is made by titrating 9.00 mmol (millimoles) of HA and 2.00 mmol of the strong base. The resulting pH is 4.71. 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 30.0 mL ?

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