A certain weak acid, HA, with a Ka value of 5.61*10^-6, is titrated with NaOH.
A solution is made by mixing 9.00 mmols (millimoles) of HA and 3.00 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 51.0 mL?
(i know that this is the math section, but there's noone in the chem section!) surely there's a chem student out there who knows how to do this problem!)

Question

A certain weak acid, HA, with a Ka value of 5.61*10^-6, is titrated with NaOH.
A solution is made by mixing 9.00 mmols (millimoles) of HA and 3.00 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 51.0 mL?
(i know that this is the math section, but there's noone in the chem section!) surely there's a chem student out there who knows how to do this problem!)