A buffer is prepared by adding 1.50x10(exponent 2)mL of 0.250M NaOH to 2.50x10(exponent 2)mL of 0.350M weak acid, HB. The solution is diluted to 1.00L. If the pH of the resulting solution is 5.55, what is the pKa of the weak acid?
From Henderson-Hasselbalch equation
pH = pKa + log ([conjugate base]/[acid])
Here pH = ...
Solution uses Henderson-Hasselbalch to solve problem, including steps.