Three milliliters of a 2.0 M solution of HCl are added to 1 liter of buffer solution containing 0.40 moles of the weak acid, propanoic acid (Ka = 1.4 x 10^-5) and 0.50 moles of its conjugate base, sodium propanate.
a.What is the original pH of the buffer before the strong acid is added?
b. What is the pH of the buffer after the HCI is added? Assume negligible volume change.

The weak base-conjugate acid buffer used in this laboratory consists of a weak base ammonia, NH₃, and its conjugate acid ammonium chloride, NH₄CI. If the NH₃ concentration is 0.05 M and the NH₄C1 concentration is 0.05 M, what is the pH of the buffer? K_b for NH3 is 1.8 x10^-5.