A 44.0-mL sample of 0.202 M CH3COOH (Ka = 1.8 x 10-5 ) solution is titrated with 0.185 M NaOH. Calculate the pH of the solution (a) before the addition of any NaOH solution  (b) after the addition of 20.0 mL,  (c) after the addition of 48.0 mL,

1) Determine the pH during the titration of 74.5 mL of 0.348 M nitrous acid (Ka = 4.5×10-4) by 0.348 M NaOH at the following points.   (a) Before the addition of any NaOH ?   (b) After the addition of 18.0 mL of NaOH ?   (c) At the half-equivalence point (the titration midpoint) ?   (d) At the equivalence point ?   (e) After the addition of 112 mL of NaOH ?

15.0 mL of a buffer is made by mixing 10.0 mL of 0.10 M HF and 5.0 mL of 0.10 M NaOH solution. What is the pH of this buffer after 0.24 mL of 1.0 M sodium hydroxide are added to it? The Ka for HF is 6.8 x 10-4.

You are given a 1.00 L buffer solution that is 0.250 M in HF and 0.250 M in LiF.  Find the pH of the solution after the addition of 0.150 moles of solid LiOH.  Assume no volume change upon the addition of base.  The Ka for HF is 3.5 × 10-4.