Consider the titration of 25 mL of 0.1 M HCHO2 (known as formic acid and has a Ka of 1.8 x 10-4) with 0.1 M of the strong base KOH. Clearly calculate the initial pH, the pH at half way to the equivalence point, the pH at the equivalence point, and the pH after the addition of infinite excess KOH.

A 50.0 mL aliquot of a 0.00100M solution of acetic acid (K, = 1.8 x 10-5) is titrated with 0.00993M NaOH. Use the Indicator Table below to decide which of the indicators listed would most accurately signal the equivalence point for this titration. Properties of Several Indicators Write the letter corresponding to your choice of indicator in the box

Determine the pH for the 4 stages of chemistry in a titration between 25.0 mL of 0.247 M HBRO2 and 0.125 M NAOH. (Equilibrium constant for HBRO2 is 1.2 x 10-5.)-0 mL, 33.2 mL, equivalence point and 72.5 mL of NaOH.

Use the Henderson-Hasselbalch equation to calculate the pH of a buffer that is 0.18 M acetic acid and 0.85 M in acetate anion. The pKa value for acetic acid is 4.74. Round your answer to two decimal places.