Given a theoretical acid, HA, with a pKa of 6.52. Calculate the pH of 30.0mL of 0.400M HA, when it is titrated with 0.150M Sr(OH)2 and calculate the pH for the following % titrant: 0.00%, 50.0%, 96.0%, 100.%, 105.% of eq. pt.

A chemist titrates 100.0 mL of a 0.0714M nitrous acid (HNO,) solution with 0.3683M KOH solution at 25 °C. Calculate the pH at equivalence. The p K, of nitrous acid is 3.35. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added. pH = |

1.Determine the pH during the titration of 62.9 mL of 0.360 M hydrocyanic acid (Ka = 4.0×10-10) by 0.360 M KOH at the following points. (Assume the titration is done at 25 °C.)(a) Before the addition of any KOH (b) After the addition of 16.0 mL of KOH (c) At the half-equivalence point (the titration midpoint)  (d) At the equivalence point  (e) After the addition of 94.4 mL of KOH    2. When a 23.3 mL sample of a 0.379 M aqueous hypochlorous acid solution is titrated with a 0.407 M aqueous sodium hydroxide solution,(1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 32.5 mL of sodium hydroxide have been added?

Determine the pH of a 10-3 mol/L solution of (a) hydrogen sulfate ion (pKa = 1.99), (b) formic acid (pKa = 3.75), (c) hypochlorous acid (pKa = 7.53), (d) phenol (pKa = 9.98)