The pKa (pka) of hypochlorous acid is 7.530. A 59.0 mL solution of 0.105 M sodium hypochlorite (NaOCl) is titrated with 0.331 M HCl. Calculate the pH of the solution after the addition of 7.11 mL of 0.331 M HCl. pH=     Calculate the pH of the solution after the addition of 19.3 mL of 0.331 M HCl. pH=     Calculate the pH of the solution at the equivalence point with 0.331 M HCl. pH=

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?

An analytical chemist is titrating 100.0mL of a 0.3300M solution of hydrazoic acid (HNg) with a 1.100M solution of KOH. The pKa of hydrazoic acid is 4.72. Calculate the pH of the acid solution after the chemist has added 50.00mL of the KOH solution to it.

Consider the titration of 80.0 mL of 0.100 M Ba (OH), by 0.400M HCl. Calculate the pH of the resulting solution after the following volumes of HCI have been added. a. 0.0 ml pH = Ь. 20.0 mL pH = c. 30.0 mL pH = d. 40.0 mL pH = e. 90.0 mL pH =

Concentration of HCl: 0.05 M Volume of HCl: 4.4 ml Concentration of NaOH: 0.0088M Volume of NaOH: 25 ml

When 30 .00 mL of 0.1011 M HCl in 50 mL of deionized water is titrated against 0.09889 M NaOH, the pH increases. What is the volume (in mL) of NaOH required to reach the equivalence point and a pH of 7.00? Find the pH when the volume of NaOH added is 0.02 mL less than the volume required to reach the equivalence point. Find the pH when the volume of NaOH added is 0.01 mL less than the volume required to reach the equivalence point. Find the pH when the volume of NaOH added is 0.02 mL more than the volume required to reach the equivalence point. Comment on the significance of the changes in pH values in relation to the increments of sodium hydroxide added when going “through” the end point. Define equivalence point. For a weak base/strong acid titration, is the pH at the equivalence point <, >, or equal to 7?

A student is titrating a 100 mL of 0.50 M solution of hydrofluoric acid (HF) with 1.0 M strong base (NaOH). a) at the equivalence point, what ions/compounds will be present in the solution? A complete answer will also be specific as to what ions/compounds are not present in solution. b) calculate the pH at the equivalence point.

An analytical chemist is titrating 79.6 mL of a 0.9000M solution of cyanic acid (HCNO) with a 1.200 M solution of NaOH. The pK of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 69.4 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = ☐

An analytical chemist is titrating 79.6 mL of a 0.9000M solution of cyanic acid (HCNO) with a 1.200 M solution of NaOH. The pK of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 69.4 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = ☐

An analytical chemist is titrating 111.5 mL of a 0.2600M solution of acetic acid (HCH,CO,) with a 0.5100M solution of NaOH. The p K, of acetic acid is 4.70. Calculate the pH of the acid solution after the chemist has added 10.45 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = |