An analytical chemist is titrating 156.4 mL of a 0.3600 M solution of formic acid (H,CO,) with a 0.6800 M solution of NaOH. The pK of formic acid is 3.74. Calculate the pH of the acid solution after the chemist has added 91.45 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.

An analytical chemist is titrating 179.6 mL of a 0.8400M solution of cyanic acid (HCNO) with a 1.200M solution of KOH. The p K, of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 144.3 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH = |

A chemist titrates 110.0 mL of a 0.1235M butanoic acid (HC,H,CO,) solution with 0.0643 M KOH solution at 25 °C. Calculate the pH at equivalence. The pK, of butanoic acid is 4.82. 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 = ] ? %3D

The pK, of hypochlorous acid is 7.530. A 52.0 mL solution of 0.148 M sodium hypochlorite (NaOCI) is titrated with 0.293 M HCI. Calculate the pH of the solution after the addition of 10.3 mL of 0.293 M HCI. pH = Calculate the pH of the solution after the addition of 27.9 mL of 0.293 M HCI. pH = Calculate the pH of the solution at the equivalence point with 0.293 M HCI. pH =

A student wishes to make a buffer that has a pH of 4.65.  The student has HNO2 and NaNO2.  Nitrous Acid (HNO2) has a pKa of 3.40 The student makes 100.0 mL of a 0.100 M solution of HNO2.  What mass (in grams) of NaNO2  should the student add to the solution to make a buffer that buffers at a pH of 4.25. (Hint: use the Henderson-Hasselbalch equation to find the molarity, then find the number of moles required to achieve that concentration in 100.0 mL of solution.)

An analytical chemist is titrating 161.4 mL of a 0.8000M solution of trimethylamine ((CH,) N) with a 0.8900M solution of HIO3. The p K, of trimethylamine 3 is 4.19. Calculate the pH of the base solution after the chemist has added 161.5 mL of the HIO, solution to it. 3. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO, solution added. Round your answer to 2 decimal places.

1. A buffer solution contains 0.419 M of ammonium chloride and 0.221 M of ammonia.If 0.0293 moles of sodium hydroxide are added to 150 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume does not change upon adding sodium hydroxide.) 2. A buffer solution contains 0.286 M of ammonium chloride and 0.472 M of ammonia. If 0.0620 moles of nitric acid are added to 250 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume does not change upon adding nitric acid.)

A chemist titrates 220.0 mL of a 0.6204 M butanoic acid (HC₂H,CO₂) solution with 0.2746 M KOH solution at 25 °C. Calculate the pH at equivalence. The PK of butanoic acid is 4.82. 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 = 0 X Ś

A formic acid buffer is prepared with 0.010 M each of formic acid (HCOOH) and Sodium formate (NaCOOH). The Ka for formic acid is 1.8 x 10-4. What is the pH of the solution? What is the pH if 0.0020 M of solid sodium hydroxide (NaOH) is added to a liter of buffer? What would be the pH of the sodium hydroxide solution without the buffer? What would the pH have been after adding sodium hydroxide if the buffer concentrations had been 0.10 M instead of 0.010 M?

An analytical chemist is titrating 143.6 mL of a 0.7000M solution of piperidine (C,H10NH) with a 0.4000M solution of HNO3. The p K, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 267.7 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH