An analytical chemist is titrating 181.5 mL of a 1.000M solution of cyanic acid (HCNO) with a 0.8500M solution of KOH. The pK of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 162.6 mL of the KOH solution to it.

An analytical chemist is titrating 75.7mL of a 0.4500M solution of cyanic acid HCNO with a 0.2400M solution of KOH. The pKa of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 168.mL of the KOH solution to it.

An analytical chemist is titrating 123.0 mL of a 0.1500M solution of dimethylamine ((CH3)2NH) with a 0.1200M solution of HNO3. The p K² of dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 84.5 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = 0 X 5

An analytical chemist is titrating 195.6 mL of a 0.3900M solution of butanoic acid (HC,H,CO,) with a 1.200M solution of KOH. The p K, of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 40.17 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 =

What molar ratio of salt to acid would be required to prepare a buffer solution with a pH of 5.9? The pKa of the acid is 5.7. How many grams of ammonium sulfate ((NH4 )2SO4 )) would you need to add to 425 mL of 0.28 M ammonia (NH3 ) to obtain a buffer solution with a pH of 9.45. Assume that the volume doesn’t change when you add the salt. Ka for the ammonium ion is 5.8 x 10-10 . (be careful with how the reaction for ammonium is written as well as stoichiometry) A 1.00 L volume of buffer is made with concentrations of 0.350 M sodium formate (NaHCOO) and 0.550 M formic acid (HCOOH). (Ka of HCOOH is 1.8 x 10-4 ) a. Calculate the initial pH of this buffer. b. What is the pH after the addition of 0.0050 mol HCl? c. How about after the addition of 0.0050 mol NaOH? [For parts b and c, assume that volume doesn’t change in the addition process and that neutralization proceeds to completion]

An analytical chemist is titrating 160.8 mL of a 1.000 M solution of nitrous acid (HNO,) with a 0.7800 M solution of KOH. The pK of nitrous acid is 3.35. Calculate the pH of the acid solution after the chemist has added 104.5 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 = Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibility acer &

An analytical chemist is titrating 198.2mL  of a  0.8000M  solution of acetic acid  HCH3CO2  with a  0.9600M  solution of  KOH . The  pKa  of acetic acid is  4.70 .Calculate the pH of the acid solution after the chemist has added  117.2mL  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.

An analytical chemist is titrating 92.2mL of a 0.4800M solution of piperidine C5H10NH with a 0.4500M solution of HNO3 . The pKb of piperidine is 2.89 .Calculate the pH of the base solution after the chemist has added 21.3mL of the HNO3 solution to it.

An analytical chemist is titrating 87.3 mL of a 0.9000M solution of butanoic acid (HC₂H₂CO₂) with a 0.6200M solution of KOH. The pK of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 150. mL of the KOH solution to it. a 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 0 X S 00. 18 Ar

An analytical chemist is titrating 101.8 mL of a 1.100M solution of benzoic acid (HC H₂CO₂) with a 0.2600M solution of KOH. The p K of benzoic acid is 4.20. Calculate the pH of the acid solution after the chemist has added 514.6 mL of the KOH solution to it. a 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 = X Ś 00. 18 Ar 8