An analytical chemist is titrating 189.5 mL of a 0.6500M solution of ammonia (NH,) with a 0.8000M solution of HNO3. The p K, of ammonia is 4.74. Calculate the pH of the base solution after the chemist has added 177.1 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 = 0 alo

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 = |

An analytical chemist is titrating 231.8 mL of a 0.9900M solution of acetic acid (HCH, CO,) with a 1.200M solution of NaOH. The p K, of acetic acid is 4.70. Calculate the pH of the acid solution after the chemist has added 131.2 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. alo pH %3| Ar Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center | Accessibility CA

A chemist titrates 210.0 mL of a 0.3206M ammonia (NH3) solution with 0.3768 M HCl solution at 25 °C. Calculate the pH at equivalence. The pK, of ammonia is 4.75. 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 HCl solution added. pH = 0 X

An analytical chemist is titrating 111.3 mL of a 0.2800 M solution of ammonia (NH, with a 0.3500 M solution of HIO,. The p K, of ammonia is 4.74. Calculate 3' the pH of the base solution after the chemist has added 99.0 mL of the HIO, solution to it. 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.

An analytical chemist is titrating 147.3 mL of a 0.3200M solution of ammonia (NH,) with a 0.8200M solution of HNO,. The p K, of ammonia is 4.74. Calculate the pH of the base solution after the chemist has added 64.7 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places.

A chemist titrates 160.0 mL of a 0.3445 M pyridine (C-H5N) solution with 0.8552M HNO3 solution at 25 °C. Calculate the pH at equivalence. The pK, of pyridine is 8.77. 6 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 HNO3 solution added. E pH = 0 X 5 OL 9 L

A chemist titrates 240.0 mL of a 0.0890M aniline (C,H,NH,) solution with 0.6621M HNO, solution at 25 °C. Calculate the pH at equivalence. The p K, of aniline is 4.87. 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 HNO, solution added. pH =

An analytical chemist is titrating 219.9 mL of a 0.5100 M solution of aniline (CH,NH,) with a 0.1800 M solution of HNO,. The p K, of aniline is 9.37. 3 Calculate the pH of the base solution after the chemist has added 360.5 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.

For each of the salts (assume at this point completely soluble), write the equation for dissociation and label the ions as acidic, basic or neutral.Each salt listed will 100% dissociate  NH4C2H3O2 Al2(CO3)3 Na2HPO4 NaI   For each of the following salts, determine the pH of a 2.50M solution of the salt.You will need the Ka and Kb tables to complete this problem.   NaBrO  CH3NH3Cl NaClO2 C6H5OK CsNO3 C6H5NH3Br