HBr + NaOH -----------> NaBr + H2O
HBr is strong acid
NaOH is s trong base
strong acid strong base titration
at equivalence point pH = 7.0 always
pH = 7.0
A chemist titrates 100.0 ml of a 0.4488 M hydrobromic acid (HBr) solution with 0.7668 M...
A chemist titrates 100.0 ml of a 0.4488 M hydrobromic acid (HBr) solution with 0.7668 M NaOH solution at 25°C. Calculate the pH at equivalence. 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 NaOH solution added. PHO 5 ?
A chemist titrates 100.0 mL of a 0.3204 M ammonia (NH) solution with 0.7322 MHBr 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 HBr solution added. PHO X 5 ?
A chemist titrates 100.0 ml of a 0,6612 M hydrocyanic acid (HCN) solution with 0.8512 M NaOH solution at 25 c. Calculate the pH at equivalence. The pk, of hydrocyanic acid is 9.21. 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 N.OH solution added. pH- x 5 ?
A chemist titrates 190.0 mL of a 0.4393 M hydrochloric acid (HCI) solution with 0.1456 M NaOH solution at 25 °C. Calculate the pH at equivalence. 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 NaOH solution added. pH = [] Х 5 ? Calculating the pH of a weak acid titrated with a strong base An analytical chemist is titrating...
A chemist titrates 250.0 mL of a 0.5659 M lidocaine (C14H21NONH) solution with 0.4276 M HBr solution at 25 °C. Calculate the pH at equivalence. The pK, of lidocaine is 7.94. 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 HBr solution added. PH -
A chemist titrates 200.0 mL of a 0.7681 M hydrocyanic acid (HCN) solution with 0.5271 M NaOH solution at 25 °C. Calculate the pH at equivalence. The pk of hydrocyanic acid is 9.21. 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 NaOH solution added. pH- х ?
A chemist titrates 160.0 mL of a 0.3337 M carbonic acid (H2CO3) solution with 0.4095 M NaOH solution at 25 °C. Calculate the pH at equivalence. The pK, of carbonic acid is 3.60. 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 NaOH solution added.
A chemist titrates 140.0 mL of a 0.0952 M aniline (CGH-NH2) solution with 0.7849 M HBr solution at 25 °C. Calculate the pH at equivalence. The pK; 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 HBr solution added.
A chemist titrates 140.0 ml of a 0.8665 Methylamine (C,H,NH,) solution with 0.5484 M HBr solution at 25 °C. Calculate the pH at equivalence. The pky of ethylamine is 3.19. 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 HBr solution added.
A chemist titrates 190.0 mL of a 0.4427 Macetic acid (HCH,CO, solution with 0.2382 M NaOH solution at 25 "C. Calculate the pH at equivalence. The pk of acetic acid is 4.76. 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 NaOH solution added. pH = 0 x 5 ?