Homework Answers
As HBr & NaOH both are strong electrolyte so dissociation happens complete And equivalence point is defined as the point when all of acis just got reacted with base so at equivalence point solution is neither acidic or base so during titration of strong acid vs strong base equivalence point is neutral so Ph = 7
Ans Ph =7
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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...
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...
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. Calc...
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...
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...
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...
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...
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...
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...
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...
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 ?
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 ?
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