A chemist titrates 190.0 mL of a 0.5359 M hydrobromic acid (HBr) solution with 0.2938M KOH 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 KOH solution added. pH = 0 %3D Submit Assi Continue O 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center Ace MacBook Air

A chemist titrates 190.0 mL of a 0.5359 M hydrobromic acid (HBr) solution with 0.2938M KOH 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 KOH solution added. pH = 0 %3D Submit Assi Continue O 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center Ace MacBook Air

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Can you please do A and B thank you!
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A 10.0 mL solution of 0.570 M NH3 is titrated with a 0.190 M HCl solution. Calculate the pH after the following additions of the HCl solution: 0.00 mL, 10.0 mL, 30.0 mL, and 40.0 mL. Round your answer to 3 decimal places. Note: Reference the K of acids at 25 °C and K₁ of bases at 25 °C tables for additional information. b Part 1 of 4 0.00 mL Added, pH = ☐ x10 Part 2 of 4 10.0 mL Added, pH = ☐ ☐ x10 Part 3 of 4 ☑ ✓ G
A chemist titrates 210.0 mL of a 0.7303M potassium hydroxide (KOH) solution with 0.0877M HNO3 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 HNO3 solution added. pH = X
A chemist titrates 160.0 mL of a 0.3349M cyanic acid (HCNO) solution with 0.3751 M KOH solution at 25 °C. Calculate the pH at equivalence. The pK of cyanic acid is 3.46. 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 = X S ?
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A chemist titrates 80.0 mL. of a 0.0754 M aniline (C6H5NH2) solution with 0.5961 M HBr solution at 25 °C. Calculate the pH at equivalence. The pKa 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.
You are given a solution that contains a mixture of two weak acids. You take a 50.00 mL sample of the mixture and titrate it with 0.1000M NaOH using a pH meter. You obtain the data shown in the plot below. 12 10 8 6 4 2 0 0 5 Titration of a mixture 10 15 vol (mL) NaOH added 20 25 30 Determine the first and second equivalence volumes. Use the equivalence volumes to determine how many moles of NaOH was used to titrate each acid. Use those values to determine the concentration of each acid in the original mixture. Finally, estimate the pKa values for each acid from the plot. Show your calculations and explain any choices you have made.
A chemist titrates 180.0 mL of a 0.3545M ammonia (NH3) solution with 0.7205M HBr 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. -0 pH = X
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