Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- Determine the pH at the equivalence point in the titration of 50.0 mL of 0.300 M CH₃COOH with 0.300 M NaOH. The value of Ka for CH₃COOH is 1.8 × 10⁻⁵. Use the table below to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction.arrow_forwardDetermine the pH of the solution (to 2 decimal points) after the addition of 25.7 mL of 0.0103 M calcium hydroxide (Ca(OH)2) to 719 mL of 0.0173 M pyridinium chloride (C5H5NHCl).Assume that the volumes are additive and that the 5% approximation is valid. pKa = 5.25arrow_forwardCalculating the pH at equivalence of a titration A chemist titrates 50.0 mL of a 0.5851 M ethylamine (C2H5NH2) solution with 0.8192M HBr solution at 25 °C. Calculate the pH at equivalence. The pK of ethylamine is 3.19. b 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 = ] ☑arrow_forward
- Calculating the pH at equivalence of a titration A chemist titrates 170.0 mL of a 0.2614M cyanic acid (HCNO) solution with 0.7980M NaOH solution at 25 °C. Calculate the pH at equivalence. The p K, 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 NAOH solution added. pH =arrow_forwardHow many moles of sodium hypobromite, NaBrO, should be added to 1.00 L of 0.396 M hypobromous acid, HBrO, to form a buffer solution of pH 8.95? The Ka of HOBr is 2.0 × 10–9. Express your answer in moles using at least three significant figures. Do not use scientific notation.arrow_forwardA chemist titrates 60.0 mL of a 0.7169M lidocaine (C14H2|NONH) solution with 0.4965 M HNO, solution at 25 °C. Calculate the pH at equivalence. The p Kb 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 HNO, solution added. pH %3Darrow_forward
- An analytical chemist is titrating 154.7mL of a 0.2900M solution of dimethylamine CH32NH with a 0.3400M solution of HNO3. The pKb of dimethylamine is 3.27 . Calculate the pH of the base solution after the chemist has added 155.7mL of the HNO3 solution to it. Round your answer to 2 decimal places.arrow_forwardAn analytical chemist is titrating 167.0mL of a 0.8000M solution of methylamine CH3NH2 with a 0.2800M solution of HIO3. The pKb of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 140.1mL of the HIO3 solution to it.Round your answer to 2 decimal places.arrow_forwardA 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 ?arrow_forward
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