I need help with 15:21 and 1523 please FOHes thish the samegen ions?eactions:5(e)reactions:ag) + OH (ag)1,0* (aq)ollowingH₂.15.19. What is the conjugate acid of the bisulfate ion, HSO,",and what is its conjugate base?*15.20. Compounds that do not ionize in water have been knownto ionize in nonaqueous solvents. In such a solvent,what would be the conjugate acid and conjugate base ofmethanol, CH,OH?Problems15.21. What is the concentration of H3O+ ions in a 0.65 Msolution of HNO₂?15.22. What is the concentration of H₂O* ions in a solution ofhydrochloric acid that was prepared by diluting 7.5 mL ofconcentrated (11.6 M) HCl to a final volume of 100.0 L?15.23. What is the value of [OH-] in a 0.0205 M solution ofBa(OH)2?15.24. Calcium hydroxide, also known as slaked lime, is thecheapest strong base available and is used in industrialprocesses in which low concentrations of base are required.Only 0.16 g of Ca(OH)₂ dissolves in 100 mL of waterat 25°C. What is the concentration of hydroxide ions in250 mL of a solution containing the maximum amount ofdissolved calcium hydroxide?pH and the Autoionization of WaterConcept Review15.25. Explain why pH values decrease as acidity increases.15.26. Solution A is 100 times more acidic than solution B.What is the difference in the pH values of solution A andsolution B?15.27. Describe a solution (solute and concentration) that has anegative pH value.15.28. Describe a solution (solute and concentration) that has anegative pOH value.*15.29. Draw the Lewis structures of the ions that would beproduced if pure ethanol underwent autoionization.*15.30. Liquid ammonia at a temperature of 223 K undergoesautoionization. The value of the equilibrium constant forthe autoionization of ammonia is considerably less thanthat of water. Write an equatic for the autoionization ofammonia and suggest a reason why the value of K for theprocess is less than that of water.Problems15.31. Calculate the pH and pOH of solutions with the following[H,O*] or [OH-] values. Indicate which solutions areacidic, basic, or neutral.a. [H₂O¹] = 5.3 x 10³ Mb. [H,O*]- 3.8 x 10 Mc. [H₂O*] = 7.2 x 10-6 Md. [OH-] = 1.0 × 10-¹4 M15.32. Calculate the pH and pOH of the solutions with thefollowing hydrogen ion or hydroxide ion concentrations.Indicate which solutions are acidic, basic, or neutral.a. [OH-] = 8.2 x 10-¹¹ Mb. [OH-] = 7.7 x 10-6 Mc. [H₂O¹] = 3.2 × 10-4 Md. [H,O*] 1.0 × 107 Ma. [H,O'] in 8b. [H,O'] in 6c. [OH-] in 4.d. [OH-] in 2.515.34. Determine the ia. pH of a solumb. pH of a solumc. pOH of a solld. pOH of a sol15.35. Calculate the pla. stomach acidb. 0.00500 MHc. a 2:1 mixtured. a 3:1 mixture15.36. Calculate the pHa. 0.0450 M NaCb. 0.160 M Ca(Oc. a 1:1 mixture od. a 2:3 mixture o15.37. Calculate the pH =15.38. Calculate the pH oCalculations Involvi.Concept Review15.39. One-molar solutionsCH₂COOH, HNO-a. Rank them in orcb. Rank them in ord(weakest to strong15.40. On the basis of the fo0.100 M solutions, selAcidC6H5COOHHFHN3CH3COOHD15.41. A 1.0 M aqueous soluticconductor of electricity tExplain why.15.42. Hydrogen chloride and wyet a solution of HCl dissconductor of electricity. E15.43. Hydrofluoric acid is a weaexpression for its acid ioni15.44. Early Antiseptic The use oacid, was pioneered in theLister (after whom Listerinin surgery. Its formula is C,is ionizable. Write the massionization equilibrium of ph*15.45. The K, values of weak acidsthey dissolve. For example, tethanol is less than its & in

We need to find the concentration of H3O+ ions in 0.65 M HNO3. HNO3 is nitric acid and is a strong…

15.21. What is the concentration of H3O+ ions in a 0.65 M solution of HNO₂? 15.22. What is the concentration of H₂O* ions in a solution of hydrochloric acid that was prepared by diluting 7.5 mL of concentrated (11.6 M) HCl to a final volume of 100.0 L? 15.23. What is the value of [OH-] in a 0.0205 M solution of Ba(OH)₂? 15.24 Cal

15.21. What is the concentration of H3O+ ions in a 0.65 M solution of HNO₂? 15.22. What is the concentration of H₂O* ions in a solution of hydrochloric acid that was prepared by diluting 7.5 mL of concentrated (11.6 M) HCl to a final volume of 100.0 L? 15.23. What is the value of [OH-] in a 0.0205 M solution of Ba(OH)₂? 15.24 Cal

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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ASSAY Calibration solutions Calibration solutions of naproxen in the range 5 – 25 μg/mL were prepared. Sample preparation 20 tablets weighing 12.3819 g were crushed to a fine powder. A portion of the powder (145.4 mg) was shaken with approximately 150 mL of acetic acid (0.05 M) for 5 min and then made up to volume in a 250 mL volumetric flask (stock solution). Approximately 50 mL of the stock solution was filtered and a 25 mL aliquot was diluted to 100 mL in a volumetric flask. 10 mL of the resulting solution was further diluted to 100 mL with acetic acid (0.05 M). Analysis The standards and sample solutions were analyzed by HPLC under the following conditions: Column: octadecylsilyl (ODS), 4.6 mmx150 mm, mobile phase: acetonitrile : 0.05 M acetic acid (85:15), flow rate: 1 ml/min, UV detection at 243 nm. Results: A calibration curve of concentration versus peak area was constructed for the standard solutions and gave the straight-line equation: y = 3555.6x + 85, r = 0.9999 The area…
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