Chemistry: Structure and Properties, Books a la Carte PACKAGE W/MasteringChemistry, 2nd Edition
2nd Edition
ISBN: 9780134777559
Author: Tro, Nivaldo J.
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 17, Problem 153E
Interpretation Introduction
To determine:
Derivation of Hendesron-Hasselbach equation.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
The final portion asks for molar solubility.
A chemist titrates 60.0 mL of a 0.8887M butanoic acid (HC,H,CO,) solution with 0.5117M KOH solution at 25 °C.
Calculate the pH at equivalence. The p K, of butanoic acid is 4.82.
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 = ||
A 1.00 liter solution contains 0.48 M ammonia and 0.37 M ammonium iodide. If 0.18 moles of hydrobromic acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydrobromic acid.)
A. The number of moles of NH3 will decrease.
B. The number of moles of NH4+ will decrease.
C. The equilibrium concentration of H3O+ will decrease.
D. The pH will remain the same.
E. The ratio of [NH3] / [NH4+] will decrease.
Chapter 17 Solutions
Chemistry: Structure and Properties, Books a la Carte PACKAGE W/MasteringChemistry, 2nd Edition
Ch. 17 - What is the pH range of human blood? How is human...Ch. 17 - What is a buffer? How does a buffer work? How does...Ch. 17 - What is the common ion effect?Ch. 17 - What is the HendersonHasselbalch equation, and why...Ch. 17 - What is the pH of a buffer when the concentrations...Ch. 17 - Suppose that a buffer contains equal amounts of a...Ch. 17 - How do you use the Henderson—Hasselbalch equation...Ch. 17 - What factors influence the effectiveness of a...Ch. 17 - What is the effective pH range of a buffer...Ch. 17 - Describe acidbase titration. What is the...
Ch. 17 - The pH at the equivalence point of the titration...Ch. 17 - The volume required to reach the equivalence point...Ch. 17 - In the titration of a strong acid with a strong...Ch. 17 - In the titration of a weak acid with a strong...Ch. 17 - The titration of a diprotic acid with sufficiently...Ch. 17 - In the titration of a polyprotic acid, the volume...Ch. 17 - What is the difference between the endpoint and...Ch. 17 - What is an indicator? How can an indicator signal...Ch. 17 - What is the solubility-product constant? Write a...Ch. 17 - What is molar solubility? How do you obtain the...Ch. 17 - How does a common ion affect the solubility of a...Ch. 17 - How is the solubility of an ionic compound with a...Ch. 17 - For a given solution containing an ionic compound,...Ch. 17 - What is selective precipitation? Under which...Ch. 17 - In which of these solutions does HNO2 ionize less...Ch. 17 - A formic acid solution has a pH of 3.25. Which of...Ch. 17 - Solve an equilibrium problem (using an ICE table)...Ch. 17 - Solve an equilibrium problem (using an ICE table)...Ch. 17 - Calculate the percent ionization of a 0.15 M...Ch. 17 - Calculate the percent ionization of a 0.13 M...Ch. 17 - Solve an equilibrium problem (using an ICE table)...Ch. 17 - Solve an equilibrium problem (using an ICE table)...Ch. 17 - A buffer contains significant amounts of acetic...Ch. 17 - A buffer contains significant amounts of ammonia...Ch. 17 - Use the HendersonHasselbalch equation to calculate...Ch. 17 - Use the Henderson—Hasselbalch equation to...Ch. 17 - Use the Henderson—Hasselbalch equation to...Ch. 17 - Use the Henderson—Hasselbaich equation to...Ch. 17 - Calculate the pH of the solution that results from...Ch. 17 - Calculate the pH of the solution that results from...Ch. 17 - Calculate the ratio of NaF to HF required to...Ch. 17 - Calculate the ratio of CH3NH2 to CH3NH3Cl...Ch. 17 - What mass of sodium benzoate should you add to...Ch. 17 - What mass of ammonium chloride should you add to...Ch. 17 - A 250.0-mL buffer solution is 0.250 M in acetic...Ch. 17 - A 100.0-mL buffer solution is 0.175 M in HCIO and...Ch. 17 - For each solution, calculate the initial and final...Ch. 17 - For each solution, calculate the initial and final...Ch. 17 - A 350.0-mL buffer solution is 0.150 in HF and...Ch. 17 - A 100.0-mL buffer solution is 0.100 M ¡n NH3 and...Ch. 17 - Determine whether the mixing of each pair of...Ch. 17 - Determine whether the mixing of each pair of...Ch. 17 - Blood s buffered by carbonic acid and the...Ch. 17 - The fluids within cells are buffered by H2PO4 and...Ch. 17 - Which buffer system is the best choice to create a...Ch. 17 - Which buffer system is the best choice to create a...Ch. 17 - A 500.0-mL buffer solution is 0.100 M in HNO2 and...Ch. 17 - Prob. 58ECh. 17 - The graphs labeled (a) and (b) are the titration...Ch. 17 - Two 25.0-mL samples, one 0.100 M HCI and the other...Ch. 17 - Two 20.0-mL samples, one 0.200 M KOH and the other...Ch. 17 - Prob. 62ECh. 17 - Consider the curve shown here for the titration of...Ch. 17 - Consider the curve shown here for the titration of...Ch. 17 - Consider the titration of a 35.0-mL sample of...Ch. 17 - A 20.0-mL sample of 0.125 M HNO3 is titrated with...Ch. 17 - Consider the titration of a 25.0-mL sample of...Ch. 17 - Prob. 68ECh. 17 - Prob. 69ECh. 17 - Prob. 70ECh. 17 - Consider the titration of a 25.0-mL sample of...Ch. 17 - Prob. 72ECh. 17 - Prob. 73ECh. 17 - Prob. 74ECh. 17 - Prob. 75ECh. 17 - Prob. 76ECh. 17 - Prob. 77ECh. 17 - Prob. 78ECh. 17 - Methyl red has a pKaof 5.0 and is red in its acid...Ch. 17 - Phenolphthalein has a pKaof 9.7. It is colorless...Ch. 17 - Referring to Table 17.1pick an indicator for use...Ch. 17 - Referring to Table 17.1 pick an indicator for use...Ch. 17 - Write balanced equations and expressions for...Ch. 17 - Prob. 84ECh. 17 - Refer to the Kspvalues in Table 17.2 to calculate...Ch. 17 - Prob. 86ECh. 17 - Use the given molar solubilities in pure water to...Ch. 17 - Prob. 88ECh. 17 - Two compounds with general formulas AX and AX2...Ch. 17 - Consider the compounds with the generic formulas...Ch. 17 - Refer to the Ksp value from Table 17.2 to...Ch. 17 - Prob. 92ECh. 17 - Calculate the molar solubility of barium fluoride...Ch. 17 - Prob. 94ECh. 17 - Calculate the molar solubility of calcium...Ch. 17 - Calculate the solubility (in grams per 1.00102 of...Ch. 17 - Is each compound more soluble in acidic solution...Ch. 17 - Is each compound more soluble in acidic solution...Ch. 17 - A solution containing sodium fluoride is mixed...Ch. 17 - A solution containing potassium bromide is mixed...Ch. 17 - Predict whether a precipitate forms if you mix...Ch. 17 - Prob. 102ECh. 17 - Prob. 103ECh. 17 - Prob. 104ECh. 17 - A solution is 0.010 M in Ba2+ and 0.020 M in Ca2+...Ch. 17 - Prob. 106ECh. 17 - A solution is made 1.1103M in Zn(NO3)2 and 0.150 M...Ch. 17 - A 120.0-mL sample of a solution that is 2.8103M in...Ch. 17 - Use the appropriate values of Kspand Kfto find the...Ch. 17 - Prob. 110ECh. 17 - A 1.500-mL solution contains 2.05 g of sodium...Ch. 17 - A solution ¡s made by combining 10.0 ml of 17.5 M...Ch. 17 - A buffer is created by combining 150.0 mL of 0.25...Ch. 17 - A buffer is created by combining 3.55 g of NH3...Ch. 17 - A 1.0-L buffer solution initially contains 0.25...Ch. 17 - A 250.0-mL buffer solution initially contains...Ch. 17 - In analytical chemistry, bases used for titrations...Ch. 17 - A 0.5224-g sample of an unknown monoprotic acid...Ch. 17 - A 0.25-mol sample of a weak acid with an unknown...Ch. 17 - A 5.55-g sample of a weak acid with Ka=1.3104 is...Ch. 17 - A 0.552-g sample of ascorbic acid (vitamin C) is...Ch. 17 - Sketch the titration curve from Problem 121by...Ch. 17 - One of the main components of hard water is CaCO3....Ch. 17 - Gout—a condition that results in joint swelling...Ch. 17 - Pseudogout, a condition with symptoms similar to...Ch. 17 - Calculate the solubility of silver chloride in a...Ch. 17 - Calculate the solubility of CuX ¡n a solution that...Ch. 17 - Aniline, C6H5NH2, is an important organic base...Ch. 17 - The Kbof hydroxylamine, NH2OH is 1.0108 . A buffer...Ch. 17 - Prob. 130ECh. 17 - Prob. 131ECh. 17 - Prob. 132ECh. 17 - What relative masses of dimethyl amine and...Ch. 17 - You are asked to prepare 2.0 L of a HCN/NaCN...Ch. 17 - Prob. 135ECh. 17 - Prob. 136ECh. 17 - Prob. 137ECh. 17 - Prob. 138ECh. 17 - When excess solid Mg(OH)2 is shaken with 1.00 L of...Ch. 17 - Prob. 140ECh. 17 - Calculate the solubility of Au(OH)3 in (a) water...Ch. 17 - Calculate the concentration of I in a solution...Ch. 17 - Prob. 143ECh. 17 - Prob. 144ECh. 17 - Find the pH of a solution prepared from 1.0 L of a...Ch. 17 - Prob. 146ECh. 17 - Prob. 147ECh. 17 - Prob. 148ECh. 17 - Consider three solutions: 0.10 M solution of a...Ch. 17 - Prob. 150ECh. 17 - Prob. 151ECh. 17 - Prob. 152ECh. 17 - Prob. 153ECh. 17 - Prob. 154ECh. 17 - A certain town gets its water from an underground...Ch. 17 - Prob. 156ECh. 17 - Prob. 157ECh. 17 - A buffer is 0.100 M in NH4CI and 0.100 M in NH3....Ch. 17 - What is the pH of a buffer that is 0.120 M in...Ch. 17 - Prob. 3SAQCh. 17 - Prob. 4SAQCh. 17 - Prob. 5SAQCh. 17 - Prob. 6SAQCh. 17 - Prob. 7SAQCh. 17 - A 10.0-mL sample of 0.200 M hydrocyanic acid (HCN)...Ch. 17 - Prob. 9SAQCh. 17 - Prob. 10SAQCh. 17 - Prob. 11SAQCh. 17 - Prob. 12SAQCh. 17 - Calculate the molar solubility of magnesium...Ch. 17 - Prob. 14SAQCh. 17 - Prob. 15SAQ
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- A 1.00 liter solution contains 0.54 M ammonia and 0.42 M ammonium chloride. If 0.21 moles of hydrobromic acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydrobromic acid.) vA. The number of moles of NH3 will increase. v B. The number of moles of NH.* will remain the same. v C. The equilibrium concentration of H3O* will increase. vD. The pH will decrease. E. The ratio of [NH3] / [NH4*] will decrease.arrow_forwardDefine pH buffers and discuss the effect of dilution. Discuss the effect of addition of acids or bases to a buffer solution.arrow_forwardA chemist titrates 180.0 mL of a 0.8675 M trimethylamine ((CH,) N) solution with 0.4585 M HCl solution at 25 °C. Calculate the pH at equivalence. The p K, of trimethylamine is 4.19. 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 HCl solution added. pH =arrow_forward
- Derive the Henderson- Hasselbalch equation for the dissociation of a weak base, B, in terms of pOH and pKb.arrow_forwardConsider the generic dissociation equation... HA + H2O →H3O* + A¯ ..where HA is a weak acid Based on what you know about buffers, explain in detail how this reaction acts as an acid buffer to keep the pH of the solution constant even when a strong acid is added to the solution. Your answer should refer to the reaction above to discuss buffers, how they work, why strong acids/bases cannot be used as buffers, and how Le Chatelier's principle impacts why buffers work.arrow_forwardA buffer system is prepared by combining 0.603 moles of ammonium chloride (NH4CI) and 0.713 moles of ammonia (NH3). What will the solution pH be if 0.239 moles of the nitric acid (HNO3) is added to the solution. Nitric acid is a strong acid. The K₁ of ammonia is 1.8 x 10-5. (Two decimal places)arrow_forward
- You have a 15 mL sample of acetylcholine (a neurotransmitter) with an unknown concentration and a pH of 8.06. You incubate this sample with the enzyme acetylcholinesterase to convert all of the acetylcholine to choline and acetic acid. The acetic acid dissociates to yield acetate and hydrogen ions. At the end of the incubation period, you measure the pH again and find that it has decreased to 5.91. Assuming there was no buffer in the assay mixture, determine the number of nanomoles of acetylcholine in the original 15 mL sample. O= CH3 Acetylcholine H₂O CH,—C−O−CH,—CH,—*N-CH, → HO−CH,—CH,—*N–CH, + CH,—C−O + H* CH3 CH 3 Choline CH3 Acetatearrow_forwardAn analytical chemist is titrating 239.7 mL of a 0.6100M solution of benzoic acid (HC,H,CO, with a 0.4400M solution of NaOH. The p K, of benzoic acid is 4.20. Calculate the pH of the acid solution after the chemist has added 135.5 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = Uarrow_forwardA chemist titrates 90.0 mL of a 0.8026 M ethylamine (C,H,NH,) solution with 0.7461 M HCl solution at 25 °C. Calculate the pH at equivalence. The p K, 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 HCl solution added. PH = [| %3Darrow_forward
- For biological buffer systems, buffer acids capacity is usually greater than buffer bases capacity. Why?arrow_forwardCalculating the pH at equivalence of a titration A chemist titrates 230.0 mL of a 0.3847 M hydrocyanic acid (HCN) solution with 0.2111 M NAOH solution at 25 °C. Calculate the pH at equivalence. The p K, 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. olo pH = Ararrow_forwardYou have a 11 mL sample of acetylcholine (a neurotransmitter) with an unknown concentration and a pH of 8.22. You incubate this sample with the enzyme acetylcholinesterase to convert all of the acetylcholine to choline and acetic acid. The acetic acid dissociates to yield acetate and hydrogen ions. At the end of the incubation period, you measure the pH again and find that it has decreased to 6.62. Assuming there was no buffer in the assay mixture, determine the number of nanomoles of acetylcholine in the original 11 mL sample. CH,—C−O−CH,—CH,—*N-CH, Acetylcholine CH3 acetycholine in original sample: I CH₂ H₂O CH₂ HO–CH,—CH,—*N–CH, + CH,-C−O + H* CH₂-8-0 Choline | CH3 Acetate nmolarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
Acid-Base Titration | Acids, Bases & Alkalis | Chemistry | FuseSchool; Author: FuseSchool - Global Education;https://www.youtube.com/watch?v=yFqx6_Y6c2M;License: Standard YouTube License, CC-BY