General Chemistry: Principles and Modern Applications (11th Edition)
11th Edition
ISBN: 9780132931281
Author: Ralph H. Petrucci, F. Geoffrey Herring, Jeffry D. Madura, Carey Bissonnette
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 17, Problem 20E
You are asked to reduce the pH of the 03001 of buffer solution in Example 17-5 from 5.09 to 5.00 How many milliliters of which of these solutions would you use. 0.100 M NaCI, 0.150 N HCI. 0.100 N NaCH2 COO, 0.125 M NaOH Explain your reasoning.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
What will be the pH of the buffer solution consisting of 94 mL butanoic acid (CH3CH2CH2COOH) 0.189 mol/L and 109 mL sodium butanoate (CH3CH2CH2COONa) 0.207 mol/L, if 10.9 mL KOH 0.5 mol/L is added?Give an answer to at least 3 decimal places.
Give good solution
Asap
Buffer A: CH3COOH 40.0 mL; NaOH 20.0 mL; H2O 20 mL
Buffer B: CH3COOH 40.0 mL; NaOH 30.0 mL; H2O 10 mL
Please identify how the buffer capacity of Buffer A and Buffer B change if the volume of water added was doubled.
And does the the buffer capacity increase, decrease, or remain the same.
Pleas explain why in detail?
Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after the following additions of base:(a) 0 mL(b) 25.00 mL(c) 39.00 mL(d) 39.90 mL(e) 40.00 mL(f ) 40.10 mL(g) 50.00 mL Use the values obtained to sketch a curveof [H₃O⁺] vs. mL of added titrant. Are there advantages or dis-advantages to viewing the results in this form? Explain.
Chapter 17 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
Ch. 17 - For a solution that e 0.275M CH2CH2 COOH...Ch. 17 - For a solution that is 0164 U NH2 and 0.102MNH4Cl...Ch. 17 - Prob. 3ECh. 17 - In Example 16-4, we calculated the percent...Ch. 17 - Calculate [H2OOH-] in a solution that is (a)...Ch. 17 - Calculate [OH-] in a solution that is (a) 0.0062 U...Ch. 17 - What concentration of formate ion, [HCOO-], should...Ch. 17 - What concentration of ammonia. [NH2] , should be...Ch. 17 - Calculate the pH of a buffer that is a. 0.012 M...Ch. 17 - Lactic acid, CH2CH(OH)COOH , is found in sour...
Ch. 17 - Indicate which of the following aqueous solutions...Ch. 17 - The H2PO4-HPO4- combination plays a role in...Ch. 17 - What is the pH of a solution Obtained by adding...Ch. 17 - What the pH of solution prepared by dissolving...Ch. 17 - You wish to prepare a buffer solution w pH = 945...Ch. 17 - You prepare a buffer solution by dissolving 2.00 g...Ch. 17 - If 0.55 ml. of 12 M HCI is added to 0100 L of the...Ch. 17 - If 0.35 mL of 15 P.4 NH is added to 0750 L of the...Ch. 17 - You are asked to prepare e buffer solution why a...Ch. 17 - You are asked to reduce the pH of the 03001 of...Ch. 17 - Given 1.00 L of a solution that is 0.100 hl...Ch. 17 - Given 125mL of a solution that is 0.0500 M CH2NH2...Ch. 17 - A solution of volume 750 mL contars 15.5 mmol...Ch. 17 - A solution of volume 0.500 L contains 1.68 g NH...Ch. 17 - A handbook lets various procedures for preparing...Ch. 17 - An acetic acid-sodium acetate buffer can be...Ch. 17 - A handbook lists the following data: Which of...Ch. 17 - With reference to the indicators listed in...Ch. 17 - In use of acid—base indicators, a. Why is it...Ch. 17 - The indicator methyl red has a pKHIN=4.95 . It...Ch. 17 - Phenol red indicator changes from yellow to red in...Ch. 17 - Thymol blue indicator has two pH ranges. It...Ch. 17 - In the titration of 10.00 mL of 0.04050 M HCI with...Ch. 17 - Solution (a) is 1000 mL of 0.100 N HCI and...Ch. 17 - A 25.00 mL sample of H2PO4(aq) requires 31.15 mL...Ch. 17 - A 2000 ml sample of H2PO4(aq) requires 18.67 mL...Ch. 17 - Two aqueous solutions are mixed 50.0 mL of 0.0150M...Ch. 17 - Two solutions are mixed 100.0 mL of HCI(aq) with...Ch. 17 - Calculate the pH at the points in the titration of...Ch. 17 - Calculate the pH at the points m the titration...Ch. 17 - Calculate the pH at the points in the titration of...Ch. 17 - Calculate the pH at the points lithe titration of...Ch. 17 - Explain why the volume of 0.100 M NeOH required to...Ch. 17 - Explain whether the equivalence point of each of...Ch. 17 - Sketch the titration curves of the following...Ch. 17 - Determine the blowing characteristeristics of the...Ch. 17 - In the titration of 2000 mL of 0175 M NaOH,...Ch. 17 - In the titration of 25.00mL of 0.100M CH2COOH ,...Ch. 17 - Sketch a titration curve (pH versus mL of titrant)...Ch. 17 - Sketch a titration curve (pH versus mL of titrant)...Ch. 17 - For me titration of 25.00 mL of 0.100M NaOH with...Ch. 17 - For the titration of 25.00 mL 0.100M NH2 with...Ch. 17 - Is a solution that is 0.10 M Na2S(aq) likely to be...Ch. 17 - Is a solution of sodium dihydrogen citrate,...Ch. 17 - Sodium phosphate Na2PO4 , is made commecie1y by...Ch. 17 - Both sodium hydrogen carbonate (sodium...Ch. 17 - The pH of a solution of 19.5 g of malonic acid in...Ch. 17 - The ionization constants of ortho-phthalic acid...Ch. 17 - What stoichimetric concentration of the indicated...Ch. 17 - What stocichiometric concentration of the...Ch. 17 - Using appropriate equilibrium constants but...Ch. 17 - Prob. 62ECh. 17 - Sodium hydrogen sulfate NaHSO4 , an acidic salt...Ch. 17 - You are given 250.0mL of 0.100M CH3 CH2 COOH...Ch. 17 - Even though the carbonic acid-hydrogen carbonate...Ch. 17 - Thymol blue in its acid range is not a suitable...Ch. 17 - Rather than calculate the pH for different volumes...Ch. 17 - Use the method of Exercise 67 to determine the...Ch. 17 - A buffer solution can be prepared by starting with...Ch. 17 - You are asked to prepare a KH2PO4-Na2HPO2 solution...Ch. 17 - You are asked to bring the pH of 0.500 L of 0.500...Ch. 17 - Because an acid-base indicator a weak acid, I can...Ch. 17 - The neutralization of NaOH 2by HCl is represented...Ch. 17 - The titration of a weak acid by a weak base a not...Ch. 17 - At times a salt of a we base can be titrated by a...Ch. 17 - Sulfuric acid is a diprotic acid, strong in the...Ch. 17 - Carbonic acid is a weak diprotic acid (H2CO2) with...Ch. 17 - Prob. 78IAECh. 17 - Complete the derivation of equation (17.10)...Ch. 17 - Explain why equation (17.10) fads when applied to...Ch. 17 - Prob. 81IAECh. 17 - Prob. 82IAECh. 17 - Prob. 83IAECh. 17 - Prob. 84IAECh. 17 - Prob. 85IAECh. 17 - Calculate the pH of a solution that is 0.050 U...Ch. 17 - Prob. 87IAECh. 17 - The Henderson-Hasselbalch equation can be written...Ch. 17 - The pH of ocean water depends on the amount of...Ch. 17 - A sample of water contains 23.0 g L1 of Na+ (aq),...Ch. 17 - Prob. 91IAECh. 17 - Prob. 92FPCh. 17 - In some cases the titration curve for a mature of...Ch. 17 - Amino acids contain both an acidic carboxylic acid...Ch. 17 - In your own words, define or explain the following...Ch. 17 - Prob. 96SAECh. 17 - Explain the important distinctions between each...Ch. 17 - Write equations to show how each of the following...Ch. 17 - Sketch the titration curves that you would expect...Ch. 17 - A 2500-mL sample of 0.0100M C8C5COOH (Kg=6.3103)...Ch. 17 - Prob. 101SAECh. 17 - Prob. 102SAECh. 17 - Prob. 103SAECh. 17 - Prob. 104SAECh. 17 - Prob. 105SAECh. 17 - Calculate the pH of a 0.5 M solution of Ca(HSe)2...Ch. 17 - Prob. 107SAECh. 17 - Prob. 108SAECh. 17 - Prob. 109SAECh. 17 - Prob. 110SAECh. 17 - Prob. 111SAE
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
- Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M pyridine with 0.100 M hydrochloric acid (Kb for pyridine is 1.7 109). Do not calculate the points at 24.9 and 25.1 mL.arrow_forwardSelect from Table 15.1 a conjugate acid-base pair that is suitable for preparing a buffer solution whose concentration of hydronium ions is (a) 4.5 103 M. (b) 5.2 108 M. (c) 8.3 106M. (d) 9.7 1011 M. Explain your choices.arrow_forwardcalculate the pH of the buffer 0.15 M NH3/0.35 M NH4Cl without using the Kb valuearrow_forward
- Consider the titration of 25 mL of 0.200 M N2H4 with 0.100 M HCl. Determine the pH of the solution at 20.00, 47.50, and 55.00 mL added HCl solution. pKb for N2H4 is 5.90. You do not have to write the full Kb expression for this problem, but it and other expressions may be helpful.arrow_forwardA sample of 100.00mL of 0.100 M HC2H3O2 is titrated with 0.100 M NaOH. Find the pH of the solution after 38.00 mL of NaOH have been added. For HC2H3O2 Ka=1.8×10-5. Explain, in detail, what steps need to be taken along with the signification of the values that need to be used (formulas, equations, etc.).arrow_forwardThe base dissociation constant for ammonia is 1.8x10-5. If you carry ouit a titration in which you have 25.0 mL of 0.200M ammonia and 0.20M nitric acid, what is the pH at the equivalence point?arrow_forward
- I need help filing in this table and calculating pH and buffer capacity solve this question correctly in 5 min pls Chemicals & Reagents • pH 4.01 and pH 7.00 Standard solutions • 0.1 M Na2HPO4 (sodium phosphate dibasic) • 0.1 M KH2PO4 (potassium phosphate monobasic) • 0.1 M NaOH (sodium hydroxide)arrow_forwardA solution is made by mixing 0.121 mol NaC2H3O2 and 0.098 mol HC2H3O2 (Ka = 2.23 x 10-5) in 0.754 litres of water q1: pH of solution ? q2: Is the pH calculated using the Henderson-Hasselbalch equation an appropriate approximation of the pH for this buffer system?arrow_forwardWhen 30.00 mL of 0.1011 M HCl in 50 mL of deionized water is titrated against 0.09889 M NaOH, the pH increases. Find the pH when the volume of NaOH added is 0.02 mL more than the volume required to reach the equivalence point. Comment on the significance of the changes in pH values in relation to the increments of sodium hydroxide added when going “through” the endpoint.arrow_forward
- Calculate the hydronium ion concentration for a buffer solution that is 2.0 M in maleic acid (H2M) and 1.5 M in potassium hydrogen malanate (KHM) (Ka1=1.20x10-2; Ka2=5.96x10-7). Verify all your assumptions.arrow_forwardCalculate the pH of a 1.26 M solution of a weak BOH, for instace NH4OH, often written as NH3, and 0.21 M of a salt derived by its conjugate acid, BCl, like NH4Cl. The base dissociation constant, Kb , is 2.89e-4. What is the pH if 42 mL of 0.092 M of a strong acid, like HCl, is added to 100 mL of the buffer solution? What if a strong base, like NaOH, is added with the same ammount instead ? pH ← please insert your values Add acid = _______ Add base = _______arrow_forwardWhich of the following solutions represent(s) a buffer solution? Explain.(a) 15 cm3 of 0,1 mol.dm–3 NaOH(b) 15 cm3 of 0,1 mol.dm–3 HC2H3O2(c) 30 cm3 of 0,1 mol.dm–3 NaOH and 30 cm3 of 0,1 mol.dm–3 HC2H3O2(d) 30 cm3 of 0,1 mol.dm–3 NaOH and 60 cm3 of 0,1 mol.dm–3 HC2H3O2arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningWorld of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
World of Chemistry, 3rd edition
Chemistry
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Brooks / Cole / Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
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