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
Videos
Textbook Question
Chapter 17, Problem 72IAE
Because an acid-base indicator a weak acid, I can be titrated with a strong base Suppose you titrated 25.00 mL of a 0.0100 M Solution of the indicator p-nitrophenol.
a. Sketch the titration curve of this titration.
b. Show the pH range over which p-nitrophenol changes color.
c. Explain why p-nitrophenol cannot serve as Is own indicator in this titration.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Will a precipitate (ppt) form when 300.0 mL of 5.0 × 10–5M AgNO3 are added to 200.0 mL of 2.5 × 10–7M NaBr? Answer yes or no, and identify the precipitate if there is one. Ksp(AgBr) = 5.0 × 10–13
Group of answer choices
yes, the ppt is AgNO3(s).
yes, the ppt is NaBr(s).
no, a precipitate will not form.
yes, the ppt is AgBr(s).
yes, the ppt is NaNO3(s).
You have 25.00 mL of a 0.100 M aqueous solution of the weak base (CH3)2NH (Kb = 7.40 x 10-4). This solution will be titrated with 0.100 M HCl.
(a) How many mL of acid must be added to reach the equivalence point?
(b) What is the pH of the solution before any acid is added? (
c) What is the pH of the solution after 10.00 mL of acid has been added?
(d) What is the pH of the solution at the equivalence point of the titration?
(e) What is the pH of the solution when 30.00 mL of acid has been added?
x10
A chemistry graduate student is given 300. mL of a 0.10M acetic acid (HCH,CO₂) solution. Acetic acid is a weak acid with K = 1.8 × 10
KCH3CO2 should the student dissolve in the HCH,CO₂ solution to turn it into a buffer with pH = 4.88?
-5
What mass of
You may assume that the volume of the solution doesn't change when the KCH3CO2 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2
significant digits.
G
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 solution is made up by adding 0.632 g of barium nitrate and 0.920 g of lanthanum nitrate, to La(NO3)3 enough water to make 0.500 L of solution. Solid sodium iodate, NalO3, is added (without volume change) to the solution. (a) Which salt will precipitate first? La(IO3)3 (Ksp=7.501012) or BAIO3 (Ksp=4.0109)? (b) What is [IO3-] when the salt in (a) first begins to precipitate?arrow_forwardAniline hydrochloride, (C6H5NH3)Cl, is a weak acid. (Its conjugate base is the weak base aniline, C6H5NH2.) The acid can be titrated with a strong base such as NaOH. C6H5NH3+(aq)+OH(aq)C6H5NH2(aq)+H2O(l) Assume 50.0 mL of 0.100 M aniline hydrochloride is titrated with 0.185 M NaOH. (Ka for aniline hydrochloride is 2.4 105.) (a) What is the pH of the (C6H5NH3) solution before the titration begins? (b) What is the pH at the equivalence point? (c) What is the pH at the halfway point of the titration? (d) Which indicator in Figure 17.11 could be used to detect the equivalence point? (e) Calculate the pH of the solution after adding 10.0, 20.0, and 30.0 mL of base. (f) Combine the information in parts (a), (b), (c), and (e), and plot an approximate titration curve.arrow_forwardWhen a diprotic acid, H2A, is titrated with NaOH, the protons on the diprotic acid are generally removed one at a time, resulting in a pH curve that has the following generic shape: a. Notice that the plot has essentially two titration curves. If the first equivalence point occurs at 100.0 mL NaOH added, what volume of NaOH added corresponds to the second equivalence point? b. For the following volumes of NaOH added, list the major species present after the OH reacts completely. i. 0 mL NaOH added ii. between 0 and 100.0 mL NaOH added iii. 100.0 mL NaOH added iv. between 100.0 and 200.0 mL NaOH added v. 200.0 mL NaOH added vi. after 200.0 mL NaOH added c. If the pH at 50.0 mL NaOH added is 4.0, and the pH at 150.0 mL NaOH added is 8.0, determine the values Ka1, and Ka2 for the diprotic acid.arrow_forward
- How do the concentrations of Ag+ and CrO42- in a saturated solution above 1.0 g of solid Ag2CrO4 Change when 100 g of solid Ag2CrO4 is added to the system? Explain.arrow_forwardA chemist creates 0.375 L of a 0.18 M acetic acid (CH3COOH) and 0.29 M sodium acetate (CH3COONa) buffer. Note that the Ka of acetic acid is 1.8 x 10-5. (a) Write the chemical equation for how the buffer responds to the addition of HBr. (b) What is the final pH if 0.0060 mol of HBr are added to the buffer solution?arrow_forwardSuppose you have an alkaline buffer consisting of 0.20 M aqueous ammonia (NHs) and 0.10 M ammonium chloride (NH4CI). What is the pH of the solution? 5 Calculate the pH of a 0.350 M solution of potassium phenolate, KC6H5O. Ka for phenol (CH5OH) is 1.0 x 10-10. How do the concentration/volumes of the buffer affect the buffer capacity? E.g., 50.0 mL of 0.10 M acetic acid solution with 50.0 mL of 0.10 M sodium acetate solution vs. the buffer you made in the lab (25.0 mL of 0.10 M acetic acid solution with 25.0 mL of 0.10 M sodium acetate solution).arrow_forward
- The solubility constant of lead (II) hydroxide [Pb(OH)2] is 1.2 x 10-15. If 100.0 g of this compound is dissolved in water what is the concentration of [OH-] and [Pb2+]? If 0.100 M NaOH is added what is the concentration of [OH-] and [Pb2+]?arrow_forwardThe Solubility Product Constant for silver bromide is 3.3 × 10-13. The molar solubility of silver bromide in a 0.249 M sodium bromide solution is M.arrow_forwardWhat mass (in g) of sodium formate, HCOONA, must be added to 10.0 L of a 0.483 Maqueous solution of HCOOH to produce a buffer solution with a pH of 3.40? Ka (HCOOH) = 1.9 x 10-4 O 84.5 O 14.2 O 3.82 O 1.88 157arrow_forward
- A chemistry graduate student is given 125. mL of a 0.20M chlorous acid (HClO₂) solution. Chlorous acid is a weak acid with K=1.1 × 10-2. What mass of KC10, should the student dissolve in the HClO solution to turn it into a buffer with pH = 1.53? You may assume that the volume of the solution doesn't change when the KCIO, is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. C TUarrow_forwardA chemistry graduate student is given 450. mL of a 0.50M methylamine (CH, NH,) solution. Methylamine is a weak base with K=4.4 x 10. What mass of CH,NH, Br should the student dissolve in the CH,NH, solution to turn it into a buffer with pH = 10.96? %3D You may assume that the volume of the solution doesn't change when the CH,NH, Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. Explanation Check 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility MacBook Pro escarrow_forwardThe buffer capacity of a solution may be defined as the number of moles of H+ that will change the pH of 1.00 L of the buffer by 1.00 pH units. What is the buffer capacity of a solution which is 0.10 M in acetic acid (Ka = 1.8 × 10-5) and 0.30 M in sodium acetate, in units of mol (H+) per liter?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY