Bundle: General Chemistry, Loose-leaf Version, 11th + OWLv2, 4 terms (24 months) Printed Access Card
11th Edition
ISBN: 9781337128391
Author: Darrell Ebbing, Steven D. Gammon
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 16, Problem 16.16QP
If the pH is 8.0 at the equivalence point for the titration of a certain weak acid with sodium hydroxide, what indicator might you use? (See Figure 15.10.) Explain your choice.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Chapter 16 Solutions
Bundle: General Chemistry, Loose-leaf Version, 11th + OWLv2, 4 terms (24 months) Printed Access Card
Ch. 16.1 - Lactic acid, HC3H5O3, is found in sour milk, where...Ch. 16.1 - What are the concentrations of hydrogen ion and...Ch. 16.1 - What is the pH of an aqueous solution that is...Ch. 16.1 - You have prepared dilute solutions of equal molar...Ch. 16.2 - Sulfurous acid, H2SO3, is a diprotic acid with Ka1...Ch. 16.3 - Quinine is an alkaloid, or naturally occurring...Ch. 16.3 - What is the hydronium-ion concentration of a 0.20...Ch. 16.3 - Prob. 16.2CCCh. 16.4 - Consider solutions of the following salts: a....Ch. 16.4 - Calculate the following at 25C, using Tables 16.1...
Ch. 16.4 - Benzoic acid, HC7H5O2, and its salts are used as...Ch. 16.4 - Which of the following aqueous solutions has the...Ch. 16.5 - The chemical equation for the hydrolysis of...Ch. 16.5 - What is the concentration of formate ion, CHO2, in...Ch. 16.5 - One liter of solution was prepared by dissolving...Ch. 16.6 - What is the pH of a buffer prepared by adding 30.0...Ch. 16.6 - Suppose you add 50.0 mL of 0.10 M sodium hydroxide...Ch. 16.6 - Prob. 16.5CCCh. 16.6 - The beaker on the left below represents a buffer...Ch. 16.7 - What is the pH of a solution in which 15 mL of...Ch. 16.7 - What is the pH at the equivalence point when 25 mL...Ch. 16.7 - Prob. 16.16ECh. 16 - Write an equation for the ionization of hydrogen...Ch. 16 - Prob. 16.2QPCh. 16 - Briefly describe two methods for determining Ka...Ch. 16 - Describe how the degree of ionization of a weak...Ch. 16 - Prob. 16.5QPCh. 16 - Phosphorous acid, H2PHO3, is a diprotic acid....Ch. 16 - Prob. 16.7QPCh. 16 - Write the equation for the ionization of aniline,...Ch. 16 - Which of the following is the strongest base: NH3,...Ch. 16 - Do you expect a solution of anilinium chloride...Ch. 16 - Prob. 16.11QPCh. 16 - The pH of 0.10 M CH3NH2 (methylamine) is 11.8....Ch. 16 - Define the term buffer. Give an example.Ch. 16 - What is meant by the capacity of a buffer?...Ch. 16 - Prob. 16.15QPCh. 16 - If the pH is 8.0 at the equivalence point for the...Ch. 16 - Which of the following salts would produce the...Ch. 16 - If you mix 0.10 mol of NH3 and 0.10 mol of HCl in...Ch. 16 - Hydrogen sulfide, H2S, is a very weak diprotic...Ch. 16 - If 20.0 mL of a 0.10 M NaOH solution is added to a...Ch. 16 - Aqueous Solutions of Acids, Bases, and Salts a For...Ch. 16 - The pH of Mixtures of Acid, Base, and Salt...Ch. 16 - Which of the following beakers best represents a...Ch. 16 - You have 0.10-mol samples of three acids...Ch. 16 - Prob. 16.25QPCh. 16 - You have the following solutions, all of the same...Ch. 16 - Prob. 16.27QPCh. 16 - A chemist prepares dilute solutions of equal molar...Ch. 16 - Prob. 16.29QPCh. 16 - Prob. 16.30QPCh. 16 - You are given the following acidbase titration...Ch. 16 - The three flasks shown below depict the titration...Ch. 16 - Write chemical equations for the acid ionizations...Ch. 16 - Write chemical equations for the acid ionizations...Ch. 16 - Acrylic acid, whose formula is HC3H3O2 or...Ch. 16 - Heavy metal azides, which are salts of hydrazoic...Ch. 16 - Boric acid, B(OH)3, is used as a mild antiseptic....Ch. 16 - Formic acid, HCHO2, is used to make methyl formate...Ch. 16 - C6H4NH2COOH, para-aminobenzoic acid (PABA), is...Ch. 16 - Barbituric acid. HC4H3N2O3, is used to prepare...Ch. 16 - A solution of acetic acid, HC2H3O2, on a...Ch. 16 - A chemist wanted to determine the concentration of...Ch. 16 - Hydrofluoric acid, HF, unlike hydrochloric acid,...Ch. 16 - Chloroacetic acid, HC2H2ClO2, has a greater acid...Ch. 16 - What is the hydronium-ion concentration of a 2.00...Ch. 16 - What is the hydronium-ion concentration of a 3.00 ...Ch. 16 - Phthalic acid, H2C8H4O4, is a diprotic acid used...Ch. 16 - Carbonic acid, H2CO3, can be found in a wide...Ch. 16 - Write the chemical equation for the base...Ch. 16 - Write the chemical equation for the base...Ch. 16 - Butylamine, C4H3NH2 is a weak base. A 0.47 M...Ch. 16 - Trimethylamine, (CH3)3N, is a gas with a fishy,...Ch. 16 - What is the concentration of hydroxide ion in a...Ch. 16 - What is the concentration of hydroxide ion in a...Ch. 16 - Note whether hydrolysis occurs for each of the...Ch. 16 - Note whether hydrolysis occurs for each of the...Ch. 16 - Prob. 16.57QPCh. 16 - Prob. 16.58QPCh. 16 - For each of the following salts, indicate whether...Ch. 16 - Note whether the aqueous solution of each of the...Ch. 16 - Decide whether solutions of the following salts...Ch. 16 - Decide whether solutions of the following salts...Ch. 16 - Obtain a the Kb value for NO2; b the Ka value for...Ch. 16 - Prob. 16.64QPCh. 16 - What is the pH of a 0.025 M aqueous solution of...Ch. 16 - Calculate the OH concentration and pH of a 0.0025...Ch. 16 - Calculate the concentration of pyridine, C5H5N, in...Ch. 16 - What is the pH of a 0.30 M solution of...Ch. 16 - Calculate the degree of ionization of a 0.75 M HF...Ch. 16 - Calculate the degree of ionization of a 0.22 M...Ch. 16 - What is the pH of a solution that is 0.600 M HCHO2...Ch. 16 - What is the pH of a solution that is 0.20 M KOCN...Ch. 16 - What is the pH of a solution that is 0.10 M CH3NH2...Ch. 16 - What is the pH of a solution that is 0.15 M...Ch. 16 - A buffer is prepared by adding 39.8 mL of 0.75 M...Ch. 16 - A buffer is prepared by adding 115 mL of 0.30 M...Ch. 16 - What is the pH of a buffer solution that is 0.10 M...Ch. 16 - A buffer is prepared by mixing 525 mL of 0.50 M...Ch. 16 - What is the pH of a buffer solution that is 0.15 M...Ch. 16 - What is the pH of a buffer solution that is 0.10 M...Ch. 16 - What is the pH of a buffer solution that is 0.15 M...Ch. 16 - What is the pH of a buffer solution that is 0.15 M...Ch. 16 - How many moles of sodium acetate must be added to...Ch. 16 - How many moles of hydrofluoric acid, HF, must be...Ch. 16 - What is the pH of a solution in which 15 mL of...Ch. 16 - What is the pH of a solution in which 35 mL of...Ch. 16 - A 1.24-g sample of benzoic acid was dissolved in...Ch. 16 - A 0.400-g sample of propionic acid was dissolved...Ch. 16 - Find the pH of the solution obtained when 32 mL of...Ch. 16 - What is the pH at the equivalence point when 22 mL...Ch. 16 - A 50.0-mL sample of a 0.100 M solution of NaCN is...Ch. 16 - Sodium benzoate, NaC7H5O2, is used as a...Ch. 16 - Calculate the pH of a solution obtained by mixing...Ch. 16 - Calculate the pH of a solution obtained by mixing...Ch. 16 - Salicylic acid, C6H4OHCOOH, is used in the...Ch. 16 - Cyanoacetic acid, CH2CNCOOH, is used in the...Ch. 16 - A 0.050 M aqueous solution of sodium hydrogen...Ch. 16 - A 0.10 M aqueous solution of sodium dihydrogen...Ch. 16 - Prob. 16.99QPCh. 16 - Calculate the base-ionization constants for PO43...Ch. 16 - Calculate the pH of a 0.072 M aqueous solution of...Ch. 16 - Calculate the pH of a 0.10 M aqueous solution of...Ch. 16 - An artificial fruit beverage contains 11.0 g of...Ch. 16 - A buffer is made by dissolving 12.5 g of sodium...Ch. 16 - Blood contains several acid base systems that tend...Ch. 16 - Codeine, C23H21NO3, is an alkaloid (Kb = 6 2 109)...Ch. 16 - Calculate the pH of a solution obtained by mixing...Ch. 16 - Calculate the pH of a solution made up from 2.0 g...Ch. 16 - Find the pH of the solution obtained when 25 mL of...Ch. 16 - What is the pH of the solution obtained by...Ch. 16 - Ionization of the first proton from H2SO4 is...Ch. 16 - Ionization of the first proton from H2SeO4 is...Ch. 16 - Methylammonium chloride is a salt of methylamine,...Ch. 16 - Sodium benzoate is a salt of benzoic acid,...Ch. 16 - Each of the following statements concerns a 0.010...Ch. 16 - Each of the following statements concerns a 0.10 M...Ch. 16 - A 0.288-g sample of an unknown monoprotic organic...Ch. 16 - A 0.239-g sample of unknown organic base is...Ch. 16 - a Draw a pH titration curve that represents the...Ch. 16 - a Draw a pH titration curve that represents the...Ch. 16 - The equilibrium equations and Ka values for three...Ch. 16 - Prob. 16.122QPCh. 16 - A 25.0-mL sample of hydroxylamine is titrated to...Ch. 16 - A 25.00-mL sample contains 0.562 g of NaHCO3. This...Ch. 16 - A solution made up of 1.0 M NH3 and 0.50 M...Ch. 16 - A solution is prepared from 0.150 mol of formic...Ch. 16 - An important component of blood is the buffer...Ch. 16 - An important component of blood is the buffer...Ch. 16 - Tartaric acid is a weak diprotic fruit acid with...Ch. 16 - Malic acid is a weak diprotic organic acid with...Ch. 16 - A quantity of 0.25 M sodium hydroxide is added to...Ch. 16 - A quantity of 0.15 M hydrochloric acid is added to...Ch. 16 - Prob. 16.133QPCh. 16 - Prob. 16.134QPCh. 16 - A 30.0-mL sample of 0.05 M HClO is titrated by a...Ch. 16 - Prob. 16.136QPCh. 16 - Prob. 16.137QPCh. 16 - Calculate the pH of a solution made by mixing 0.62...Ch. 16 - Cyanic acid, HOCN, is a weak acid with a Ka value...Ch. 16 - The Kb for NH3 is 1.8 105 at 25C. Calculate the...Ch. 16 - Ka for formic acid is 1.7 104 at 25C. A buffer is...Ch. 16 - K4 for acetic acid is 1.7 105 at 25C. A buffer...Ch. 16 - Prob. 16.143QPCh. 16 - Prob. 16.144QPCh. 16 - Prob. 16.145QPCh. 16 - Two samples of 1.00 M HCl of equivalent volumes...Ch. 16 - Prob. 16.147QPCh. 16 - Prob. 16.148QPCh. 16 - A solution of weak base is titrated to the...Ch. 16 - A buffer solution is prepared by mixing equal...Ch. 16 - The pH of a white vinegar solution is 2.45. This...Ch. 16 - The pH of a household cleaning solution is 11.50....Ch. 16 - What is the freezing point of 0.92 M aqueous...Ch. 16 - Prob. 16.154QPCh. 16 - A chemist needs a buffer with pH 4.35. How many...Ch. 16 - A chemist needs a buffer with pH 3.50. How many...Ch. 16 - Weak base B has a pKb of 6.78 and weak acid HA has...
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
- What is the pH of a buffer that is 0.150 M in a weak acid and 0.150 M in the acids conjugate base? The acids ionization constant is 6.8 106.arrow_forwardA solution of weak base is titrated to the equivalence point with a strong acid. Which one of the following statements is most likely to be correct? a The pH of the solution at the equivalence point is 7.0. b The pH of the solution is greater than 13.0. c The pH of the solution is less than 2.0. d The pH of the solution is between 2.0 and 7.0. e The pH of the solution is between 7.0 and 13.0. The reason that best supports my choosing the answer above is a Whenever a solution is titrated with a strong acid, the solution will be very acidic. b Because the solution contains a weak base and the acid (titrant) is used up at the equivalence point, the solution will be basic. c Because the solution contains the conjugate acid of the weak base at the equivalence point, the solution will be acidic.arrow_forwardA 0.239-g sample of unknown organic base is dissolved in water and titrated with a 0.135 M hydrochloric acid solution. After the addition of 18.35 mL of acid, a pH of 10.73 is recorded. The equivalence point is reached when a total of 39.24 mL of HCl is added. The base and acid combine in a 1:1 ratio. a What is the molar mass of the organic base? b What is the Kb value for the base? The Kb value could have been determined very easily if a pH measurement had been made after the addition of 19.62 mL of HCl. Why?arrow_forward
- A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution but reverses the two solutions and places the weak acid solution in the buret. After 23.75 mL of the weak acid solution has been added to 50.0 mL of the 0.100 M NaOH solution, the pH of the resulting solution is 10.50. Calculate the original concentration of the solution of weak acid.arrow_forwardA solution made up of 1.0 M NH3 and 0.50 M (NH4)2SO4 has a pH of 9.26. a Write the net ionic equation that represents the reaction of this solution with a strong acid. b Write the net ionic equation that represents the reaction of this solution with a strong base. c To 100. mL of this solution, 10.0 mL of 1.00 M HCl is added. How many moles of NH3 and NH4+ are present in the reaction system before and after the addition of the HCl? What is the pH of the resulting solution? d Why did the pH change only slightly upon the addition of HCl?arrow_forwardA quantity of 0.25 M sodium hydroxide is added to a solution containing 0.15 mol of acetic acid. The final volume of the solution is 375 mL and the pH of this solution is 4.45. a What is the molar concentration of the sodium acetate? b How many milliliters of sodium hydroxide were added to the original solution? c What was the original concentration of the acetic acid?arrow_forward
- a Draw a pH titration curve that represents the titration of 50.0 mL of 0.10 M NH3 by the addition of 0.10 M HCl from a buret. Label the axes and put a scale on each axis. Show where the equivalence point and the buffer region are on the titration curve. You should do calculations for the 0%, 30%, 50%, and 100% titration points. b Is the solution neutral, acidic, or basic at the equivalence point? Why?arrow_forwardA quantity of 0.15 M hydrochloric acid is added to a solution containing 0.10 mol of sodium acetate. Some of the sodium acetate is converted to acetic acid, resulting in a final volume of 650 mL of solution. The pH of the final solution is 4.56. a What is the molar concentration of the acetic acid? b How many milliliters of hydrochloric acid were added to the original solution? c What was the original concentration of the sodium acetate?arrow_forwardBriefly describe how a buffer solution can control the pH of a solution when strong acid is added and when strong base is added. Use NH3/NH4Cl as an example of a buffer and HCl and NaOH as the strong acid and strong base.arrow_forward
- Consider all acid-base indicators discussed in this chapter. Which of these indicators would be suitable for the titration of each of these? (a) NaOH with HClO4 (b) acetic acid with KOH (c) NH3 solution with HBr (d) KOH with HNO3 Explain your choices.arrow_forwardWhich of these combinations is the best to buffer the pH at approximately 9? Explain your choice. CH3COOH/NaCH3COO HCl/NaCl NH3/NH4Clarrow_forwardA 25.0-mL sample of hydroxylamine is titrated to the equivalence point with 35.8 mL of 0.150 M HCl. a What was the concentration of the original hydroxylamine solution? b What is the pH at the equivalence point? c Which indicators, bromphenol blue, methyl red, or phenolphthalein, should be used to detect the end point of the titration? Why?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
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 Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
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