![OWLv2 for Ebbing/Gammon's General Chemistry, 11th Edition, [Instant Access], 1 term (6 months)](https://s3.amazonaws.com/compass-isbn-assets/textbook_empty_images/large_textbook_empty.svg)
OWLv2 for Ebbing/Gammon's General Chemistry, 11th Edition, [Instant Access], 1 term (6 months)
11th Edition
ISBN: 9781305673939
Author: Darrell Ebbing; Steven D. Gammon
Publisher: Cengage Learning US
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 16, Problem 16.78QP
A buffer is prepared by mixing 525 mL of 0.50 M formic acid, HCHO2, and 475 mL of 0.50 M sodium formate, NaCHO2. Calculate the pH. What would be the pH of 85 mL of the buffer to which 8.6 mL of 0.15 M hydrochloric acid had been added?
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
A buffer solution is formed by adding 0.180 moles of solid potassium nitrite, KNO₂, to 200.0 ml of 0.600 M Nitrous acid, HNO₂ solution. You may assume that the change in volume is negligible upon addition of the solid.
Calculate the pH of the buffer solution.pH = AnswerCalculate the pH of the buffer solution after the addition of 8.00 ml of 1.50 M HCl.pH = Answer
A buffer solution is formed by adding 0.320 moles of solid sodium lactate, NaC₃H₅O₃, to 600.0 ml of 0.600 M lactic acid, HC₃H₅O₃ solution. You may assume that the change in volume is negligible upon addition of the solid. Calculate the pH of the buffer solution.pH = Answer Calculate the pH of the buffer solution after the addition of 6.00 ml of 5.00 M HCl. pH = Answer
A buffer solution is formed by adding 0.150 moles of solid strontium acetate, Sr(C₂H₃O₂)₂, to 500.0 ml of 0.400 M acetic acid, HC₂H₃O₂ solution. You may assume that the change in volume is negligible upon addition of the solid.Calculate the pH of the buffer solution.Calculate the pH of the buffer solution after the addition of 7.50 ml of 2.00 M NaOH.
Acetic Acid: pKa = 4.75
Ka=1.76E-5
M.w.=60.05 g/mol
Chapter 16 Solutions
OWLv2 for Ebbing/Gammon's General Chemistry, 11th Edition, [Instant Access], 1 term (6 months)
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
- Ka for formic acid is 1.7 104 at 25C. A buffer is made by mixing 529 mL of 0.465 M formic acid, HCHO2, and 494 mL of 0.524 M sodium formate, NaCHO2. Calculate the pH of this solution at 25C after 110 mL of 0.152 M HCl has been added to this buffer.arrow_forwardThe titration of 0.100 M acetic acid with 0.100 M NaOH is described in the text. What is the pH of the solution when 35.0 mL of the base has been added to 100.0 mL of 0.100 M acetic acid?arrow_forwardA buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer.arrow_forward
- Calculate the mass of sodium acetate, NaCH3COO, you should add to 500. mL of a 0.150-M solution of acetic acid, CH3COOH, to buffer a solution at a pH of 4.57.arrow_forwardA solution is prepared by dissolving 0.350 g of benzoic acid, HC7H5O2, in water to make 100.0 mL of solution. A 30.00-mL sample of the solution is titrated with 0.272 M KOH. Calculate the pH of the solution (a) before titration. (b) halfway to the equivalence point. (c) at the equivalence point.arrow_forwardA buffer solution is prepared by dissolving 1.50 g each of benzoic acid, C6H5CO2H, and sodium benzoate, NaC6H5CO2, in 150.0 mL of solution. (a) What is the pH of this buffer solution? (b) Which buffer component must be added, and in what quantity, to change the pH to 4.00? (c) What quantity of 2.0 M NaOH or 2.0 M HCl must be added to the buffer to change the pH to 4.00?arrow_forward
- Phenol, C6H5OH, is a weak organic acid. Suppose 0.515 g of the compound is dissolved in enough water to make 125 mL of solution. The resulting solution is titrated with 0.123 M NaOH. C6H5OH(aq) + OH(aq) C6H5O(aq) + H2O() (a) What is the pH of the original solution of phenol? (b) What are the concentrations of all of the following ions at the equivalence point: Na+, H3O+, OH, and C6H5O? (c) What is the pH of the solution at the equivalence point?arrow_forwardDoes the pH of the solution increase, decrease, or stay the same when you (a) Add solid sodium oxalate, Na2C2O4, to 50.0 mL of 0.015-M oxalic acid? (b) Add solid ammonium chloride to 100. mL of 0.016-M HCl? (c) Add 20.0 g NaCl to 1.0 L of 0.012-M sodium acetate, NaCH3COO?arrow_forwardWhat 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_forward
- A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?arrow_forwardYou are given the following acidbase titration data, where each point on the graph represents the pH after adding a given volume of titrant (the substance being added during the titration). a What substance is being titrated, a strong acid, strong base, weak acid, or weak base? b What is the pH at the equivalence point of the tiration? c What indicator might you use to perform this titration? Explain.arrow_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
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 & 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: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher: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 & 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: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
General, Organic, and Biological Chemistry
Chemistry
ISBN:9781285853918
Author:H. Stephen Stoker
Publisher:Cengage Learning
General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY