![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
Question
Chapter 16, Problem 16.15QP
Interpretation Introduction
Interpretation:
The pH changes that occur during the titration of a weak base by a strong acid has to be described.
The term equivalence point has to be explained.
Concept Information:
The titration curve of weak base by a strong acid will be similar to the curve of weak acid by a strong base.
Methyl orange can be used as indicator for this titration.
The equivalence point is the point obtained in a titration once a stoichiometric amount of reactant has been added.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Equimolar quantities of potassium fluoride and hydrofluoric acid are placed into solution.
What happens to the buffer system if some hydrochloric acid is added to the solution?
The hydrochloric acid reacts with the fluoride ions so the pH decreases only slightly.
The hydrochloric acid reacts with the fluoride ions so the pH decreases significantly.
) The hydrochloric acid reacts with the hydrofluoric acid so the pH increases only slightly.
The hydrochloric acid reacts with the hydrofluoric acid so the pH increases significantly.
Back aboard the ship, in the botany lab, Mr. Sulu is performing a titration on a weak acid he has
extracted from a native plant from the planet's surface. If he titrates this weak acid with sodium
hydroxide, what value of pH does he expect before the titration begins, half-way to the equivalence
point, at the equivalence point and after the equivalence point of his titration? Why would he get
each of these pH values? (explain by indicating what species are in the beaker)
A series of carbonic acid or carbonate buffers regulate pH in blood within the human body. The kidneys and the lungs work together to help maintain a blood pH of 7.4 by affecting the components of the buffers in the blood.
What conjugate acid/base pair is the main component in the buffer? Write out the chemical reaction that the conjugate pair undergoes in water.
What is the ratio of the acid to the base?
What is the ideal pH range for this buffer?
Is the pH of blood within the ideal range of the buffer? If it is not, what is the physiological reason that the body would have for still using a carbonate buffer as opposed to another conjugate pair?
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
- You 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_forwardDescribe the meanings of acidosis and alkalosis. How do buffers function in this system?arrow_forwardSelect the statements that describe a method which can be used to make a buffer. Add appropriate quantities of weak acid and its conjugate base to water. Partially neutralize a strong base solution by addition of a strong acid. Partially neutralize a strong acid solution by addition of a strong base. Partially neutralize a weak base solution by addition of a strong acid. Partially neutralize a weak acid solution by addition of a strong base.arrow_forward
- For biological buffer systems, buffer acids capacity is usually greater than buffer bases capacity. Why?arrow_forwardConsider the buffer system of carbonic acid (H₂CO₂) and its salt, KHCO₂, which provides the conjugate base, HCO,. H_COjlog) + HJO W 7 HyO" loạ) + HCOy loa) How does the buffer react when some base is added? The bicarbonate ion (HCO) of the buffer reacts with the base. OHCO and H₂CO, both react with the base. O The buffer does not react. O The carbonic acid (H₂CO₂) of the buffer reacts with the base Question 15 Indicate whether each of the following reactions is an example of reaction of an acid with a metal, reaction of an acid with a carbonate, or acid-base neutralization reaction using the dropdown on the right. Reaction A: ZnCO3(s) + 2HBr(aq) → ZnBr₂(aq) + CO₂(g) + H₂O(l) Reaction B: Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g) HCI(g) + NaHCO3(s)→ NaCl(aq) + CO₂(g) + H₂O(0) H₂SO4(aq) + Mg(OH)2(s)→ MgSO4(aq) + 2H₂O(1) 3LIOH(aq) + H₂PO₂(aq) → Li₂PO₂(aq) + 3H₂O(0) Cal(s) + H₂SO4(aq) → H₂(g) + CaSO₂(aq) Reaction C: Reaction D: Reaction E: Reaction Earrow_forwardExplain why the solubility of a sparingly soluble salt represents an equilibrium system.arrow_forward
- The indicator thymol blue changes from red to yellow between pH 1.2 and pH 2.8. If thymol blue is added to a solution, and the solution turns yellow, then the pH of the solution must be above 2.8, and the solution is basic. the pH of the solution must be above 2.8, and the solution is acidic. the solution is basic, and the pH must be at or below 1.2. the pH of the solution is above 2.8, and the solution could be acidic, neutral or basic. the solution is acidic, and the pH must be at or below 1.2.arrow_forwardThe indicator thymol blue changes from red to yellow between pH 1.2 and pH 2.8. If thymol blue is added to a solution, and the solution turns yellow, then the pH of the solution must be above 2.8, and the solution is acidic. the solution is acidic, and the pH must be at or below 1.2. the solution is basic, and the pH must be at or below 1.2. the pH of the solution must be above 2.8, and the solution is basic. the pH of the solution is above 2.8, and the solution could be acidic, neutral or basic.arrow_forwardDescribe the role of buffers in maintaining the pH of a solution.arrow_forward
- TRUE OR FALSE During neutralization reaction, the concentration of the buffer system remains the samearrow_forwardBuffers usually are composed of: Weak acids and conjugate bases Weak acids and weak bases Weak acids and conjugate acids 98. Which of the following leads to an overall decrease in energy of a system? Freezing Sublimation Melting Vaporizationarrow_forwardLet's say that you're titrating an acid with a sodium hydroxide solution, and you think you're at the equivalence point (when acid moles = base moles). You (or your partner, I guess) accidentally add an extra drop of base, and the solution immediately turns dark pink. Oh no! Why does the color's intensity change so drastically? a) Sodium Hydroxide is a strong base, so adding any extra amount will dramatically decrease the pH, thus forcing the indicator to turn dark pink. b) Sodium Hydroxide is a strong acid, so adding any extra amount will dramatically decrease the pH, thus forcing the indicator to turn dark pink. c) Sodium Hydroxide is a strong base, so adding any extra amount will dramatically increase the pH, thus forcing the indicator to turn dark pink. d) Sodium Hydroxide is a strong acid, so adding any extra amount will dramatically increase the pH, thus forcing the indicator to turn dark pink.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
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
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
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
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