Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 14, Problem 39QAP
Metacresol purple is an indicator that changes from yellow to purple at pH 8.2.
(a) What is Ka for this indicator?
(b) What is its pH range?
(c) What is the color of a solution with pH 9.0 and a few drops of metacresol purple?
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Based on the results obtained in the table, What is the color of acid-base indicator B when the pH of the medium is equal to its pKa?
. (a) Which is the stronger base—the basic form of the indicator cresol red or the basic form of thymolphthalein?(b) A solution is prepared in which cresol red is red and thymolphthalein is colorless. Estimate the pH of this solution.
During the fermentation of wine, a buffer consisting of tartaric acid and potassium hydrogen
tartrate is produced by a biochemical reaction. Assuming that the concentration of tartaric acid is
0.3158 M and potassium hydrogen tartrate is 0.3851 M, what is the pH of the wine? The Ka of
tartaric acid is 1.1x10-3.
Chapter 14 Solutions
Chemistry: Principles and Reactions
Ch. 14 - Write a net ionic equation for the reaction...Ch. 14 - Write a net ionic equation for the reaction...Ch. 14 - Write a balanced net ionic equation for the...Ch. 14 - Write a balanced net ionic equation for the...Ch. 14 - Calculate K for the reactions in Question 1.Ch. 14 - Calculate K for the reactions in Question 2.Ch. 14 - Prob. 7QAPCh. 14 - Calculate K for the reactions in Question 4.Ch. 14 - Calculate [H+] and pH in a solution in which...Ch. 14 - Calculate [OH-] and pH in a solution in which the...
Ch. 14 - A buffer is prepared by dissolving 0.0250 mol of...Ch. 14 - A buffer is prepared by dissolving 0.062 mol of...Ch. 14 - A buffer solution is prepared by adding 15.00 g of...Ch. 14 - A buffer solution is prepared by adding 5.50 g of...Ch. 14 - A solution with a pH of 9.22 is prepared by adding...Ch. 14 - An aqueous solution of 0.057 M weak acid, HX, has...Ch. 14 - Which of the following would form a buffer if...Ch. 14 - Which of the following would form a buffer if...Ch. 14 - Calculate the pH of a solution prepared by mixing...Ch. 14 - Calculate the pH of a solution prepared by mixing...Ch. 14 - Calculate the pH of a solution prepared by mixing...Ch. 14 - Calculate the pH of a solution prepared by mixing...Ch. 14 - Consider the weak acids in Table 13.2. Which...Ch. 14 - Prob. 24QAPCh. 14 - A sodium hydrogen carbonate-sodium carbonate...Ch. 14 - You want to make a buffer with a pH of 10.00 from...Ch. 14 - Prob. 27QAPCh. 14 - The buffer capacity indicates how much OH- or H+...Ch. 14 - A buffer is made up of 0.300 L each of 0.500 M...Ch. 14 - A buffer is made up of 239 mL of 0.187 M potassium...Ch. 14 - Enough water is added to the buffer in Question 29...Ch. 14 - Enough water is added to the buffer in Question 30...Ch. 14 - A buffer is prepared in which the ratio [ H2PO4...Ch. 14 - A buffer is prepared using the butyric...Ch. 14 - Blood is buffered mainly by the HCO3 H2CO3 buffer...Ch. 14 - There is a buffer system in blood H2PO4 HPO42 that...Ch. 14 - Given three acid-base indicators—methyl orange...Ch. 14 - Given the acid-base indicators in Question 37,...Ch. 14 - Metacresol purple is an indicator that changes...Ch. 14 - Thymolphthalein is an indicator that changes from...Ch. 14 - When 25.00 mL of HNO3 are titrated with Sr(OH)2,...Ch. 14 - A solution of KOH has a pH of 13.29. It requires...Ch. 14 - A solution consisting of 25.00 g NH4Cl in 178 mL...Ch. 14 - A 50.0-mL sample of NaHSO3 is titrated with 22.94...Ch. 14 - A sample of 0.220 M triethylamine, (CH3CH2)3 N, is...Ch. 14 - A 35.00-mL sample of 0.487 M KBrO is titrated with...Ch. 14 - A 0.4000 M solution of nitric acid is used to...Ch. 14 - A 0.2481 M solution of KOH is used to titrate...Ch. 14 - Consider the titration of butyric acid (HBut) with...Ch. 14 - Morphine, C17H19O3N, is a weak base (K b =7.4107)....Ch. 14 - Consider a 10.0% (by mass) solution of...Ch. 14 - A solution is prepared by dissolving 0.350 g of...Ch. 14 - Prob. 53QAPCh. 14 - Ammonia gas is bubbled into 275 mL of water to...Ch. 14 - For an aqueous solution of acetic acid to be...Ch. 14 - Prob. 56QAPCh. 14 - Prob. 57QAPCh. 14 - Water is accidentally added to 350.00 mL of a...Ch. 14 - A solution of an unknown weak base...Ch. 14 - Consider an aqueous solution of HF. The molar heat...Ch. 14 - Each symbol in the box below represents a mole of...Ch. 14 - Use the same symbols as in Question 61 ( = anion,...Ch. 14 - The following is the titration curve for the...Ch. 14 - Prob. 64QAPCh. 14 - Follow the directions of Question 64. Consider two...Ch. 14 - Prob. 66QAPCh. 14 - Indicate whether each of the following statements...Ch. 14 - Prob. 68QAPCh. 14 - Consider the following titration curves. The...Ch. 14 - Consider the titration of HF (K a=6.7104) with...Ch. 14 - The species called glacial acetic acid is 98%...Ch. 14 - Four grams of a monoprotic weak acid are dissolved...Ch. 14 - Prob. 73QAPCh. 14 - Fifty cm3 of 1.000 M nitrous acid is titrated with...Ch. 14 - A diprotic acid, H2B(MM=126g/moL), is determined...Ch. 14 - Prob. 76QAPCh. 14 - Two students were asked to determine the Kb of an...Ch. 14 - How many grams of NaOH must be added to 1.00 L of...Ch. 14 - How many grams of NaF must be added to 70.00 mL of...Ch. 14 - Prob. 80QAP
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 have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.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_forwardConsider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?arrow_forward
- A solution of carbonate (pKa = 6.3, 10.3) contains 0.0100 mol HCO3- and 0.00500 mol CO32-. Calculate the pH at equilibrium.arrow_forwardConsider a buffer solution containing an acid with a pKa of 2.3 and an acid concentration that is one fourth the concentration of the conjugate base. What is the pH of the solution?arrow_forwardThe phenolphthalein pH indicator is clear and colorless in an acidic solution, but it turns a pink in a basic solution. Knowing this, you examine two clear and colorless solutions. One, you are told is acidic and the other is basic. Furthermore, you are told that the acidic solution contains phenolphthalein. So which is which? You don’t know because both solutions are colorless. To find out, you add a drop of Solution 1 to Solution 2. A pink color appears for a moment, but then disappears. This tells you that Select one: a. you now need to try adding Solution 2 to Solution 1. b. Solution 2 is acidic. c. Solution 1 is acidic. d. both solutions are now neutralized.arrow_forward
- You are told that a heavily polluted sewer contains high concentrations of H2S (pKa₁ = 7.2) and ammonia (pKa = 9.3). Upon inspect of the manhole at the sewage treatment plant you can smell ammonia (NH3) but cannot detect any H2S odor. What can you say about the likely pH range of the sewage?arrow_forwardHow many moles of sodium hydroxide would have to be added to 225 mL of a 0.404 M nitrous acid solution, in order to prepare a buffer with a pH of 3.550?arrow_forwardIf 10 mL of 0.1 M hypothetical acid, HA, is added with 10 mL of 0.1 M of the salt of its conjugate base, XA, what is the pH of the solution?arrow_forward
- What is the color of methyl red indicator in a solution of pH 5?arrow_forwardThe weak base colloquially known as Tris, and more precisely as tris(hydroxymethyl)-am inomethane, has pKa = 8.3 at 20 °C and is commonly used to produce a buffer for biochemical applications. At what pH would you expect Tris to act as a buffer in a solution that has equal molar concentrations of Tris and its conjugate acid?arrow_forwardCarbonate and bicarbonate can be combined to form a buffer system. How many grams of magnesium carbonate would have to be dissolved in 750.0 mL of a 0.1330 M bicarbonate solution to prepare a solution with a pH of 9.33? (Ka of bicarbonate is 4.7 X 10 -11)arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
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