Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 16, Problem 97GQ
The base ethylamine
(a) Which of the two bases is stronger?
(b) Calculate the pH of a 0.10M solution of the strong base?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
At 25°C, the Ka of pentafluorobenzoic acid (C6F5COOH) is 0.033. Suppose 0.100 mol of pentafluorobenzoic acid is dissolved in 1.00 L of water. What is the pH of this solution?
Fill in the left side of this equilibrium constant equation for the reaction of diethylmethylamine (C3H13N), a weak base, with water.
D= K,
olo
Calculate the equilibrium constant for the acid–base reaction between the reactants in each of the following pairs: (a) HCl + H2O (b) CH3COOH + H2O (c) CH3NH2 + H2O (d) CH3N+H3 + H2O
Chapter 16 Solutions
Chemistry & Chemical Reactivity
Ch. 16.2 - What are the hydronium ion and hydroxide ion...Ch. 16.4 - For each of the following salts in water, predict...Ch. 16.5 - (a) Which is the stronger Bronsted acid, HCO3 or...Ch. 16.7 - A solution prepared from 0.055 mol of butanoic...Ch. 16.7 - What are the equilibrium concentrations of acetic...Ch. 16.7 - What are the equilibrium concentrations of HF, F...Ch. 16.7 - The weak base, CIO (hypochlorite ion), is used in...Ch. 16.7 - Calculate the pH after mixing 15 mL of 0.12 M...Ch. 16.8 - What is the pH of a 0.10 M solution of oxalic...Ch. 16.10 - Prob. 1.1ACP
Ch. 16.10 - Prob. 1.2ACPCh. 16.10 - The pKa, of the conjugate acid of atropine is...Ch. 16.10 - Convert the pK values to K values for the...Ch. 16.10 - Other solvents also undergo autoionization. (a)...Ch. 16.10 - Prob. 2.3ACPCh. 16.10 - Prob. 2.4ACPCh. 16.10 - To measure the relative strengths of bases...Ch. 16 - Write the formula and the give the name of the...Ch. 16 - Write the formula and give the name of the...Ch. 16 - What are the products of each of the following...Ch. 16 - What are the products of each of the following...Ch. 16 - Write balanced equations showing how the hydrogen...Ch. 16 - Write a balanced equation showing how the HPO42...Ch. 16 - In each of the following acid-base reactions,...Ch. 16 - In each of the following acid-base reactions,...Ch. 16 - An aqueous solution has a pH of 3.75. What is the...Ch. 16 - A saturated solution of milk of magnesia. Mg(OH)2,...Ch. 16 - What is the pH of a 0.0075 M solution of HCl? What...Ch. 16 - What is the pH of a 1.2 104 M solution of KOH?...Ch. 16 - What is the pH of a 0.0015 M solution of Ba(OH)2?Ch. 16 - The pH of a solution of Ba(OH)2 is 10.66 at 25 ....Ch. 16 - Write an equilibrium constant expression for the...Ch. 16 - Write an equilibrium constant expression for the...Ch. 16 - Several acids are listed here with their...Ch. 16 - Several acids are listed here with their...Ch. 16 - Which of the following ions or compounds has the...Ch. 16 - Which of the following compounds or ions has the...Ch. 16 - Which of the following compounds or ions has the...Ch. 16 - Which of the following compounds or ion has the...Ch. 16 - Dissolving K2CO3 in water gives a basic solution....Ch. 16 - Dissolving ammonium bromide in water gives an...Ch. 16 - If each of the salts listed here were dissolved in...Ch. 16 - Which of the following common food additives gives...Ch. 16 - Prob. 27PSCh. 16 - Prob. 28PSCh. 16 - Prob. 29PSCh. 16 - An organic acid has pKa = 8.95. What is its Ka...Ch. 16 - Prob. 31PSCh. 16 - Which is the stronger of the following two acids?...Ch. 16 - Chloroacetic acid (ClCH2CO2H) has Ka = 1.41 103....Ch. 16 - A weak base has Kb = 1.5 109. What is the value...Ch. 16 - The trimethylammonium ion, (CH3)3NH+, is the...Ch. 16 - The chromium(III) ion in water, [Cr(H2O)6]3+. Is a...Ch. 16 - Acetic acid and sodium hydrogen carbonate, NaHCO3,...Ch. 16 - Ammonium chloride and sodium dihydrogen phosphate,...Ch. 16 - For each of the following reactions, predict...Ch. 16 - For each of the following reactions, predict...Ch. 16 - Equal molar quantities of sodium hydroxide and...Ch. 16 - Equal molar quantities of hydrochloric acid and...Ch. 16 - Equal molar quantities of acetic acid and sodium...Ch. 16 - Equal molar quantities of ammonia and sodium...Ch. 16 - A 0.015 M solution of hydrogen cyanate, HOCN, has...Ch. 16 - A 0.10 M solution of chloroacetic acid, CICH2CO2H,...Ch. 16 - A 0.025 M solution of hydroxyl amine has a pH of...Ch. 16 - Methylamine, CH3NH2, is a weak base. CH3NH2(aq) +...Ch. 16 - A 2.5 103 M solution of an unknown acid has a pH...Ch. 16 - A 0.015M solution of a base has a pH of 10.09 a)...Ch. 16 - What are the equilibrium concentrations of...Ch. 16 - The ionizations constant of a very weak acid, HA...Ch. 16 - What are the equilibrium concentration of H3O+, CN...Ch. 16 - Phenol (C6H5OH) commonly called carbolic acid is a...Ch. 16 - What are the equilibrium concentrations of...Ch. 16 - A hypothetical weak base has Kb=5.0104.Calculate...Ch. 16 - The weak base methylamine, CH3NH2, has Kb=4.2104....Ch. 16 - Calculate the pH of a 0.12 M aqueous solution of...Ch. 16 - Calculate the pH of a 0.0010 M aqueous solution of...Ch. 16 - A solution of hydrofluoric acid, HF, has a pH of...Ch. 16 - Calculate the hydronium ion concentration and pH...Ch. 16 - Calculate the hydronium ion concentration and pH...Ch. 16 - Sodium cyanide is the salt of the weak acid HCN....Ch. 16 - The sodium salt of propionic acid, NaCH3CH2CO2 is...Ch. 16 - Calculate the hydronium ion concentration and pH...Ch. 16 - Calculate the hydronium ion concentration and the...Ch. 16 - For each of the following cases, decide whether...Ch. 16 - For each of the following cases, decide whether...Ch. 16 - Oxalic acid, H2C2O4, is a diprotic acid. Write a...Ch. 16 - Sodium carbonate is a diprotic base. Write a...Ch. 16 - Prove that Ka1 Kb2 = Kw for oxalic acid H2C2O4,...Ch. 16 - Prove that Ka3 Kb1 = Kw for phosphoric acid,...Ch. 16 - Sulphurous acid, H2SO3, is a weak acid capable of...Ch. 16 - Ascorbic acid (vitamin C, C6H8O6) is a diprotic...Ch. 16 - Hydrazine, N2H4, can interact with water in two...Ch. 16 - Ethylene diamine, H2NCH2CH2NH2, can interact with...Ch. 16 - Which should be stronger acid, HOCN or HCN?...Ch. 16 - Prob. 78PSCh. 16 - Explain why benzene sulfonic acid is a Brnsted...Ch. 16 - The structure of ethylene diamine is illustrated...Ch. 16 - Decide whether each of the following substances...Ch. 16 - Decide whether each of the following substances...Ch. 16 - Carbon monoxide forms complexes with low-valent...Ch. 16 - Trimethylamine, (CH3)3N, is a common reagent. It...Ch. 16 - About this time, you may be wishing you had an...Ch. 16 - Consider the following ions: NH4+, CO32, Br, S2,...Ch. 16 - A 2.50 g sample of a solid that could be Ba(OH)2...Ch. 16 - In a particular solution, acetic acid is 11%...Ch. 16 - Hydrogen, H2S, and sodium acetate, NaCH3CO2 are...Ch. 16 - For each of the following reactions predict...Ch. 16 - A monoprotic acid HX has Ka = 1.3 103. Calculate...Ch. 16 - Arrange the following 0.10M solutions in order of...Ch. 16 - m-Nitrophenol, a weak acid, can be used as a pH...Ch. 16 - The butylammonium ion, C4H9NH3+, has a Ka of 2.3 ...Ch. 16 - The local anaesthetic novocaine is the hydrogen...Ch. 16 - Pyridine is weak organic base and readily forms a...Ch. 16 - The base ethylamine (CH3CH2NH2) has a Kb of. A...Ch. 16 - Chloroacetic acid, ClCH2CO2H, is a moderately weak...Ch. 16 - Saccharin (HC7H4NO3S) is a weak acid with pKa =...Ch. 16 - Given the following solutions: (a) 0.1 M NH3 (b)...Ch. 16 - For each of the following salts, predict whether a...Ch. 16 - Nicotine, C10H14N2, has two basic nitrogen atoms...Ch. 16 - Prob. 103GQCh. 16 - The equilibrium constant for the reaction of...Ch. 16 - The equilibrium constant for the reaction of...Ch. 16 - Calculate the pH of the solution that results from...Ch. 16 - To what volume should 1.00 102 mL of any weak...Ch. 16 - The hydrogen phthalate ion, C8HsO4, is a weak acid...Ch. 16 - Prob. 109GQCh. 16 - Prob. 110GQCh. 16 - Prob. 111ILCh. 16 - Prob. 112ILCh. 16 - Prob. 113ILCh. 16 - A hydrogen atom in the organic base pyridine,...Ch. 16 - Nicotinic acid, C6H5NO2, is found in minute...Ch. 16 - Prob. 116ILCh. 16 - Sulfanilic acid, which is used in making dyes, is...Ch. 16 - Amino acids are an important group of compounds....Ch. 16 - How can water be both a Brnsied base and a Lewis...Ch. 16 - The nickel(II) ion exists as [Ni(H2O)4]2+ in...Ch. 16 - The halogens form three stable, weak acids, HOX....Ch. 16 - The acidity of the oxoacids was described in...Ch. 16 - Perchloric acid behaves as an acid, even when it...Ch. 16 - You purchase a bottle of water. On checking its...Ch. 16 - Prob. 125SCQCh. 16 - Prob. 126SCQCh. 16 - Prob. 127SCQCh. 16 - Prob. 128SCQCh. 16 - Consider a salt of a weak base and a weak acid...
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
- For the following acid-base reaction, (1) predict the products, showing both reactants and products complete Lewis structures and arrows showing electron flow; (2) label each structure with the lowing: Bronsted acid, Bronsted base, conjugate acid, conjugate base; (3) give a brief definition of a ronsted acid and Bronsted base; (4) predict the direction of the equilibrium and justify your answer. HC0OH + CH3 Nta PRん106Y pkb = 3.36arrow_forward3) Calculate the pH of a 27 mg/L solution of hydrocyanic acid (HCN). The pKa of hydrocyanic acid is 9.3.arrow_forwardThe acid dissociation constant K, of trimethylacetic acid (HC (CH3) CO2 is 9.33 × 10 *. Calculate the pH of a 6.1M solution of trimethylacetic acid. Round your answer to 1 decimal place. PHarrow_forward
- Ammonia, NH3, is amphoteric. (a) Give the formula for the conjugate acid of NH3. (b) Give the formula for the conjugate base of NH3.arrow_forwardLithium diisopropylamide (LDA) is used as a strong base in organic synthesis. LDA is itself prepared by an acid-base reaction between butyllithium and N,N-diisopropylamine, [(CH3)2CH]2NH. Write an equation for this reaction, and place the appropriate labels on each reagent and product from the following list: stronger acid, stronger base, weaker acid, weaker base.arrow_forward10. The K, of methanol is 5.01 * 1016. Which side of the following reaction is favored, reactants or products? Explain your reasoning. Methanol (CH3OH) + NaOH H20 Con Basearrow_forward
- Phenylamine is an aromatic amine that is used in the manufacture of dyes. When absorbed through the skin itcauses the Fe+2 in hemoglobin to become oxidized into Fe+3, resulting in the formation of methemoglobin whichcannot bind to or transport oxygen. Phenylamine is soluble in water and acts as a weak base.C6H5NH2 (aq) + H2O (ℓ) ⇋ C6H5NH3+ (aq) + OH- (aq)a. When you measure the concentrations of the ionized substances you find them to be:[C6H5NH2] = 0.234 mol/L [C6H5NH3+] = 2.8 x 10-5 mol/L [OH-]= 2.8 x 10-5 mol/LIf the Kb is 4.27 x 10-10, is the reaction at equilibrium? If not, which direction does it need to move (rightor left) to reach equilibrium? Explain. b. At equilibrium the concentrations of the ionized substances are:[C6H5NH2] = 0.0537 mol/L [C6H5NH3+] = 4.79 x 10-6 mol/L [OH-]= 4.79 x 10-6 mol/LIf this reaction is taking place in a 2.0L container, and 1.5 moles of phenylamine were added to thereaction, what will the new concentrations of the three ionic species be when…arrow_forwardWould CH3NH3C2H3O2 (salt) be neutral, basic, acidic or cannot be determined?arrow_forwardCalculate the pH of a 0.295 M solution of ethylenediamine (H₂NCH,CH,NH₂). The pKa values for the acidic form of ethylenediamine (HNCH,CH,NH) are 6.848 (pKa1) and 9.928 (pKa2). pH = Calculate the concentration of each form of ethylenediamine in this solution at equilibrium. [H2NCH2CH2NH₂] = [H2NCH,CH,NH] = [HNCH,CH,NH3] = M M Marrow_forward
- 6. Acids and bases are defined by their donation or acceptance of a proton according to the (a) Arrhenius model. (b) Bronsted-Lowry model. (c) Lewis model.arrow_forwardWhat is the conjugate acid of H2C6H7O5 -1aq2? What is its conjugate base?arrow_forwardCalculate the pH of a 0.172 M solution of ethylenediamine (H,NCH,CH,NH,). The pK, values for the acidic form of ethylenediamine (HNCH,CH,NH) are 6.848 (pKat) and 9.928 (pKaz). pH = Calculate the concentration of each form of ethylenediamine in this solution at equilibrium. [H₂NCH,CH,NH₂] [H2NCH2CH2NH] = [HNCH2CH2NH] = M M Marrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY