Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 16, Problem 127SCQ

(a)

Interpretation Introduction

Interpretation:

The relationship between the degree of ionization of weak base or weak acid and equilibrium constant and initial concentration of acid or base has to be determined.

Concept Introduction:

Degree of ionization of a weak acid or weak base can be determined by writing the equilibrium concentration of all species involved in the equilibrium.

From the relationship of the equilibrium constant, the degree of ionization and initial concentration, the value of the degree of ionization of ammonium ion can be determined.

(b)

Interpretation Introduction

Interpretation:

The degree of ionization for weak acid ammonium ion has to be calculated.

Concept Introduction:

Degree of ionization of a weak acid or weak base can be determined by writing the equilibrium concentration of all species involved in the equilibrium.

From the relationship of the equilibrium constant, the degree of ionization and initial concentration, the value of the degree of ionization of ammonium ion can be determined.

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Chapter 16 Solutions

Chemistry & Chemical Reactivity

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...
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  • Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ion
    Table 13-4 lists the stepwise Ka values for some polyprotic acids. What is the difference between a monoprotic acid, a diprotic acid, and a triprotic acid? Most polyprotic acids are weak acids; the major exception is H2SO4. To solve for the pH of a solution of H2SO4, you must generally solve a strong acid problem as well as a weak acid problem. Explain. Write out the reactions that refer to Ka1 and Ka2 for H2SO4. For H3PO4, Ka1 = 7.5 103, Ka2 = 6.2 108, and Ka3= 4.8 1013. Write out the reactions that refer to the Ka1, Ka2and Ka3equilibrium constants. What are the three acids in a solution of H3PO4? Which acid is strongest? What are the three conjugate bases in a solution of H3PO4? Which conjugate base is strongest? Summarize the strategy for calculating the pH of a polyprotic acid in water.
    For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
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