Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 16, Problem 21PS
Dissolving K2CO3 in water gives a basic solution. Rite a balanced equation showing how this can occur.
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Consider the following acidic equilibrium: H₂CO₃(aq) + H₂O(l) ⇌ HCO₃⁻(aq) + H₃O⁺(aq). If you add NaHCO₃ to this solution, which of the following will occur?
A) The reaction quotient will decrease.
B) The reaction will shift in the reverse direction.
C) The equilibrium constant will increase.
D) No changes to the equilibrium positions will take place.
Arrange the following compounds in an increasing order of basic strengths in their aqueous solutions : NH3, CH3NH2, (CH3)2NH, (CH3)3N
8a and 8b
Chapter 16 Solutions
Chemistry & Chemical Reactivity
Ch. 16.1 - 1. H3PO4 phosphoric acid, can donate two protons...Ch. 16.1 - 2. The cyanide ion, CN−, accepts a proton from...Ch. 16.1 - 3. In the following reaction, identify the acid on...Ch. 16.1 - Prob. 4RCCh. 16.2 - What are the hydronium ion and hydroxide ion...Ch. 16.2 - What is the pH of a 0.0012 M NaOH solution at 25C?...Ch. 16.2 - The pH of a diet soda is 432 at 25C. What is the...Ch. 16.2 - If the pH of a solution containing the strong base...Ch. 16.3 - Prob. 1RCCh. 16.3 - Which acid has the strongest conjugate base? (a)...
Ch. 16.3 - Prob. 3RCCh. 16.3 - Prob. 4RCCh. 16.3 - Prob. 5RCCh. 16.4 - For each of the following salts in water, predict...Ch. 16.4 - Prob. 1RCCh. 16.4 - Prob. 2RCCh. 16.5 - (a) Which is the stronger Bronsted acid, HCO3 or...Ch. 16.5 - Prob. 1RCCh. 16.5 - 2. In the following reaction, does the equilibrium...Ch. 16.6 - Equal amounts (moles) of HCl(aq) and NaCN(aq) are...Ch. 16.6 - 2. Equal amounts (moles) of acetic acid(aq) and...Ch. 16.6 - Prob. 3RCCh. 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. 16.7 - 1. What is [H3O+] in a 0.10 M solution of HCN at...Ch. 16.7 - 2. A 0.040 M solution of an acid, HA, has a pH of...Ch. 16.7 - What are the pH and ion concentrations in a...Ch. 16.7 - Prob. 4RCCh. 16.7 - Prob. 1QCh. 16.7 - Prob. 2QCh. 16.7 - The pKa, of the conjugate acid of atropine is...Ch. 16.8 - What is the pH of a 0.10 M solution of oxalic...Ch. 16.8 - Hydrazine (N2H4) is like CO32 in that it is a...Ch. 16.9 - Which of the following is the stronger acid? (a)...Ch. 16.9 - Prob. 2RCCh. 16.9 - Prob. 3RCCh. 16.10 - 1. Which of the following can act as a Lewis acid?...Ch. 16.10 - 2. The molecule whose structure is illustrated...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. 3QCh. 16.10 - Prob. 4QCh. 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 - 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. 25PSCh. 16 - Prob. 26PSCh. 16 - Prob. 27PSCh. 16 - An organic acid has pKa = 8.95. What is its Ka...Ch. 16 - Prob. 29PSCh. 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. 76PSCh. 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. 101GQCh. 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. 107GQCh. 16 - Prob. 108GQCh. 16 - Prob. 109ILCh. 16 - Prob. 110ILCh. 16 - Prob. 111ILCh. 16 - A hydrogen atom in the organic base pyridine,...Ch. 16 - Nicotinic acid, C6H5NO2, is found in minute...Ch. 16 - Prob. 114ILCh. 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. 123SCQCh. 16 - Prob. 124SCQCh. 16 - Prob. 125SCQCh. 16 - Consider a salt of a weak base and a weak acid...
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- Which of the following conditions indicate an acidic solution? pH = 3.04 (H+| > 1.0 X IO’7 A/ pOH = 4.51 |OH-J = 3.21 X 10"12 Marrow_forward. Calculate the pH corresponding to each of the pOH values listed, and indicate whether each solution is acidic, basic, or neutral. a. pOH = 4.32 b. pOH = 8.90 c. pOH = 1.81 d. pOH = 13.1arrow_forwardHydrogen, H2S, and sodium acetate, NaCH3CO2 are mixed in water. Using Table 16.2, write a balanced equation for the acid-base reaction that could in principle, occur. Does the equilibrium lie toward the products or the reactants?arrow_forward
- What are the major species in solution after NaHSO4 is dissolved in water? What happens to the pH of the solution as more NaHSO4 is added? Why? Would the results vary if baking soda (NaHCO3) were used instead?arrow_forwardAcids You make a solution by dissolving 0.0010 mol of HCl in enough water to make 1.0 L of solution. a Write the chemical equation for the reaction of HCl(aq) and water. b Without performing calculations, give a rough estimate of the pH of the HCl solution. Justify your answer. c Calculate the H3O+ concentration and the pH of the solution. d Is there any concentration of the base OH present in this solution of HCl(aq)? If so, where did it come from? e If you increase the OH concentration of the solution by adding NaOH, does the H3O+ concentration change? If you think it does, explain why this change occurs and whether the H3O+ concentration increases or decreases. f If you were to measure the pH of 10 drops of the original HCl solution, would you expect it to be different from the pH of the entire sample? Explain. g Explain how two different volumes of your original HCl solution can have the same pH yet contain different moles of H3O+. h If 1.0 L of pure water were added to the HCl solution, would this have any impact on the pH? Explain.arrow_forwardH3PO4 is another polyprotic acid with three acidic hydrogens. Write a complete balanced equation for the three-step neutralization reaction between H3PO4 and NaOH. Net reaction: 3NaOH + H3PO4 === Na3PO4 + 3H2O 1. H3PO4 + NaOH → NaH2PO4 + H2O 2. H3PO4 + 2 NaOH → Na2HPO4 + 2 H2O 3. H3PO4 + 3 NaOH → Na3PO4 + 3 H2O Sketch an approximate graph of pH vs. volume on the following page, explaining why you choose to draw it this way.arrow_forward
- What is the pH of a solution with [H3O+] of 1.9 x 108 M?arrow_forward30. In the reaction HCl(aq) + H₂O(l) ⇒Cl¯(aq)+ H3O+ (aq) does water act as a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither, or both? (A) Neither as an acid nor as a base; water is neutral (B) Both an acid and a base. (C) An acid (D) A base (E) Depends temperaturearrow_forwardIn the reaction HPO 2 (aq) + H20(1) PO,3-(aq) + H30* (aq) HPO (aq) is the H20(1) is the PO43 (aq) is th and H30*(aq) is the Bronsted Lowry acid Bronsted Lowry base reactant product conjugate acid conjugate basearrow_forward
- If HNO3 is added to water, how does [OH-] change? How does pH change? (b) Use the pH values in Figure 16.5 to estimate the pH of a solution with [OH-] = 0.014 M. Is the solution acidic or basic? (c) If pH = 6.6, first estimate and then calculate the molar concentrations of OH-(aq) and H+(aq) in the solution. Figure 16.5arrow_forwardWhat is the concentration of H3O+ in a solution that is 0.0600 M Hypochlorous acid (HClO)? What is the pH? To solve this problem: Write the acid dissociation equilibrium for HClO Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, ClO- and HClO at equilibrium, in terms of x. Decide if x can be neglected. You may neglect x if the initial concentration of the HClO is greater than 100 times the Ka. You will need the value of Ka. Look it up on the chart (p 4 of packet) Solve for x Find the pH The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic aicd “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it…arrow_forwardThese are the characteristics of a strong acid. • ionizes completely in aqueous solutions has equilibrium far to the right ⚫ has a weaker bond to acidic hydrogen ○ True Falsearrow_forward
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