- 14.1: Consider two beakers of pure water at different temperatures. How d...
- 14.2: Differentiate between the terms strength and concentration as they ...
- 14.3: Sketch two graphs: (a) percent dissociation for weak acid HA versus...
- 14.4: Consider a solution prepared by mixing a weak acid HA and HCl. What...
- 14.5: Explain why salts can be acidic, basic, or neutral, and show exampl...
- 14.6: Consider two separate aqueous solutions: one of a weak acid HA and ...
- 14.7: You are asked to calculate the H_ concentration in a solution of Na...
- 14.8: Consider a solution prepared by mixing a weak acid HA, HCl, and NaA...
- 14.9: Consider a solution formed by mixing 100.0 mL of 0.10 M HA 100.00 m...
- 14.10: A certain sodium compound is dissolved in water to liberate Na_ ion...
- 14.11: Acids and bases can be thought of as chemical opposites (acids are ...
- 14.12: Consider two solutions of the salts NaX(aq) and NaY(aq) at equal co...
- 14.13: What is meant by pH? True or false: A strong acid solution always h...
- 14.14: Why is the pH of water at equal to 7.00?
- 14.15: Can the pH of a solution be negative? Explain.
- 14.16: Why is H3O_ the strongest acid and the strongest base that can exis...
- 14.17: How many significant figures are there in the numbers: 10.78, 6.78,...
- 14.18: In terms of orbitals and electron arrangements, what must be presen...
- 14.19: Give three example solutions that fit each of the following descrip...
- 14.20: Derive an expression for the relationship between pKa and pKb for a...
- 14.21: Consider the following statements. Write out an example reaction an...
- 14.22: Which of the following statements is(are) true? Correct the false s...
- 14.23: Consider the following mathematical expressions. a. b. c. d. For ea...
- 14.24: Consider a 0.10 M H2CO3 solution and a 0.10 M H2SO4 solution. Witho...
- 14.25: Of the hydrogen halides, only HF is a weak acid. Give a possible ex...
- 14.26: Explain why the following are done, both of which are related to ac...
- 14.27: Write balanced equations that describe the following reactions. a. ...
- 14.28: Write the dissociation reaction and the corresponding Ka equilibriu...
- 14.29: For each of the following aqueous reactions, identify the acid, the...
- 14.30: For each of the following aqueous reactions, identify the acid, the...
- 14.31: Classify each of the following as a strong acid or a weak acid.
- 14.32: Consider the following illustrations: Which beaker best illustrates...
- 14.33: Use Table 14.2 to order the following from the strongest to the wea...
- 14.34: Use Table 14.2 to order the following from the strongest to the wea...
- 14.35: You may need Table 14.2 to answer the following questions. a. Which...
- 14.36: You may need Table 14.2 to answer the following questions. a. Which...
- 14.37: Calculate the of each of the following solutions at Identify each s...
- 14.38: Calculate the of each of the following solutions at Identify each s...
- 14.39: Values of Kw as a function of temperature are as follows: a. Is the...
- 14.40: At the value of a. Calculate the [H_] and in pure water at . b. Wha...
- 14.41: Calculate the pH and pOH of the solutions in Exercises 37 and 38.
- 14.42: Calculate [H_] and for each solution at Identify each solution as n...
- 14.43: Fill in the missing information in the following table.
- 14.44: Fill in the missing information in the following table.
- 14.45: The pH of a sample of gastric juice in a persons stomach is 2.1. Ca...
- 14.46: The pOH of a sample of baking soda dissolved in water is 5.74 at Ca...
- 14.47: What are the major species present in 0.250 M solutions of each of ...
- 14.48: Calculate the pH of each of the following solutions of a strong aci...
- 14.49: A solution is prepared by adding 50.0 mL of 0.050 M HCl to 150.0 mL...
- 14.50: A solution is prepared by mixing 90.0 mL of 5.00 M HCl and 30.0 mL ...
- 14.51: How would you prepare 1600 mL of a solution using concentrated (12 ...
- 14.52: What mass of is present in 250.0 mL of a nitric acid solution having a
- 14.53: What are the major species present in 0.250 M solutions of each of ...
- 14.54: What are the major species present in 0.250 M solutions of each of ...
- 14.55: A 0.0560-g sample of acetic acid is added to enough water to make 5...
- 14.56: For propanoic acid determine the concentration of all species prese...
- 14.57: Calculate the concentration of all species present and the pH of a ...
- 14.58: Calculate the pH of a 0.20 M solution of iodic acid
- 14.59: Monochloroacetic acid, HC2H2ClO2, is a skin irritant that is used i...
- 14.60: A typical aspirin tablet contains 325 mg of acetylsalicylic acid, C...
- 14.61: Calculate the pH of each of the following. a. a solution containing...
- 14.62: Calculate the pH of a solution that contains 1.0 M HF and 1.0 M HOC...
- 14.63: Calculate the percent dissociation of the acid in each of the follo...
- 14.64: Using the Ka values in Table 14.2, calculate the percent dissociati...
- 14.65: A 0.15 M solution of a weak acid is 3.0% dissociated. Calculate Ka.
- 14.66: An acid HX is 25% dissociated in water. If the equilibrium concentr...
- 14.67: The pH of a M solution of cyanic acid (HOCN) is 2.77 at . Calculate...
- 14.68: Trichloroacetic acid (CCl3CO2H) is a corrosive acid that is used to...
- 14.69: A solution of formic acid has a pH of 2.70. Calculate the initial c...
- 14.70: One mole of a weak acid HA was dissolved in 2.0 L of solution. Afte...
- 14.71: Write the reaction and the corresponding Kb equilibrium expression ...
- 14.72: Write the reaction and the corresponding Kb equilibrium expression ...
- 14.73: Use Table 14.3 to help order the following bases from strongest to ...
- 14.74: Use Table 14.3 to help order the following acids from strongest to ...
- 14.75: Use Table 14.3 to help answer the following questions. a. Which is ...
- 14.76: Use Table 14.3 to help answer the following questions. a. Which is ...
- 14.77: Calculate the pH of the following solutions. a. 0.10 M NaOH b. M Na...
- 14.78: Calculate , pOH, and pH for each of the following. a. 0.00040 M Ca(...
- 14.79: What are the major species present in 0.015 M solutions of each of ...
- 14.80: What are the major species present in the following mixtures of bas...
- 14.81: What mass of KOH is necessary to prepare 800.0 mL of a solution hav...
- 14.82: Calculate the concentration of an aqueous Sr(OH)2 that has
- 14.83: What are the major species present in a 0.150 M NH3 solution? Calcu...
- 14.84: For the reaction of hydrazine (N2H4) in water, Kb is Calculate the ...
- 14.85: Calculate , [H_], and the pH of 0.20 M solutions of each of the fol...
- 14.86: Calculate , [H_], and the pH of 0.20 M solutions of each of the fol...
- 14.87: Calculate the pH of a 0.20 M C2H5NH2 solution
- 14.88: Calculate the pH of a 0.050 M (C2H5)2NH solution
- 14.89: Calculate the percent ionization in each of the following solutions...
- 14.90: Calculate the percentage of pyridine (C5H5N) that forms pyridinium ...
- 14.91: Codeine (C18H21NO3) is a derivative of morphine that is used as an ...
- 14.92: Calculate the mass of HONH2 required to dissolve in enough water to...
- 14.93: Write out the stepwise Ka reactions for the diprotic acid H2SO3.
- 14.94: Write out the stepwise Ka reactions for citric acid (H3C6H5O7), a t...
- 14.95: Using the Ka values in Table 14.4 and only the first dissociation s...
- 14.96: Arsenic acid (H3AsO4) is a triprotic acid with _ 5 _ 10_3, _ 8 _ 10...
- 14.97: Calculate the pH of a 2.0 M H2SO4 solution.
- 14.98: Calculate the pH of a M solution of H2SO4.
- 14.99: Arrange the following 0.10 M solutions in order of most acidic to m...
- 14.100: Arrange the following 0.10 Msolutions in order from most acidic to ...
- 14.101: Given that the Ka value for acetic acid is and the Ka value for hyp...
- 14.102: The Kb values for ammonia and methylamine are and respectively. Whi...
- 14.103: Sodium azide (NaN3) is sometimes added to water to kill bacteria. C...
- 14.104: Calculate the concentrations of all species present in a 0.25 M sol...
- 14.105: Calculate the pH of each of the following solutions. a. 0.10 M CH3N...
- 14.106: Calculate the pH of each of the following solutions. a. 0.12 M KNO2...
- 14.107: An unknown salt is either NaCN, NaC2H3O2, NaF, NaCl, or NaOCl. When...
- 14.108: Consider a solution of an unknown salt having the general formula B...
- 14.109: Calculate the pH of a 0.050 M Al(NO3)3 solution. The Ka value for A...
- 14.110: Calculate the pH of a 0.10 M CoCl3 solution. The Ka value for Co(H2...
- 14.111: Are solutions of the following salts acidic, basic, or neutral? For...
- 14.112: Are solutions of the following salts acidic, basic, or neutral? For...
- 14.113: Place the species in each of the following groups in order of incre...
- 14.114: Place the species in each of the following groups in order of incre...
- 14.115: Place the species in each of the following groups in order of incre...
- 14.116: Using your results from Exercise 115, place the species in each of ...
- 14.117: Will the following oxides give acidic, basic, or neutral solutions ...
- 14.118: Will the following oxides give acidic, basic, or neutral solutions ...
- 14.119: Identify the Lewis acid and the Lewis base in each of the following...
- 14.120: Identify the Lewis acid and the Lewis base in each of the following...
- 14.121: Aluminum hydroxide is an amphoteric substance. It can act as either...
- 14.122: Zinc hydroxide is an amphoteric substance. Write equations that des...
- 14.123: Would you expect Fe3_ or Fe2_ to be the stronger Lewis acid? Explain.
- 14.124: Use the Lewis acidbase model to explain the following reaction.
- 14.125: A 10.0-mL sample of an HCl solution has a pH of 2.000. What volume ...
- 14.126: Which of the following represent conjugate acidbase pairs? For thos...
- 14.127: A solution is made by adding 50.0 mL of 0.200 M acetic acid to 50.0...
- 14.128: You have 100.0 g of saccharin, a sugar substitute, and you want to ...
- 14.129: A solution is tested for pH and conductivity as pictured below: The...
- 14.130: A 0.25-g sample of lime (CaO) is dissolved in enough water to make ...
- 14.131: At , a saturated solution of benzoic acid has a pH of 2.80. Calcula...
- 14.132: Calculate the pH and [S2_] in a 0.10 M solution. Assume
- 14.133: A typical vitamin C tablet (containing pure ascorbic acid, H2C6H6O6...
- 14.134: Calculate the pH of an aqueous solution containing M HCl, 1.0 _ 10_...
- 14.135: Acrylic acid is a precursor for many important plastics. Ka for acr...
- 14.136: A 0.20 M sodium chlorobenzoate (NaC7H4ClO2) solution has a pH of 8....
- 14.137: The equilibrium constant Ka for the reaction is 6.0 _ 10_3. a. Calc...
- 14.138: Rank the following 0.10 M solutions in order of increasing pH. a. H...
- 14.139: Is an aqueous solution of NaHSO4 acidic, basic, or neutral? What re...
- 14.140: Calculate in a 0.010 M solution of CO2 in water (H2CO3). If all the...
- 14.141: Hemoglobin (abbreviated Hb) is a protein that is responsible for th...
- 14.142: Calculate the value for the equilibrium constant for each of the fo...
- 14.143: Students are often surprised to learn that organic acids, such as a...
- 14.144: The pH of M hydrochloric acid is not 8.00. The correct pH can be ca...
- 14.145: Calculate the pH of a M solution of NaOH in water.
- 14.146: Calculate in a M solution of Ca(OH)2.
- 14.147: Consider 50.0 mL of a solution of weak acid which has a pH of 4.000...
- 14.148: Making use of the assumptions we ordinarily make in calculating the...
- 14.149: Calculate the pH of a 0.200 M solution of C5H5NHF. Hint: C5H5NHF is...
- 14.150: Determine the pH of a 0.50 M solution of NH4OCl. See Exercise 149.
- 14.151: Calculate in a solution obtained by adding 0.0100 mol of solid NaOH...
- 14.152: What mass of NaOH(s) must be added to 1.0 L of 0.050 M NH3 to ensur...
- 14.153: A certain acid, HA, has a vapor density of 5.11 g/L when in the gas...
- 14.154: Calculate the mass of sodium hydroxide that must be added to 1.00 L...
- 14.155: Consider the species . Each ion can act as a base in water. Determi...
- 14.156: Calculate the pH of a 0.10 M solution of sodium phosphate. See papH...
- 14.157: Will 0.10 M solutions of the following salts be acidic, basic, or n...
- 14.158: a. The principal equilibrium in a solution of NaHCO3 is Calculate t...
- 14.159: A 0.100-g sample of the weak acid HA (molar mass _ 100.0 g/mol) is ...
- 14.160: A sample containing 0.0500 mol of Fe2(SO4)3 is dissolved in enough ...
- 14.161: A 2.14-g sample of sodium hypoiodite is dissolved in water to make ...
- 14.162: Isocyanic acid (HNCO) can be prepared by heating sodium cyanate in ...
- 14.163: Papaverine hydrochloride (abbreviated molar mass _ 378.85 g/mol) is...
- 14.164: Captain Kirk, of the Starship Enterprise, has been told by his supe...
- 14.165: For the following, mix equal volumes of one solution from Group I w...
Solutions for Chapter 14: Acids and Bases
Full solutions for Chemistry | 7th Edition
ISBN: 9780618528448
Since 165 problems in chapter 14: Acids and Bases have been answered, more than 190444 students have viewed full step-by-step solutions from this chapter. Chemistry was written by and is associated to the ISBN: 9780618528448. This expansive textbook survival guide covers the following chapters and their solutions. Chapter 14: Acids and Bases includes 165 full step-by-step solutions. This textbook survival guide was created for the textbook: Chemistry, edition: 7.
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allylic
The positions that are adjacent to the vinylic positions of a carboncarbon double bond.
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atomic mass unit (amu).
A mass exactly equal to 1 12th the mass of one carbon-12 atom. (3.1)
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azo coupling
An electrophilic aromatic substitution reaction in which an aryldiazonium salt reacts with an activated aromatic ring.
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condensation reaction
A chemical reaction in which a small molecule (such as a molecule of water) is split out from between two reacting molecules. (Sections 12.6 and 22.8)
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coordination number
The number of adjacent atoms to which an atom is directly bonded. In a complex the coordination number of the metal ion is the number of donor atoms to which it is bonded. (Sections 12.37 and 24.2)
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Covalent bond
A chemical bond formed between two atoms by sharing one or more pairs of electrons.
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critical mass
The amount of fissionable material necessary to maintain a nuclear chain reaction. (Section 21.7)
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Deactivating group
Any substituent on a benzene ring that causes the rate of electrophilic aromatic substitution to be lower than that for benzene.
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decomposition reaction
A chemical reaction in which a single compound reacts to give two or more products. (Section 3.2)
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High-density lipoprotein (HDL)
Plasma particles, density 1.06–1.21 g/mL, consisting of approximately 33% proteins, 30% cholesterol, 29% phospholipids, and 8% triglycerides.
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Hybrid orbital
An orbital formed by the combination of two or more atomic orbitals.
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hyperconjugation
An effect that explains why alkyl groups stabilize a carbocation.
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molecular solids
Solids that are composed of molecules. (Sections 12.1 and 12.6)
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percent ionization
The percent of a substance that undergoes ionization on dissolution in water. The term applies to solutions of weak acids and bases. (Section 16.6)
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Primary structure of proteins
The sequence of amino acids in the polypeptide chain, read from the N-terminal amino acid to the C-terminal amino acid.
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prostaglandins
Lipids that contain 20 carbon atoms and are characterized by a five-membered ring with two side chains.
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solubility
The amount of a substance that dissolves in a given quantity of solvent at a given temperature to form a saturated solution. (Sections 4.2 and 13.2)
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solvent extraction
A process by which one or more compounds are removed from a mixture of organic compounds, based on a difference in solubility and/or acid-base properties.
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syn addition
An addition reaction in which two groups are added to the same face of a p bond.
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Tesla (T)
The SI unit for magnetic fi eld strength.