- 18.1: Write balanced equations for the reactions between the following. a...
- 18.2: Challenge Write the net ionic equation for the reaction in Question...
- 18.3: Identify the conjugate acid-base pairs in each reaction. a. N H 4 +...
- 18.4: Challenge The products of an acid-base reaction are H 3O + and S O ...
- 18.5: Explain why many Lewis acids and bases are not classified as Arrhen...
- 18.6: Compare the physical and chemical properties of acids and bases
- 18.7: Explain how the concentrations of hydrogen ions and hydroxide ions ...
- 18.8: Explain why many compounds that contain one or more hydrogen atoms ...
- 18.9: Identify the conjugate acid-base pairs in the following equation. H...
- 18.10: Write the Lewis structure for phosphorus trichloride (PC l 3 ). Is ...
- 18.11: Interpret Scientific Illustrations In the accompanying structural f...
- 18.12: Write ionization equations and acid ionization constant expressions...
- 18.13: Write the first and second ionization equations for H 2Se O
- 18.14: Challenge Given the expression K a = [As O 4 3-][ H 3O + __] [HCN] ...
- 18.15: Write ionization equations and base ionization constant expressions...
- 18.16: Challenge Write an equation for a base equilibrium in which the bas...
- 18.17: Describe the contents of dilute aqueous solutions of the strong aci...
- 18.18: Relate the strength of a weak acid to the strength of its conjugate...
- 18.19: Identify the conjugate acid-base pairs in each equation. a. HCOOH(a...
- 18.20: Explain what the K b for aniline ( C 6 H 5 N H 2 ) tells you ( K b ...
- 18.21: Interpret Data Use the data in Table 18.4 to put the seven acids in...
- 18.22: The concentration of either the H + ion or the O H - ion is given f...
- 18.23: Challenge Calculate the number of H + ions and the number of O H - ...
- 18.24: Calculate the pH of solutions having the following ion concentratio...
- 18.25: Calculate the pH of aqueous solutions with the following [ H +] at ...
- 18.26: Challenge Calculate the pH of a solution having [O H -] = 8.2 1 0 -6M.
- 18.27: Calculate the pH and pOH of aqueous solutions with the following co...
- 18.28: Calculate the pH and pOH of aqueous solutions with the following co...
- 18.29: Challenge Calculate pH and pOH for an aqueous solution containing 1...
- 18.30: Calculate [ H +] and [O H -] in each of the following solutions. a....
- 18.31: Challenge Calculate the [ H +] and [O H -] in a sample of seawater ...
- 18.32: Calculate the K a for the following acids using the given informati...
- 18.33: Calculate the K a of the following acids using the given informatio...
- 18.34: Challenge Calculate the K a of a 0.0091M solution of an unknown aci...
- 18.35: Explain why the pH of an acidic solution is always a smaller number...
- 18.36: Describe how you can determine the pH of a solution if you know its...
- 18.37: Explain the significance of K w in aqueous solutions
- 18.38: Explain, using Le Chteliers principle, what happens to the [ H +] o...
- 18.39: List the information needed to calculate the K a of a weak acid
- 18.40: Calculate The pH of a tomato is approximately 4.50. What are [ H +]...
- 18.41: Determine the pH of a solution that contains 1.0 1 0 -9 mol of O H ...
- 18.42: Calculate the pH of the following solutions. a. 1.0M HI c. 1.0M KOH...
- 18.43: Interpret Diagrams Refer to Figure 18.15 to answer these questions:...
- 18.44: What is the molarity of a nitric acid solution if 43.33 mL of 0.100...
- 18.45: What is the concentration of a household ammonia cleaning solution ...
- 18.46: Challenge How many milliliters of 0.500M NaOH would neutralize 25.0...
- 18.47: Write equations for the salt hydrolysis reactions occuring when the...
- 18.48: Challenge Write the equation for the reaction that occurs in a titr...
- 18.49: Explain why the net ionic equation for the neutralization reaction ...
- 18.50: Explain the difference between the equivalence point and the end po...
- 18.51: Compare the results of two experiments: First, a small amount of ba...
- 18.52: Calculate the molarity of a solution of hydrobromic acid (HBr) if 3...
- 18.53: Interpret What substances could be used to make a buffer solution w...
- 18.54: Design an Experiment Describe how you would design and perform a ti...
- 18.55: In terms of ion concentrations, distinguish between acidic, neutral...
- 18.56: Write a balanced chemical equation that represents the self-ionizat...
- 18.57: Classify each compound as an Arrhenius acid or an Arrhenius base. a...
- 18.58: Geology When a geologist adds a few drops of HCl to a rock, gas bub...
- 18.59: Explain the meaning of the relative sizes of the two shaded areas t...
- 18.60: Explain the difference between a monoprotic acid, a diprotic acid, ...
- 18.61: Why can H + and H 3 O + be used interchangeably in chemical equations?
- 18.62: Use the symbols <, >, and = to express the relationship between the...
- 18.63: Explain how the definition of a Lewis acid differs from the definit...
- 18.64: Write a balanced chemical equation for each of the following. a. th...
- 18.65: Explain the difference between a strong acid and a weak acid.
- 18.66: Explain why equilibrium arrows are used in the ionization equations...
- 18.67: Which of the beakers shown in Figure 18.29 might contain a solution...
- 18.68: How would you compare the strengths of two weak acids experimentall...
- 18.69: . Identify the conjugate acid-base pairs in the reaction of H 3 P O...
- 18.70: Ammonia Cleaner Write the chemical equation and K b expression for ...
- 18.71: Disinfectant Hypochlorous acid is an industrial disinfectant. Write...
- 18.72: Write the chemical equation and the K b expression for the ionizati...
- 18.73: A fictional weak base, Za H 2 , reacts with water to yield a soluti...
- 18.74: Select a strong acid, and explain how you would prepare a dilute so...
- 18.75: What is the relationship between the pOH and the O H - ion concentr...
- 18.76: Solution A has a pH of 2.0. Solution B has a pH of 5.0. Which solut...
- 18.77: If the concentration of H + ions in an aqueous solution decreases, ...
- 18.78: Use Le Chteliers principle to explain what happens to the equilibri...
- 18.79: Common Acids and Bases Use the data in Table 18.8 to answer the fol...
- 18.80: What is [O H -] in an aqueous solution at 298 K in which [ H +] = 5...
- 18.81: What are the pH and pOH for the solution described in Question 80?
- 18.82: If 5.00 mL of 6.00M HCl is added to 95.00 mL of pure water, the fin...
- 18.83: Given two solutions, 0.10M HCl and 0.10M HF, which solution has the...
- 18.84: Metal Cleaner Chromic acid is used as an industrial cleaner for met...
- 18.85: What acid and base must react to produce an aqueous sodium iodide s...
- 18.86: What acid-base indicators, shown in Figure 18.24, would be suitable...
- 18.87: When might a pH meter be better than an indicator to determine the ...
- 18.88: What happens when an acid is added to a solution containing the HF/...
- 18.89: When methyl red is added to an aqueous solution, a pink color resul...
- 18.90: Give the name and formula of the acid and the base from which each ...
- 18.91: Write formula equations and net ionic equations for the hydrolysis ...
- 18.92: Air Purifier Lithium hydroxide is used to purify air by removing ca...
- 18.93: In an acid-base titration, 45.78 mL of a sulfuric acid solution is ...
- 18.94: Write the equation for the ionization reaction and the base ionizat...
- 18.95: How many milliliters of 0.225M HCl would be required to titrate 6.0...
- 18.96: What is the pH of a 0.200M solution of hypobromous acid (HBrO)? K a...
- 18.97: Which of the following are polyprotic acids? Write successive ioniz...
- 18.98: Write balanced chemical equations for the two successive ionization...
- 18.99: Sugar Refining Strontium hydroxide is used in the refining of beet ...
- 18.100: What are the concentrations of O H - ions in solutions having pH va...
- 18.101: The pH probe in Figure 18.31 is immersed in a 0.200M solution of a ...
- 18.102: Write the chemical equation for the reaction that would occur when ...
- 18.103: An aqueous solution buffered by benzoic acid ( C 6 H 5 COOH) and so...
- 18.104: Critique the following statement: A substance whose chemical formul...
- 18.105: Analyze and Conclude Is it possible that an a Arrhenius acid is not...
- 18.106: Apply Concepts Use the ion product constant of water at 298 K to ex...
- 18.107: . Identify the Lewis acids and bases in the following reactions. a....
- 18.108: Interpret Scientific Illustrations Sketch the shape of the approxim...
- 18.109: Recognize Cause and Effect Illustrate how a buffer works using the ...
- 18.110: Predict Salicylic acid, shown in Figure 18.32, is used to manufactu...
- 18.111: Apply Concepts Like all equilibrium constants, the value of K w var...
- 18.112: You have 20.0 mL of a solution of a weak acid, HX, whose K a equals...
- 18.113: What factors determine whether a molecule is polar or nonpolar? (Ch...
- 18.114: What property of some liquids accounts for the meniscus that forms ...
- 18.115: Which of the following physical processes are exothermic for waterf...
- 18.116: Explain why an air pump gets hot when you pump air into a bicycle t...
- 18.117: When 5.00 g of a compound was burned in a calorimeter, the temperat...
- 18.118: What is the difference between an exothermic and an endothermic rea...
- 18.119: Figure 18.33 shows how energy changes during the progress of a reac...
- 18.120: Hydrogen and fluorine react to form HF according to the following e...
- 18.121: Acid/Base Theories Imagine that you are the Danish chemist Johannes...
- 18.122: Amino Acids Twenty amino acids combine to form proteins in living s...
- 18.123: In general, what is the trend in the average pH for the years 1990 ...
- 18.124: Calculate the [ H +] for the lowest and the highest pH measurements...
- 18.125: What is the pH of the trend line in 2003? How much has the average ...
Solutions for Chapter 18: Acids and Bases
Full solutions for Chemistry: Matter & Change | 1st Edition
ISBN: 9780078746376
Chemistry: Matter & Change was written by and is associated to the ISBN: 9780078746376. This textbook survival guide was created for the textbook: Chemistry: Matter & Change, edition: 1. Chapter 18: Acids and Bases includes 125 full step-by-step solutions. This expansive textbook survival guide covers the following chapters and their solutions. Since 125 problems in chapter 18: Acids and Bases have been answered, more than 256640 students have viewed full step-by-step solutions from this chapter.
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Allylic carbon
A carbon adjacent to a carbon-carbon double bond.
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Antiaromatic compound
A monocyclic compound that is planar or nearly so, has one 2p orbital on each atom of the ring, and has 4n p electrons in the cyclic arrangement of overlapping 2p orbitals, where n is an integer. Antiaromatic compounds are especially unstable
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atomic orbital
A three-dimensional plot of y2 of a wavefunction. It is a region of space that can accommodate electron density.
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bond length.
The distance between the nuclei of two bonded atoms in a molecule. (9.4)
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chemical reactions
Processes in which one or more substances are converted into other substances; also called chemical changes. (Section 1.3)
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copolymer
A complex polymer resulting from the polymerization of two or more chemically different monomers. (Section 12.8)
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debye (D)
A unit of measure fordipole moments, where 1 debye = 10-18 esu×cm.
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Frequency
The number of full cycles of a wave that pass a given point in a second, and reported in hertz (Hz), which has the units s21
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halogenation
A reaction that involves the addition of X2 (either Br2 or Cl2) across an alkene.
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heat of combustion
The heat given off during a reaction in which an alkane reacts with oxygen to produce CO2 and water.
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hemiacetal
A compound containing a hydroxyl group (OH) and an alkoxy group (OR) connected to the same carbon atom.
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hydroboration-oxidation
A twostep process that achieves an anti-Markovnikov addition of a proton and a hydroxyl group (OH) across an alkene.
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Hydroboration-oxidation
A method for converting an alkene to an alcohol. The alkene is treated with borane (BH3) to give a trialkylborane, which is then oxidized with alkaline hydrogen peroxide to give an alcohol
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hypothesis
A tentative explanation of a series of observations or of a natural law. (Section 1.3)
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imine
A compound containing a CRN bond.
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Isomers
Different compounds with the same molecular formula.
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lock-and-key model
A model of enzyme action in which the substrate molecule is pictured as fitting rather specifically into the active site on the enzyme. It is assumed that in being bound to the active site, the substrate is somehow activated for reaction. (Section 14.7)
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molecular orbital (MO)
An allowed state for an electron in a molecule. According to molecular-orbital theory, a molecular orbital is entirely analogous to an atomic orbital, which is an allowed state for an electron in an atom. Most bonding molecular orbitals can be classified as s or p, depending on the disposition of electron density with respect to the internuclear axis. (Section 9.7)
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molecular-orbital diagram
A diagram that shows the energies of molecular orbitals relative to the atomic orbitals from which they are derived; also called an energy-level diagram. (Section 9.7)
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primary
A term used to indicate that exactly one alkyl group is attached directly to a particular position. For example, a primary carbocation has one alkyl group (not more) attached directly to the electrophilic carbon atom (C+).