15.15.11) Calculate the pH of a 0.20 M ammonium acetate (CH3COONH4) solution.
15.15.65) What are the concentrations of HSO4 2, SO4 22, and H1 in a 0.20 M KHSO4 solution?
15.15.66) Calculate the concentrations of H1, HCO3 2, and CO3 22 in a 0.025 M H2CO3 solution.
15.15.67) List four factors that affect the strength of an acid.
15.1E) What causes heartburn? What are some possible ways to alleviate heartburn?
15.1SAQ) ?Identify the conjugate base in the reaction shown here: a) HClO2 b) H2O c) H3O+ d) ClO2-
15.2E) What are the general physical and chemical properties of acids? Of bases?
15.15.16) Calculate the concentration of H1 ions in a 0.62 M NaOH solution
15.2SAQ) ?Which pair is a Brønsted–Lowry conjugate acid–base pair?
15.3E) What is a carboxylic add? Give an example.
15.4E) What is the Arrhenius definition of an acid? Of a base?
15.15.69) Predict the acid strengths of the following compounds: H2O, H2S, and H2Se.
15.5E) ?What is a hydronium ion? Does H+ exist in solution by itself?
15.15.17) Calculate the pH of each of the following solutions: (a) 0.0010 M HCl, (b) 0.76 M KOH.
15.6E) What is the Bronsted-Lowry definition of an acid? Of a base?
15.8E) Describe amphoteric behavior and give an example.
15.9E) What is a conjugate acid-base pair? Provide an example.
15.15.121) Calculate the pH of a 2.00 M NH4CN solution
15.10E) Explain the difference between a strong acid and a weak acid and list one example of each.
15.11E) ?What are diprotic and triprotic acids? List an example of each.
15.15.71) Which of the following is the stronger acid: CH2ClCOOH or CHCl2COOH? Explain your choice.
15.15.122) Calculate the concentrations of all species in a 0.100 M H3PO4 solution.
15.12E) Define the acid ionization constant and explain its significance.
15.14E) ?What happens to the [OH-] of a solution when the [H3O+] is increased? Decreased?
15.15E) Define pH. What pH range is considered acidic? Basic? Neutral?
15.15.21) Complete the following table for a solution: pH [H1] Solution is ,7 ,1.0 3 1027 M Neutral
15.16E) Define pOH. What pOH range is considered acidic? Basic? Neutral?
15.21E) ?Write a generic equation showing how a weak base ionizes Water.
15.15.74) Explain why small, highly charged metal ions are able to undergo hydrolysis
15.24E) What kinds of cations act as weak acids? List some examples.
15.15.126) Calculate the concentrations of all the species in a 0.100 M Na2CO3 solution.
15.15.75) Al31 is not a Brnsted acid but Al(H2O)31 6 is. Explain
15.28E) ?Which factors affect the relative acidity of an oxyacid?
15.29E) What is the Lewis definition of an acid? Of a base?
15.30E) What is a general characteristic of a Lewis acid? Of a Lewis base?
15.31E) What is acid rain? What causes it and where is the problem the greatest?
15.15.25) How much NaOH (in grams) is needed to prepare 546 mL of solution with a pH of 10.00?
15.37E) ?Write the formula for the conjugate base of each acid. a. HCl b. H2SO3 c. HCHO2 d. HF
15.38E) ?Write the formula for the conjugate acid of each base. a. NH3 b. ClO4- c. HSO4- d. CO32-
15.15.27) Explain what is meant by the strength of an acid
15.45E) ?Pick the stronger base from each pair. a. F- or Cl- b. NO2- or NO3- c. F- or ClO
15.46E) ?Pick the stronger base from each pair. a. ClO4- or ClO2- b. Cl- or H2O c. CN- or ClO
15.50E) ?Calculate [H3O+] and [OH-] for each solution. a. pH = 8.55 b. pH = 11.23 c. pH = 2.87
15.51E) ?Complete the table. (All solutions are at \(25\ ^{\circ}\mathrm{C}\).)
15.52E) ?Complete the table. (All solutions are at 25 oC.)
15.15.81) Calculate the pH of a 0.36 M CH3COONa solution.
15.63E) ?Determine the [H3O+] and pH of a 0.100 M solution of benzoic acid.
15.15.82) Calculate the pH of a 0.42 M NH4Cl solution.
15.64E) ?Determine the [H3O+] and pH of a 0.200 M solution of formic acid.
15.15.83) Predict the pH (. 7, , 7, < 7) of a NaHCO3 solution.
15.71E) Determine the percent ionization of a 0.125 M HCN solution.
15.72E) ?Determine the percent ionization of a 0.225 M solution of benzoic acid.
15.15.84) Predict whether a solution containing the salt K2HPO4 will be acidic, neutral, or basic.
15.15.86) Write equations for the reactions between (a) CO2 and NaOH(aq), (b) Na2O and HNO3(aq).
15.89E) ?Determine the [OH-], pH, and pOH of a 0.15 M ammonia solution.
15.90E) ?Determine the [OH-], pH, and pOH of a solution that is 0.125 M in CO32-.
15.15.37) Predict the direction that predominates in this reaction: F2(aq) 1 H2O(l) HF(aq) 1 OH2(aq)
15.94E) ?A 0.135 M solution of a weak base has a pH of 11.23. Determine Kb for the base.
15.97E) ?Determine the [OH-] and pH of a solution that is 0.140 M in F-.
15.98E) ?Determine the [OH-] and pH of a solution that is 0.250 M in HCO3-.
15.15.29) What does the ionization constant tell us about the strength of an acid?
15.104E) ?Arrange the solutions in order of increasing basicity. CH3NH3Br, KOH, KBr, KCN, C5H5NHNO2
15.105E) ?Determine the pH of each solution. a. 0.10 M NH4Cl b. 0.10 M NaC2H3O2 c. 0.10 M NaCl
15.107E) Calculate the concentration of all species in a 0.15 M KF solution.
15.15.4) List the factors on which the Ka of a weak acid depends.
15.108E) ?Calculate the concentration of all species in a 0.225 M C6H5NH3Cl solution.
15.113E) ?Calculate the concentration of all species in a 0.500 M solution of H2SO3.
15.114E) ?Calculate the concentration of all species in a 0.155 M solution of H2CO3.
15.121E) ?Which is a stronger base, S2- or Se2-? Explain.
15.122E) ?Which is a stronger base, PO43- or AsO43-? Explain.
15.123E) ?Classify each species as either a Lewis acid or a Lewis base. a. Fe3+ b. BH3 c. NH3 d. F-
15.15.147) Calculate the pH and percent ionization of a 0.80 M HNO2 solution.
15.126E) ?Identify the Lewis acid and Lewis base from among the reactants in each equation.
15.127E) ?Based on these molecular views, determine whether each pictured acid is weak or strong.
15.128E) ?Based on these molecular views, determine whether each pictured base is weak or strong.
15.15.97) Determine the concentration of a NaNO2 solution that has a pH of 8.22
15.15.98) Determine the concentration of a NH4Cl solution that has a pH of 5.64.
15.149E) ?Calculate the pH of a solution that is 0.00115 M in HCl and 0.0100 M in HClO2.
15.159E) ?Rank the acids in order of increasing acid strength. CH3COOH CH2ClCOOH CHCl2COOH CCl3COOH
15.15.102) The pH of a 0.0642 M solution of a monoprotic acid is 3.86. Is this a strong acid?
Summary of Chapter 15: Acids and Bases
Chapter 15: Acids and Bases includes 308 full step-by-step solutions. Since 308 problems in chapter 15: Acids and Bases have been answered, more than 1390065 students have viewed full step-by-step solutions from this chapter. This expansive textbook survival guide covers the following chapters and their solutions. Chemistry: A Molecular Approach was written by and is associated to the ISBN: 9780321809247. This textbook survival guide was created for the textbook: Chemistry: A Molecular Approach, edition: 3.
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activation energy (Ea).
The minimum amount of energy required to initiate a chemical reaction. (13.4)
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atomic number (Z).
The number of protons in the nucleus of an atom. (2.3)
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battery
A self-contained electrochemical power source that contains one or more voltaic cells. (Section 20.7)
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carbide
A binary compound of carbon with a metal or metalloid. (Section 22.9)
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dipole-dipole interactions
Theresulting net attraction between two dipoles.
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E2
A bimolecular b-elimination reaction.
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energy
The capacity to do work or to transfer heat. (Section 5.1)
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Energy diagram
A graph showing the changes in energy that occur during a chemical reaction; energy is plotted on the vertical axis, and reaction progress is plotted on the horizontal axis. Also called a reaction coordinate diagram
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Epoxide
A cyclic ether in which oxygen is one atom of a three-membered ring
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fragmentation
In mass spectrometry, when the molecular ion breaks apart into fragments.
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Ka
A measure of the strength of an acid: Ka = Keq 3H2O4 = 3H3O+ 4 3A- 4 3HA4
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nucleophilic acyl substitution
A reaction in which a nucleophile attacks a carboxylic acid derivative.
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Organometallic compound
A compound that contains a carbon-metal bond.
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overall reaction order
The sum of the reaction orders of all the reactants appearing in the rate expression when the rate can be expressed as rate = k3A4a 3B4b... . (Section 14.3)
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primitive lattice
A crystal lattice in which the lattice points are located only at the corners of each unit cell. (Section 12.2)
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reaction quotient (Q)
The value that is obtained when concentrations of reactants and products are inserted into the equilibrium expression. If the concentrations are equilibrium concentrations, Q = K; otherwise, Q ? K. (Section 15.6)
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spin magnetic quantum number 1ms2
A quantum number associated with the electron spin; it may have values of +12 or -12. (Section 6.7)
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spontaneous
A reaction with a negative DG, which means that products are favored at equilibrium.
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Stereochemistry
The study of three-dimensional arrangements of atoms in molecules
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Ylide
A neutral molecule with positive and negative charges on adjacent atoms