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Science
Chemistry
EBK CHEMISTRY
Chapter 16, Problem 16.10P
Chapter 16, Problem 16.10P
BUY
EBK CHEMISTRY
8th Edition
ISBN:
9780135216972
Author: Robinson
Publisher:
PEARSON CO
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1 Chemical Tools Experimentation And Measurement
2 Atoms, Molecules, And Ions
3 Mass Relationships In Chemical Reactions
4 Reactions In Aqueous Solution
5 Periodicity And The Electronic Structure Of Atoms
6 Ionic Compounds Periodic Trends And Bonding Theory
7 Covalent Bonding And Electron-dot Structures
8 Covalent Compounds Bonding Theories And Molecular Structure
9 Thermochemistry Chemical Energy
10 Gases Their Properties And Behavior
11 Liquids And Phase Changes
12 Solids And Solid-state Materials
13 Solutions And Their Properties
14 Chemical Kinetics
15 Chemical Equilibrium
16 Aqueous Equilibria: Acids And Bases
17 Applications Of Aqueous Equilibria
18 Thermodynamics: Entropy, Free Energy, And Spontaneity
19 Electrochemistry
20 Nuclear Chemistry
21 Transition Elements And Coordination Chemistry
22 The Main-group Elements
23 Organic And Biological Chemistry
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Chapter Questions
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Problem 16.1P: Write a balanced equation for the dissociation of the Bronsted-Lowry acid, HSO4- , in water.
Problem 16.2A: Write the reaction between the carbonate ion (CO32) and water.
Problem 16.3P: Conceptual PRACTICE 15.3 For the following reaction in aqueous solution, identify the Brønsted-Lowry...
Problem 16.4A: Conceptual APPLY 15.4 For the following reactions in aqueous solution, identify the Brønsted—Lowry...
Problem 16.5P: If you mix equal concentrations of reactants and products, will the reaction proceed to the right or...
Problem 16.6A: Conceptual APPLY 15.6 The following pictures represent aqueous solutions of two acids HA (A = X or...
Problem 16.7P: Which pair has the stronger acid listed first? H2S and H2Se HNO2 and HNO3 H2Te and HI H2SO3 and...
Problem 16.8A: Which acid is stronger, H3PO4orH3AsO4?
Problem 16.9P: PRACTICE 15.9 The concentration of H3O+ ions in the runoff from a coal mine is 1.4 10-4 M....
Problem 16.10P
Problem 16.11P: Calculate the pH of a sample of seawater that has an OH- concentration of 1.5810-6M .
Problem 16.12A: During mining operations, the mineral pyrite (FeS2) is exposed to air and oxygen and reacts to...
Problem 16.13P: Calculate the concentrations of H3O+ and OH- in a cola beverage (pH2.80).
Problem 16.14P
Problem 16.15P: Calculate the pH of the following solutions: (a) 0.050MHClO4(b) 0.010MBa(OH)2
Problem 16.16A: Calculate the pH of a solution prepared by dissolving 0.25 g of CaO in enough water to make 1.50 L...
Problem 16.17A
Problem 16.18A: The following pictures represent aqueous solutions of three acids HA(A=X,YorZ); water molecules have...
Problem 16.19P: Acetic acid, CH3CO2H, is the solute that gives vinegar its characteristic odor and sour taste....
Problem 16.20A: Wha concentration of formic acid will result in a solution with pH=2.00? Refer to Table 16.2 to find...
Problem 16.21P: Calculate the pH and the concentration of all species present in 0.10M ascorbic acid (H2C6H6O6)...
Problem 16.22A: Carbonated drinks are prepared by dissolving CO2 under high pressure. CO2 reacts with water to...
Problem 16.23P: Calculate the pH and the concentrations of all species present in 0.40 M NH3(Kb=1.8105)
Problem 16.24A: Lactated Ringers solution is given intravenously to replenish fluids in patients who have...
Problem 16.25P
Problem 16.26A: The following pictures represent aqueous solutions of three acids HA(A=X,Y,orZ); water molecules...
Problem 16.27P: Predict whether a solution of 0.20 M NaNO2 is neutral, acidic, or basic, and calculate the pH....
Problem 16.28A: Calculate the pH and percent dissociation of Zn(H2O)62+ prepared from a 0.40 M ZnCl2 solution. Ka...
Problem 16.29P
Problem 16.30A: For the following Lewis acid— base reaction, draw electron-dot structures for the reactants and...
Problem 16.31P: What are the chemical formulas and names of the two acids that are the largest contributors to acid...
Problem 16.32P: What were the average pH ranges for rainfall in the eastern United States in 1985 and 2016? Refer to...
Problem 16.33P
Problem 16.34P: (a) Natural or “unpolluted” rain has a pH of 5.6. By what fact or has the concentration of H3O+...
Problem 16.35P
Problem 16.36P
Problem 16.37P: Because sulfur and nitrogen oxides are the main causes of acid rain, elevated levels of NO3- and...
Problem 16.38CP
Problem 16.39CP: The following pictures represent aqueous solutions of three acids HA(A=X,Y,orZ); water molecules...
Problem 16.40CP: Locate sulfur, selenium, chlorine, and bromine in the perioodic table: Which binary acid...
Problem 16.41CP
Problem 16.42CP
Problem 16.43CP: The followign pictures represent solutions of three salts NaA(A-=X-,Y-,orZ-) ; water molecules and...
Problem 16.44CP
Problem 16.45CP: Look at the electron-dot structures of the following molecules and ions: (a) Which of these...
Problem 16.46CP: Boric acid (H3BO3) is a weak monoprotic acid that yields H3O+ ions in water H3BO3 might behave...
Problem 16.47CP
Problem 16.48SP
Problem 16.49SP: Which of the following can behave both as a Bronsted-Lowry acid and as a Bronsted-Lowry base? (a)...
Problem 16.50SP: Give the formula for the conjugate base of each of the following Bronsted-Lowry acids. HSO4 H2SO3...
Problem 16.51SP: Give the formula for the conjugate acid of each of the following Bronsted-Lowry bases. SO32 H2O...
Problem 16.52SP: For each of the following reactions, identify the Bronsted-Lowry acids and bases and the conjugate...
Problem 16.53SP: For each of the following reactions, identify the Bronsted-Lowry acids and bases and the conjugate...
Problem 16.54SP: Aqueous solutions of hydrogen sulfide contain H2S,HS-,S2-,H3O+ , OH-, and H2O- in varying...
Problem 16.55SP
Problem 16.56SP: Choose from the conjugate acid-base pairs HSO4-/SO4 , HF/F-, and HF/F-,NH4+/NH3 to complete the...
Problem 16.57SP
Problem 16.58SP
Problem 16.59SP
Problem 16.60SP: Arrange each group of compounds in order of increasing acid strength. Explain your reasoning....
Problem 16.61SP: Arrange each group of compounds in order of increasing acid strength. Explain your reasoning....
Problem 16.62SP
Problem 16.63SP: Identify the weakest acid in each of the following sets. Explain your reasoning. H2SO3,HClO3,HClO4...
Problem 16.64SP
Problem 16.65SP: Identify the stronger base in each of the following pairs. Explain your reasoning. ClO2-orClO3...
Problem 16.66SP
Problem 16.67SP
Problem 16.68SP: The concentration of OH- in a sample of seawater is 2.0106M. Calculate the concentration of H3O+...
Problem 16.69SP: The concentration of OH- in human blood is 2.24107M. Calculate the concentration of H3O+ ions, and...
Problem 16.70SP: For each of the following solutions, calculate [OH-] from [H3O+]or[H3O+]from[OH-]. Classify each...
Problem 16.71SP: For each of the following solutions, calculate [OH-] from [H3O+]or[H3O+]from[OH-]. Classify each...
Problem 16.72SP: Water superheated under pressure to 200oC and 750 atm has Kw=1.51011 . What is [OH] at 200 oC? Is...
Problem 16.73SP: Water at 500oC and 250 atm is a supercritical fluid. Under these conditions, Kw is approximately...
Problem 16.74SP: Calculate the pH to the correct number of significant figures for solutions with the following...
Problem 16.75SP: Calculate the pH to the correct number of significant figures for solutions with the following...
Problem 16.76SP: Calculate the H3O+ concentration to the correct number of significant figures for solutions with the...
Problem 16.77SP: Calculate the H3O+ concentration to the correct number of significant figures for solutions with the...
Problem 16.78SP
Problem 16.79SP: Which of the indicators given in Figure 16.5, methyl violet, bromcresol green, phenol red, or...
Problem 16.80SP: Which of the following species behave a strong acids or as strong bases in aqueous solutions? HNO2...
Problem 16.81SP: Which of the following species behave as strong acids or as strong bases in aqueous solution? H- O2...
Problem 16.82SP: Calculate the pH of the following solutions: 1.010-3MSr(OH)2 0.015MHNO3 0.035MNaOH
Problem 16.83SP: Calculate the pH of the following solutions: 0.48 M HCl 2.5103MBa(OH)2 0.075 M NaOH
Problem 16.84SP
Problem 16.85SP: Calculate the pH of solutions prepared by: RAN (a) Dissolving 0.20 g of sodium oxide in water to...
Problem 16.86SP: How many grams of CaO should be dissolved in sufficient water to make 1.00 L of a solution with pH...
Problem 16.87SP
Problem 16.88SP: Look up the value of Ka in Appendix C for C6H5OH,HNO3,CH3CO2H and HOCl, and arrange these acids in...
Problem 16.89SP: Look up the value of Ka in Appendix C for HCO2H,HCN,HClO4, and HOBr, and arrange these acids in...
Problem 16.90SP: The pH of 0.040 M hypobromous acid (HOBr) is 5.05. Set up the equilibrium equation for the...
Problem 16.91SP: Lactic acid (C3H6O3) , which occurs in sour milk and foods such as sauerkraut, is a weak mnonprotic...
Problem 16.92SP: The pH of 0.050 M gallic acid, an acid found in tea leaves, is 2.86. Calculate Ka and pKa for gallic...
Problem 16.93SP: The pH of 0.040 M pyruvic acid, an acid found in tea leaves, is 2.86. Calculate Ka and pKa for...
Problem 16.94SP: A vitamin C tablet containing 250 mg of ascorbic acid (C6H8O6;Ka=8.010-5) is dissolved in a 250 mL...
Problem 16.95SP: Acetic acid (CH3COOH;Ka=1.810-5) has a concentration in vinegar of 3.50 by mass. What is the pH of...
Problem 16.96SP: Acrylic acid (HC3H3O2) is used in the manufacture of paints and plastics. The pKa of acrylic acid is...
Problem 16.97SP: Hippuric acid (HC9H8NO3) , found in horse urine, has pKa=3.62. Calculate the pH and the...
Problem 16.98SP: Calculat the pH and the percent dissociation in 1.5 M HNO2(Ka=4.5104).
Problem 16.99SP: A typical aspirin tablet contains 324 mg of aspirin (acetylsalicylic acid, (C9H8O4) , a monoprotic...
Problem 16.100SP
Problem 16.101SP: Calculate the percent dissociation of HNO2(Ka=4.5104) in 0.010 M HNO2 1.00 M HNO2
Problem 16.102SP: Write balanced net ionic equations and the corresponding equilibrium equations for the stepwise...
Problem 16.103SP: Write balanced net ionic equations and the corresponding equilibrium equations for the stepwise...
Problem 16.104SP: Calculate the pH and the concentrations of all species present (H2CO3,HCO3,CO32,H3O+,andOH) in 0.010...
Problem 16.105SP
Problem 16.106SP
Problem 16.107SP: Tartaric acid (C4H6O6) is a diprotic acid that plays an important role in lowering the pH of wine to...
Problem 16.108SP: Like sulfuric acid, selenic acid (H2SeO4) is a diprotic acid that has a very large value of Ka1 ....
Problem 16.109SP: Calculate the concentrations of H3O+ and SO42- in a solution prepared by mixing equal of 0.2 M HCl...
Problem 16.110SP
Problem 16.111SP
Problem 16.112SP: Write a balanced net ionic equation and the corresponding equilibrium equation for the reaction of...
Problem 16.113SP: Write a balanced net ionic equation and the corresponding equilibrium equation for the reaction of...
Problem 16.114SP: Styrchine (C21H22N2O2) , a deadly poison used for killing rodents, is a weak base having Kb=1.8106 ....
Problem 16.115SP: What is the pH of 0.5 M ammonia (NH3)?(Kb=1.8105)
Problem 16.116SP: Morphine (C17H19NO3), a narcotic used in painkillers, is a weak organic base. If the pH of a 7.0104...
Problem 16.117SP: A 1.00103M solution of quinine, a drug used in treating malaria, has a pH of 9.75. What are the...
Problem 16.118SP: Oxycodone (C18H21NO4), a narcotic analgesic, is a week base with pKb=5.47 . Calcualte the pH and the...
Problem 16.119SP: Morpholine (C4H9NO) is a weak organic base with pKb=5.68. Calculate the pH and the concentrations of...
Problem 16.120SP: Using values of Kb in Appendix C, calculate values of Ka for each of the following ions....
Problem 16.121SP: Using values of Ka in Appendix C, calculate values of Kb for each of the following ions. Fluoride...
Problem 16.122SP
Problem 16.123SP: Sodium benzoate (C6H5CO2Na) is used as a food preservative. Calculate the pH and the concentrations...
Problem 16.124SP: Write a balanced net ionic equation for the reaction of each of the following ions with water. In...
Problem 16.125SP: Write a balanced net ioflk equation for the principal react ion in solutions of each of the...
Problem 16.126SP: Classify each of the following ions according to whether they react with water to give a neutral,...
Problem 16.127SP: Classify each of the following salt solutions as neutral, acidic, or basic. See Appendix C for...
Problem 16.128SP: Calculate the concentrations of all species present and the pH in 0.10 M solutions of the following...
Problem 16.129SP
Problem 16.130SP: Calculate Ka for the cation Kb for the anion in an aqueous NH4CN solution. Is the solution acidic,...
Problem 16.131SP: Classify each of the following salt solutions as acidic, basic, or neutral. KBr NaNO2 NH4Br ZnCl2...
Problem 16.132SP
Problem 16.133SP: Classify each of the following salt solutions as neutral, acidic, or basic. See Appendix C for...
Problem 16.134SP: Calculate the pH and the concentrations of all species present RAN in 0.25 M solutions of each of...
Problem 16.135SP: Calculate the pH and the percent dissociation of the hydrat ed cation in the following solutions....
Problem 16.136SP
Problem 16.137SP
Problem 16.138SP
Problem 16.139SP: For each of the following reactions, identify the Lewis acid and the Lewis base. 2Cl-+BeCl2BeCl42...
Problem 16.140SP
Problem 16.141SP: For each of the Lewis acid—base reactions in Problem 16.139, draw electron-dot structures for the...
Problem 16.142SP
Problem 16.143SP
Problem 16.144MP
Problem 16.145MP
Problem 16.146MP
Problem 16.147MP
Problem 16.148MP: Normal rain has a pH of 5.6 due to dissolved atmospheric carbon dioxide at a current level of 400...
Problem 16.149MP: Sulfur dioxide is quite soluble in water: SO2(g)+H2O(l)H2SO3(aq)K=1.33 The H2SO3 produced is a weak...
Problem 16.150MP
Problem 16.151MP: Acid and base behavior can be observed in solvents other than water. One commonly used solvent is...
Problem 16.152MP
Problem 16.153MP: In the case of very weak acids, [H3O+] from the dissoc iation of water is significant compared with...
Problem 16.154MP
Problem 16.155MP
Problem 16.156MP: Neutralization reactions involving either a strong acid or a strong base go essentially to...
Problem 16.157MP
Problem 16.158MP
Problem 16.159MP: A 200.0 mL sample of 0.350 M acetic acid (CH3CO2H) was allowed to react with 2.000 L of gaseous...
Problem 16.160MP
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