Study Guide for Zumdahl/Zumdahl/DeCoste...10th EditionSteven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste Publisher: Cengage LearningISBN: 9781305957473
Study Guide for Zumdahl/Zumdahl/DeCoste...
Solutions for Study Guide for Zumdahl/Zumdahl/DeCoste’s Chemistry, 10th Edition
Problem 1RQ:
What is meant by the presence of a common ion? How does the presence of a common ion affect an...Problem 2RQ:
Define a buffer solution. What makes up a buffer solution? How do buffers absorb added H+ or OH with...Problem 3RQ:
One of the most challenging parts of solving acidbase problems is writing out the correct equation....Problem 4RQ:
A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If...Problem 5RQ:
Draw the general titration curve for a strong acid titrated by a strong base. At the various points...Problem 6RQ:
Instead of the titration of a strong acid by a strong base considered in Question 5, consider the...Problem 7RQ:
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations...Problem 8RQ:
Sketch the titration curve for a weak base titrated by a strong acid. Weak basestrong acid titration...Problem 9RQ:
What is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a...Problem 10RQ:
Why does an indicator change from its acid color to its base color over a range of pH values? In...Problem 1ALQ:
What are the major species in solution after NaHSO4 is dissolved in water? What happens to the pH of...Problem 2ALQ:
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt...Problem 3ALQ:
Mixing together solutions of acetic acid and sodium hydroxide can make a buffered solution. Explain....Problem 5ALQ:
Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong...Problem 6ALQ:
Sketch a pH curve for the titration of a weak acid (HA) with a strong base (NaOH). List the major...Problem 7ALQ:
You have a solution of the weak acid HA and add some HCl to it. What are the major species in the...Problem 8ALQ:
You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major...Problem 11Q:
The common ion effect for weak acids is to significantly decrease the dissociation of the acid in...Problem 13Q:
A best buffer has about equal quantities of weak acid and conjugate base present as well as having a...Problem 14Q:
Consider the following pH curves for 100.0 mL of two different acids with the same initial...Problem 15Q:
An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker...Problem 16Q:
Consider the following four titrations. i. 100.0 mL of 0.10 M HCl titrated by 0.10 M NaOH ii. 100.0...Problem 17Q:
Figure 14-4 shows the pH curves for the titrations of six different acids by NaOH. Make a similar...Problem 18Q:
Acidbase indicators mark the end point of titrations by magically turning a different color. Explain...Problem 19Q:
Consider the titration of 100.0 mL of 0.10 M H3AsO4 by 0.10 M NaOH. What are the major species...Problem 20Q:
Consider the following two acids: pKa1 = 2.98; pKa2 = 13.40 HO2CCH2CH2CH2CH2CO2H Adipic acid pKa1 =...Problem 21E:
How many of the following are buffered solutions? Explain your answer. Note: Counter-ions and water...Problem 22E:
Which of the following can be classified as buffer solutions? a. 0.25 M HBr + 0.25 M HOBr b. 0.15 M...Problem 23E:
A certain buffer is made by dissolving NaHCO3 and Na2CO3 in some water. Write equations to show how...Problem 24E:
A buffer is prepared by dissolving HONH2 and HONH3NO3 in some water. Write equations to show how...Problem 25E:
Calculate the pH of each of the following solutions. a. 0.100 M propanoic acid (HC3H5O2, Ka = 1.3 ...Problem 26E:
Calculate the pH of each of the following solutions. a. 0.100 M HONH2 (Kb= 1.1 108) b. 0.100 M...Problem 27E:
Compare the percent dissociation of the acid in Exercise 21a with the percent dissociation of the...Problem 28E:
Compare the percent ionization of the base in Exercise 22a with the percent ionization of the base...Problem 29E:
Calculate the pH after 0.020 mole of HCl is added to 1.00 L of each of the four solutions in...Problem 30E:
Calculate the pH after 0.020 mole of HCl is added to 1.00 L of each of the four solutions in...Problem 31E:
Calculate the pH after 0.020 mole of NaOH is added to 1.00 L of each of the four solutions in...Problem 32E:
Calculate the pH after 0.020 mole of NaOH is added to 1.00 L of each of the solutions in Exercise...Problem 33E:
Which of the solutions in Exercise 21 shows the least change in pH upon the addition of acid or...Problem 37E:
Calculate the pH after 0.10 mole of NaOH is added to 1.00 L of the solution in Exercise 31, and...Problem 38E:
Calculate the pH after 0.10 mole of NaOH is added to 1.00 L of the solution in Exercise 32, and...Problem 39E:
Calculate the pH of each of the following buffered solutions. a. 0.10 M acetic acid/0.25 M sodium...Problem 40E:
Calculate the pH of each of the following buffered solutions. a. 0.50 M C2H5NH2/0.25 M C2H5NH3Cl b....Problem 41E:
Calculate the pH of a buffered solution prepared by dissolving 21.5 g benzoic acid (HC7H5O2) and...Problem 42E:
A buffered solution is made by adding 50.0 g NH4Cl to 1.00 L of a 0.75-M solution of NH3. Calculate...Problem 43E:
Calculate the pH after 0.010 mole of gaseous HCl is added to 250.0 mL of each of the following...Problem 44E:
Calculate the pH after 0.15 mole of solid NaOH is added to 1.00 L of each of the following...Problem 45E:
Some K2SO3 and KHSO3 are dissolved in 250.0 mL of solution and the resulting pH is 7.25. Which is...Problem 46E:
An aqueous solution contains dissolved C6H5NH3Cl and C6H5NH2. The concentration of C6H5NH2 is 0.50 M...Problem 47E:
Calculate the mass of sodium acetate that must be added to 500.0 mL of 0.200 M acetic acid to form a...Problem 48E:
What volumes of 0.50 M HNO2 and 0.50 M NaNO2 must be mixed to prepare 1.00 L of a solution buffered...Problem 49E:
Consider a solution that contains both C5H5N and C5H5NHNO3. Calculate the ratio [C5H5N]/[C5H5NH+] if...Problem 50E:
Calculate the ratio [NH3]/[NH4+] in ammonia/ammonium chloride buffered solutions with the following...Problem 51E:
Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid...Problem 52E:
When a person exercises, muscle contractions produce lactic acid. Moderate increases in lactic acid...Problem 53E:
Consider the acids in Table 13-2. Which acid would be the best choice for preparing a pH = 7.00...Problem 54E:
Consider the bases in Table 13-3. Which base would be the best choice for preparing a pH = 5.00...Problem 55E:
Calculate the pH of a solution that is 0.40 M H2NNH2 and 0.80 M H2NNH3NO3. In order for this buffer...Problem 56E:
Calculate the pH of a solution that is 0.20 M HOCl and 0.90 M KOCl. In order for this buffer to have...Problem 57E:
Which of the following mixtures would result in buffered solutions when 1.0 L of each of the two...Problem 58E:
Which of the following mixtures would result in a buffered solution when 1.0 L of each of the two...Problem 59E:
What quantity (moles) of NaOH must be added to 1.0 L of 2.0 M HC2H3O2 to produce a solution buffered...Problem 60E:
Calculate the number of moles of HCl(g) that must be added to 1.0 L of 1.0 M NaC2H3O2 to produce a...Problem 61E:
Consider the titration of a generic weak acid HA with a strong base that gives the following...Problem 62E:
Sketch the titration curve for the titration of a generic weak base B with a strong acid. The...Problem 63E:
Consider the titration of 40.0 mL of 0.200 M HClO4 by 0.100 M KOH. Calculate the pH of the resulting...Problem 64E:
Consider the titration of 80.0 mL of 0.100 M Ba(OH)2 by 0.400 M HCl. Calculate the pH of the...Problem 65E:
Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 105) by 0.100 M KOH. Calculate...Problem 66E:
Consider the titration of 100.0 mL of 0.100 M H2NNH2 (Kb = 3.0 106) by 0.200 M HNO3. Calculate the...Problem 67E:
Lactic acid is a common by-product of cellular respiration and is often said to cause the burn...Problem 68E:
Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M propanoic acid...Problem 69E:
Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M NH3 (Kb = 1.8 105)...Problem 70E:
Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M pyridine with 0.100...Problem 71E:
Calculate the pH at the halfway point and at the equivalence point for each of the following...Problem 72E:
In the titration of 50.0 mL of 1.0 M methylamine, CH3NH2 (Kb = 4.4 104), with 0.50 M HC1, calculate...Problem 73E:
You have 75.0 mL of 0.10 M HA. After adding 30.0 mL 0.10 M NaOH, the pH is 5.50. What is the Ka...Problem 74E:
A student dissolves 0.0100 mole of an unknown weak base in 100.0 mL water and titrates the solution...Problem 75E:
Two drops of indicator HIn (Ka = 1.0 109), where HIn is yellow and In is blue, are placed in 100.0...Problem 76E:
Methyl red has the following structure: It undergoes a color change from red to yellow as a solution...Problem 77E:
Potassium hydrogen phthalate, known as KHP (molar mass = 204.22 g/mol), can be obtained in high...Problem 78E:
A certain indicator HIn has a pKa of 3.00 and a color change becomes visible when 7.00% of the...Problem 79E:
Which of the indicators in Fig. 14-8 could be used for the titrations in Exercises 57 and 59?Problem 81E:
Which of the indicators in Fig. 14-8 could be used for the titrations in Exercises 61 and 63?Problem 83E:
Estimate the pH of a solution in which bromcresol green is blue and thymol blue is yellow. (See Fig....Problem 84E:
Estimate the pH of a solution in which crystal violet is yellow and methyl orange is red. (See Fig....Problem 85E:
A solution has a pH of 7.0. What would be the color of the solution if each of the following...Problem 86E:
A solution has a pH of 4.5. What would be the color of the solution if each of the following...Problem 87AE:
When a diprotic acid, H2A. is titrated with NaOH, the protons on the diprotic acid are generally...Problem 88AE:
Consider die titration of 50.0 mL of 0.10 M H3A (Ka1 = 5.0 104, Ka2 = 1.0 108, Ka3 = 1.0 1012)...Problem 89AE:
Derive an equation analogous to the HendersonHasselbalch equation but relating pOH and pKb of a...Problem 90AE:
a. Calculate the pH of a buffered solution that is 0.100 M in C6H5CO2H (benzoic acid, Ka = 6.4 105)...Problem 91AE:
Tris(hydroxymethyl)aminomethane, commonly called TRIS or Trizma, is often used as a buffer in...Problem 92AE:
You make 1.00 L of a buffered solution (pH = 4.00) by mixing acetic acid and sodium acetate. You...Problem 93AE:
You have the following reagents on hand: Solids (pKa of Acid Form Is Given) Solutions Benzoic acid...Problem 95AE:
Phosphate buffers are important in regulating the pH of intracellular fluids at pH values generally...Problem 96AE:
When a diprotic acid, H2A, is titrated with NaOH, the protons on the diprotic acid are generally...Problem 97AE:
Consider the blood buffer system discussed in the Exercise 96. Patients with severe diarrhea can...Problem 98AE:
What quantity (moles) of HCl(g) must be added to 1.0 L of 2.0 M NaOH to achieve a pH of 0.00?...Problem 100AE:
The following plot shows the pH curves for the titrations of various acids by 0.10 M NaOH (all of...Problem 101AE:
Calculate the volume of 1.50 102 M NaOH that must be added to 500.0 mL of 0.200 M HCl to give a...Problem 103AE:
A certain acetic acid solution has pH = 2.68. Calculate the volume of 0.0975 M KOH required to reach...Problem 104AE:
A 0.210-g sample of an acid (molar mass = 192 g/mol) is titrated with 30.5 mL of 0.108 M NaOH to a...Problem 105AE:
The active ingredient in aspirin is acetylsalicylic acid. A 2.51-g sample of acetylsalicylic acid...Problem 106AE:
One method for determining the purity of aspirin (C9H8O4) is to hydrolyze it with NaOH solution and...Problem 107AE:
A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution...Problem 108AE:
A student titrates an unknown weak acid, HA, to a pale pink phenolphthalein end point with 25.0 mL...Problem 109AE:
A sample of a certain monoprotic weak acid was dissolved in water and titrated with 0.125 M NaOH,...Problem 110AE:
The pigment cyanidin aglycone is one of the anthocyanin molecules that gives red cabbage (Brassica...Problem 112CWP:
Consider 1.0 L of a solution that is 0.85 M HOC6H5 and 0.80 M NaOC6H5. (Ka for HOC6H5 = 1.6 1010.)...Problem 113CWP:
What concentration of NH4Cl is necessary to buffer a 0.52-M NH3 solution at pH= 9.00? (Kb for NH3 =...Problem 114CWP:
Consider the following acids and bases: HCO2H Ka = 1.8 104 HOBr Ka = 2.0 109 (C2H5)2NH Kb = 1.3 ...Problem 115CWP:
Consider a buffered solution containing CH3NH3Cl and CH3NH2. Which of the following statements...Problem 116CWP:
Consider the titration of 150.0 mL of 0.100 M HI by 0.250 M NaOH. a. Calculate the pH after 20.0 mL...Problem 117CWP:
Consider the titration of 100.0 mL of 0.100 M HCN by 0.100 M KOH at 25C. (Ka for HCN = 6.2 1010.)...Problem 118CWP:
Consider the titration of 100.0 mL of 0.200 M HONH2 by 0.100 M HCI. (Kb for HONH2 = 1.1 108.) a....Problem 119CWP:
Consider the following four titrations (iiv): i. 150 mL of 0.2 M NH3 (Kb = 1.8 105) by 0.2 M HCl...Problem 120CP:
Another way to treat data from a pH titration is to graph the absolute value of the change in pH per...Problem 121CP:
A buffer is made using 45.0 mL of 0.750 M HC3H5O2 (Ka = 1.3 105) and 55.0 mL of 0.700 M NaC3H5O2....Problem 122CP:
A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where...Problem 123CP:
What volume of 0.0100 M NaOH must be added to 1.00 L of 0.0500 M HOCl to achieve a pH of 8.00?Problem 124CP:
Consider a solution formed by mixing 50.0 mL of 0.100 M H2SO4, 30.0 mL of 0.100 M HOCI, 25.0 mL of...Problem 125CP:
Cacodylic acid, (CH3)2AsO2H, is a toxic compound that is a weak acid with pKa = 6.19. It is used to...Problem 127CP:
The titration of Na2CO3 with HCl bas the following qualitative profile: a. Identify the major...Problem 128CP:
Consider the titration curve in Exercise 115 for the titration of Na2Cr3 with HCl. a. If a mixture...Problem 129CP:
A few drops of each of the indicators shown in the accompanying table were placed in separate...Problem 130CP:
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH,...Problem 131IP:
A buffer solution is prepared by mixing 75.0 mL of 0.275 M fluorobenzoic acid (C7H5O2F) with 55.0 mL...Problem 132IP:
A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in...Browse All Chapters of This Textbook
Chapter 1 - Chemical FoundationsChapter 2 - Atoms, Molecules, And IonsChapter 3 - StoichiometryChapter 4 - Types Of Chemical Reactions And Solution StoichiometryChapter 5 - GasesChapter 6 - ThermochemistryChapter 7 - Atomic Structure And PeriodicityChapter 8 - Bonding: General ConceptsChapter 9 - Covalent Bonding: OrbitalsChapter 10 - Liquids And Solids
Chapter 11 - Properties Of SolutionsChapter 12 - Chemical KineticsChapter 13 - Chemical EquilibriumChapter 14 - Acids And BasesChapter 15 - Acid-base EquilibriaChapter 16 - Solubility And Complex Ion EquilibriaChapter 17 - Spontaneity, Entropy, And Free EnergyChapter 18 - ElectrochemistryChapter 19 - The Nucleus: A Chemist's ViewChapter 20 - The Representative ElementsChapter 21 - Transition Metals And Coordination ChemistryChapter 22 - Organic And Biological Molecules
Sample Solutions for this Textbook
We offer sample solutions for Study Guide for Zumdahl/Zumdahl/DeCoste’s Chemistry, 10th Edition homework problems. See examples below:
Chapter 1, Problem 1RQChapter 1, Problem 34EChapter 1, Problem 39EChapter 1, Problem 40EChapter 1, Problem 42EChapter 1, Problem 49EGiven data: The amount mercury in a polluted lake is 0.4 μg Hg/mL 0.4 μg/mL = 4 × 10-7 kg/LThe...Chapter 1, Problem 61EChapter 1, Problem 63E
Chapter 1, Problem 64EChapter 1, Problem 67EChapter 1, Problem 68EChapter 1, Problem 77EChapter 1, Problem 121CPChapter 2, Problem 1RQChapter 2, Problem 68EChapter 2, Problem 71EChapter 2, Problem 72EExplanation: Atomic number given is 13. From the periodic table we can identify that the element...Chapter 2, Problem 75EExplanation: To determine: The naming of CuI The name of CuI is copper(I) iodide. In naming of...Explanation: To determine: The naming of HC2H3O2 The naming of HC2H3O2 is acetic acid. Rules for...To determine: The formula of of sulfur difluoride The formula of sulfur difluoride is SF2 Sulfur...Explanation: To determine: The formula of sodium oxide. The formula of sodium oxide is Na2O The...Chapter 2, Problem 90EChapter 2, Problem 92EExplanation: To determine: The formula and the name of the binary compound formed from Ca and N. The...Explanation: Given, 1531X Atomic number, Z =15 Mass number, A =31 The atomic number of the element...Explanation: To determine: The explanation for the term “counting by weighing”. The stated concept,...Chapter 3, Problem 61EChapter 3, Problem 62EChapter 3, Problem 63EExplanation: Given The mass of P4O6 is 1.00 g . The molar mass of P4O6 is 219.866 g/mol . Formula...Chapter 3, Problem 69EChapter 3, Problem 70EChapter 3, Problem 73EChapter 3, Problem 75EChapter 3, Problem 78EChapter 3, Problem 81EChapter 3, Problem 102EChapter 3, Problem 103EChapter 3, Problem 115EChapter 3, Problem 125EChapter 3, Problem 127EChapter 3, Problem 132EChapter 3, Problem 152AEChapter 3, Problem 160AEChapter 3, Problem 162CWPChapter 3, Problem 192IPChapter 4, Problem 1RQChapter 4, Problem 7RQExplanation: NaBr(s)→Na(aq)++Braq- Figure 1 Let us consider the above molecular-level pictures of...Explanation: Record the given data Moles of Sodium phosphate= 0.200 moles Volume of the solution=...Chapter 4, Problem 85EChapter 4, Problem 88EChapter 4, Problem 91EChapter 4, Problem 92EChapter 4, Problem 93EChapter 4, Problem 94EChapter 4, Problem 107AEChapter 4, Problem 137CPExplanation Record the given data Mass of the sample mixture = 0.205 g Mass of the precipitate =...Chapter 4, Problem 154CPChapter 4, Problem 155CPChapter 4, Problem 161MPA barometer consists of Mercury column that is tipped inverted and positioned in a dish containing...Chapter 5, Problem 45EExplanation: The relation between pressures measured in the manometers containing mercury and...Explanation According to ideal gas equation, PV=nRT By rearranging the above equation, PVnT=R Since...Chapter 5, Problem 94EExplanation: To find: the mole fractions of CH4 and O2 in the given mixture if the partial pressure...Explanation To find: the number of moles of dimethyl hydrazine from its given mass. The number of...Explanation To determine: The partial pressure of carbon monoxide Partial pressure of carbon...Explanation To determine: The mixing ratio of benzene Mixing ratio of benzene = 9.47 × 10-3ppmv For...Chapter 5, Problem 143AEExplanation To find: the empirical formula of the compound Convert the mass percent to gram 58.51%...Chapter 5, Problem 147AEExplanation To find: the balanced chemical equation of the given reaction of combustion of...Chapter 5, Problem 160CPChapter 5, Problem 161CPExplanation To determine: Mass of hot air when the average molar mass of air 29.0g/mol Mass of hot...To determine: The mass percent of elements in the unknown compound from the given data Mass % of...Chapter 5, Problem 172IPChapter 6, Problem 1RQChapter 6, Problem 24QChapter 6, Problem 38EChapter 6, Problem 54EChapter 6, Problem 56EChapter 6, Problem 79EChapter 6, Problem 85EChapter 6, Problem 86EExplanation: The balanced equation is: a) N2(g)→N2(l) In (a) the volume of products is decreases...Chapter 6, Problem 114AEChapter 6, Problem 121AEChapter 6, Problem 136CPChapter 6, Problem 137CPChapter 6, Problem 143IPChapter 6, Problem 145MPChapter 7, Problem 1RQChapter 7, Problem 28QChapter 7, Problem 49EChapter 7, Problem 51EChapter 7, Problem 63EChapter 7, Problem 64EChapter 7, Problem 68EChapter 7, Problem 69EChapter 7, Problem 75EChapter 7, Problem 80EChapter 7, Problem 85EChapter 7, Problem 87EChapter 7, Problem 88EChapter 7, Problem 99EChapter 7, Problem 100EChapter 7, Problem 101EChapter 7, Problem 103EChapter 7, Problem 152AEChapter 7, Problem 179CPChapter 7, Problem 181CPChapter 8, Problem 1RQExplanation: Refer to figure 3-4. The electro negativity of carbon (C) , nitrogen (N) , and oxygen...Explanation: Refer to figure 3-4 The electro negativity of Sodium (Na) Potassium (K) and Rubidium...Chapter 8, Problem 50EChapter 8, Problem 51EChapter 8, Problem 53EExplanation: In a periodic table the size of ions depends on the nuclear attraction on the valence...Chapter 8, Problem 58EChapter 8, Problem 66EChapter 8, Problem 81EChapter 8, Problem 85EChapter 8, Problem 88EChapter 8, Problem 93EChapter 8, Problem 105EChapter 8, Problem 106EChapter 8, Problem 135AEChapter 8, Problem 162CPChapter 8, Problem 163CPChapter 9, Problem 1RQChapter 9, Problem 27EChapter 9, Problem 28EChapter 9, Problem 30EChapter 9, Problem 33EChapter 9, Problem 34EChapter 9, Problem 43EChapter 9, Problem 56EChapter 9, Problem 57EChapter 9, Problem 67AEChapter 9, Problem 95CPChapter 10, Problem 1RQChapter 10, Problem 43EExplanation: CCl4 , CBr4, CF4 Identify the compound which has highest boiling point and justify it....Chapter 10, Problem 55EChapter 10, Problem 57EChapter 10, Problem 58EChapter 10, Problem 59EChapter 10, Problem 60EChapter 10, Problem 61EChapter 10, Problem 62EChapter 10, Problem 64EChapter 10, Problem 80EChapter 10, Problem 82EChapter 10, Problem 90EChapter 10, Problem 141CPChapter 10, Problem 156CPChapter 10, Problem 158IPExplanation: To explain molarity Molarity can be defined as moles of solute to litres of solution....Chapter 11, Problem 18SRChapter 11, Problem 39EExplanation: Record the given data Gram equivalent of HCl = 0.25 Molarity of HCl = 0.25 M To...Explanation: KrF2 8+2(7)=22e- KrF2 is dissolves in CCl4 . KrF2 is non-polar molecule that makes it...Chapter 11, Problem 69EChapter 11, Problem 85EExplanation: Record the given data, Molality of MgCl2= 0.050 m Molality of FeCl3= 0.050 m To...Explanation: Record the given data, Molality of MgCl2= 0.050 m Molality of FeCl3= 0.050 m To...Explanation: To find the Acetone and water polarity CH3COCH3 and H2O The electrostatic possible...Explanation: Record the given data, Freezing point of an aqueous solution =- 2.79°C To calculate...Chapter 11, Problem 117AEChapter 11, Problem 128CPChapter 11, Problem 138CPChapter 11, Problem 142IPChapter 12, Problem 1RQChapter 12, Problem 29EChapter 12, Problem 32EChapter 12, Problem 35EChapter 12, Problem 37EChapter 12, Problem 38EChapter 12, Problem 60EChapter 12, Problem 88AEChapter 12, Problem 90AEChapter 12, Problem 91AEChapter 12, Problem 97AEChapter 12, Problem 101AEChapter 12, Problem 113CPChapter 12, Problem 122CPChapter 13, Problem 1RQChapter 13, Problem 5ALQChapter 13, Problem 27EChapter 13, Problem 38EChapter 13, Problem 45EChapter 13, Problem 48EChapter 13, Problem 60EChapter 13, Problem 62EChapter 13, Problem 63EChapter 13, Problem 82AEChapter 13, Problem 83AEChapter 13, Problem 88AEChapter 13, Problem 114CPChapter 13, Problem 116CPChapter 14, Problem 1RQChapter 14, Problem 53EChapter 14, Problem 65EChapter 14, Problem 66EChapter 14, Problem 70EChapter 14, Problem 74EChapter 14, Problem 75EChapter 14, Problem 98EChapter 14, Problem 101EChapter 14, Problem 107EChapter 14, Problem 108EChapter 14, Problem 109EChapter 14, Problem 119EChapter 14, Problem 120EChapter 14, Problem 123EChapter 14, Problem 125EChapter 14, Problem 126EChapter 14, Problem 153AEChapter 14, Problem 163AEChapter 14, Problem 172CWPChapter 15, Problem 1RQChapter 15, Problem 7RQChapter 15, Problem 49EChapter 15, Problem 63EChapter 15, Problem 64EChapter 15, Problem 65EChapter 15, Problem 66EChapter 15, Problem 67EChapter 15, Problem 68EChapter 15, Problem 69EChapter 15, Problem 70EChapter 15, Problem 71EExplanation The value of pH of solution when 0.0 mL NaOH has been added is. 1.0_ . Given: The...Chapter 15, Problem 119CWPChapter 16, Problem 1RQExplanation To determine: The solubility product of CaC2O4 . The concentration of Ca2+ is 4.8×10−5...Chapter 16, Problem 26EChapter 16, Problem 31EChapter 16, Problem 32EChapter 16, Problem 39EChapter 16, Problem 40EChapter 16, Problem 41EChapter 16, Problem 44EChapter 16, Problem 57EChapter 16, Problem 74EChapter 16, Problem 107CPChapter 16, Problem 108CPChapter 17, Problem 1RQChapter 17, Problem 57EChapter 17, Problem 59EChapter 17, Problem 69EChapter 17, Problem 70EChapter 17, Problem 74EChapter 17, Problem 76EChapter 17, Problem 78EChapter 17, Problem 80EChapter 17, Problem 84EChapter 17, Problem 93AEChapter 17, Problem 96AEChapter 17, Problem 100AEChapter 17, Problem 131MPChapter 18, Problem 1RQChapter 18, Problem 18RORRChapter 18, Problem 22RORRChapter 18, Problem 47EChapter 18, Problem 67EChapter 18, Problem 68EChapter 18, Problem 73EChapter 18, Problem 74EChapter 18, Problem 83EChapter 18, Problem 84EChapter 18, Problem 93EChapter 18, Problem 111AEChapter 18, Problem 113AEChapter 18, Problem 144CPExplanation The half cell reactions are, Anode: Hg→Hg2++2e− Eanodeο=0.242 V Cathode: 2Ag++2e−→2Ag...Chapter 18, Problem 153CPChapter 18, Problem 159MPExplanation (a) To define: The term thermodynamic stability. The thermodynamic stability is related...Explanation: Alpha particle is emitted. The parent nuclide is 232Th and the nuclide after the...Explanation The most stable isotope is 81Kr and the hottest one is 73Kr The nuclides having longer...Explanation Given The atomic mass of 232Pu is 3.85285×10−22 g . The mass of a neutron is...Explanation The atomic mass of 11H=1.0078 amu The mass of a neutron is 1.0087 amu . Mass of...Explanation To determine: The decay events per second in a 180−lb person. The number of atoms of 14C...Explanation Given The value of half life of 87Rb is 4.5×109 years . The decay constant is calculated...Explanation The decay constant is calculated by the formula given below. λ=0.693t1/2 Where t1/2 is...Explanation: The zirconium metal is capable of reducing water to form hydrogen gas at standard...Explanation The number of α and β particles produced are 4_ and 2_ . The mass number of 92238U is...Explanation The nuclear reaction for the synthesis of cobalt- 60 is, 2658Fe+201n→ 2760Co+ −10e . The...Chapter 20, Problem 1RQExplanation The valence electron configuration for halogens is ns2np5 . The common halogen elements...The stated reaction is, CH4(g)+H2O(g)⇌CO(g)+3H2(g) Refer to Appendix 4 The value of ΔH°(kJ/mol) for...Chapter 20, Problem 12QExplanation The value of ΔH° for the given reaction is 180 kJ_ . The stated reaction is,...Explanation: The compound XeO4 and IO4− ion are isoelectronic. The molecule xenon tetroxide (XeO4)...Explanation: The Lewis structure, molecular structure, bond angle and hybridization of central atom...Explanation: Hydrogen gas is produced by reacting graphite with water. C(s)+H2O(g)→CO(g)+H2(g) The...Explanation: The number of moles of hydrogen gas is 0.249 mol_. Given Mass of alkaline earth metal...Explanation: Mass of radon (Ra) is 25 g_ . Given Mass of pitch-blende is 1.75×108 g . The conversion...Explanation Given Temperature is 900 K . Pressure of In(CH3)3 is 2.00 atm . Volume of In(CH3)3 is...Chapter 20, Problem 118IPChapter 20, Problem 119IPChapter 21, Problem 1RQExplanation: (I) To determine: The geometry and associated bond angles when a metal ion has a...Valence electrons are filled in four principal orbitals according to the energy levels. The four...EXPLANATION (a) To write: The electron configuration of metal ion in (NH4)2[Fe(H2O)2Cl4] . The...Explanation The complex ion is [Ru(NH3)5Cl]2+. This ion contains positive charge. Oxidation state of...Explanation The complex compound is [Co(NH3)6]Cl2 . Oxidation state of Chlorine ion (Cl−) is −1 ....Explanation The complex compound is [Cr(H2O)5Br]Br2 . Oxidation state of Bromine ion (Br−) is −1 ....Explanation The value of ΔH° for the given reaction is −11 kJ_ . For the reaction,...Explanation The reaction that takes place is, 3Fe2O3(s)+CO(g)→2Fe3O4(s)+CO2(g) Refer to Appendix 4....The given compound is CoCl2.6H2O. It is used in novelty devices that predict rain. The coordination...Explanation The given equations are, Co+3+e−→Co+2 Eο=1.82 V (1) Co2++3en→Co(en)32+ K=1.5×1012 (2)...Chapter 21, Problem 107IPChapter 22, Problem 1RQChapter 22, Problem 5RQChapter 22, Problem 18EChapter 22, Problem 49EExplanation To determine: The monomer of the given polymer. The monomer is vinyl fluoride. It is an...Explanation The correct name of the compound is 2,3,5,6−Tetramethyl−octane whose structure is shown...Explanation The structure of the given compound 2,3,7,8−tetrachloro−dibenzo−p−dioxin is shown in...Chapter 22, Problem 142AEChapter 22, Problem 148AEChapter 22, Problem 158CPExplanation The equilibrium constant for the given reaction is 6.88×10−13_ . The equilibrium...Chapter 22, Problem 162CPExplanation The structure of C5H12 is shown in Figure 1. The structure of C5H12 is, Figure 1 The...Explanation The structure of the polymer of ABS plastic is shown in figure 1. The reaction of Abs...Chapter 22, Problem 171CPExplanation Given Electronic configuration of M+2 is [Ar]3d10. So, atomic number of M is 30. In...Explanation The empirical formula of the given helicene is C5H3 . Helicene is an aromatic compound...The correct responses are urea and Ammonium cyanate. The first organic compound that is synthesized...Explanation Aldohexose is a six carbon aldehyde sugar with an aldehyde group on one end.
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