Chemistry 10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
1 Chemical Foundations 2 Atoms, Molecules, And Ions 3 Stoichiometry 4 Types Of Chemical Reactions And Solution Stoichiometry 5 Gases 6 Thermochemistry 7 Atomic Structure And Periodicity 8 Bonding: General Concepts 9 Covalent Bonding: Orbitals 10 Liquids And Solids 11 Properties Of Solutions 12 Chemical Kinetics 13 Chemical Equilibrium 14 Acids And Bases 15 Acid-base Equilibria 16 Solubility And Complex Ion Equilibria 17 Spontaneity, Entropy, And Free Energy 18 Electrochemistry 19 The Nucleus: A Chemist's View 20 The Representative Elements 21 Transition Metals And Coordination Chemistry 22 Organic And Biological Molecules Chapter15: Acid-base Equilibria
Chapter Questions Section: Chapter Questions
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 12Q 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 34E Problem 35E: Calculate the pH of a solution that is 1.00 M HNO2 and 1.00 M NaNO2. Problem 36E: Calculate the pH of a solution that is 0.60 M HF and 1.00 M KF. 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 80E Problem 81E: Which of the indicators in Fig. 14-8 could be used for the titrations in Exercises 61 and 63? Problem 82E 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 94AE 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 99AE 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 102AE 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... Problem 133IP: Calculate the pH of a solution prepared by mixing 250. mL of 0.174 m aqueous HF (density = 1.10... Problem 134MP: Consider a solution prepared by mixing the foUowing: 50.0 mL of 0.100 M Na3PO4 100.0 mL of 0.0500 M... Problem 81E: Which of the indicators in Fig. 14-8 could be used for the titrations in Exercises 61 and 63?
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Ba2+(aq) + CrO42-(aq) ⇄ BaCrO4(s)
Do you think BaCrO4 is more soluble in acidic or in neutral solutions? Explain your answer using relevant chemical reactions. Attach a file if necessary.
Definition Definition Transformation of a chemical species into another chemical species. A chemical reaction consists of breaking existing bonds and forming new ones by changing the position of electrons. These reactions are best explained using a chemical equation.
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