Chemical Principles
8th Edition
ISBN: 9781337247269
Author: Steven S. Zumdahl; Donald J. DeCoste
Publisher: Cengage Learning US
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Chapter 8, Problem 20E
Derive an equation analogous to the Henderson— Hasselbalch equation that relates
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Phosphoric acid is a triprotic acid (?a1= 6.9×10^−3, ?a2= 6.2×10^−8, and ?a3= 4.8×10^−13).
To find the pH of a buffer composed of H2PO−4(aq) and HPO2−4(aq), which p?a value should be used in the Henderson–Hasselbalch equation?
p?a1 = 2.16
p?a2 = 7.21
p?a3 = 12.32
Calculate the pH of a buffer solution obtained by dissolving 11.0 g of KH2PO4(s) and 28.0 g of Na2HPO4(s) in water and then diluting to 1.00 L.
An analytical chemist is titrating 83.1 mL of a 0.2800M solution of piperidine (C5H₁0NH) with a 0.5900M solution of
HIO3. The p K of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 44.5 mL of the
HIO3 solution to it.
Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the
volume of HIO3 solution added.
Round your answer to 2 decimal places.
pH =
X
An analytical chemist is titrating 179.3 mL of a 0.3400M solution of benzoic acid (HC H,CO₂) with a 0.3300M solution of NaOH. The p K of benzoic acid is
4.20. Calculate the pH of the acid solution after the chemist has added 88.89 mL of the NaOH solution to it.
Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added.
Round your answer to 2 decimal places.
pH = 0
Chapter 8 Solutions
Chemical Principles
Ch. 8 - Prob. 1DQCh. 8 - Prob. 2DQCh. 8 - Mixing together solutions of acetic acid and...Ch. 8 - Sketch two pH curves, one for the titration of a...Ch. 8 - Sketch a pH curve for the titration of a weak acid...Ch. 8 - You have a solution of the weak acid HA and add...Ch. 8 - You have a solution of the weak acid HA and add...Ch. 8 - Prob. 8DQCh. 8 - You are browsing through the Handbook of...Ch. 8 - A friend tells you: "The constant Ksp of a salt is...
Ch. 8 - What happens to the Ksp value of a solid as the...Ch. 8 - Which is more likely to dissolve in an acidic...Ch. 8 - Prob. 13DQCh. 8 - Under what circumstances can the relative...Ch. 8 - Define a buffered solution. What makes up a...Ch. 8 - A good buffer generally contains relatively equal...Ch. 8 - How many of the following are buffered solutions?...Ch. 8 - Which of the following can be classified as buffer...Ch. 8 - Prob. 19ECh. 8 - Derive an equation analogous to the Henderson—...Ch. 8 - Calculate the pH of each of the following...Ch. 8 - Calculate the pH after 0.020 mole of HCl is added...Ch. 8 - Calculate the pH after 0.020 mole of NaOH is added...Ch. 8 - The results of Exercises 21-23 illustrate an...Ch. 8 - One of the most challenging parts of solving...Ch. 8 - a. Calculate the pH of a buffered solution that is...Ch. 8 - Calculate the pH of a solution that is...Ch. 8 - Calculate the pH of a solution that is...Ch. 8 - Calculate the pH after 0.10mole of NaOH is added...Ch. 8 - Calculate the pH after 0.020mole of NaOH is added...Ch. 8 - Calculate the pH of a solution that is 0.40M H 2...Ch. 8 - Calculate the pH of a solution that is...Ch. 8 - Calculate the pH of a buffered solution prepared...Ch. 8 - A buffered solution is made by adding...Ch. 8 - Prob. 35ECh. 8 - How many moles of NaOH must be added to...Ch. 8 - Calculate the number of moles of HCl(g) that must...Ch. 8 - You make 1.00L of a buffered solution (pH=4.00) by...Ch. 8 - Calculate the mass of sodium acetate that must be...Ch. 8 - Calculate the pH after 0.010mole of gaseous HCl is...Ch. 8 - An aqueous solution contains dissolved...Ch. 8 - What volumes of 0.50MHNO2and0.50MNaNO2 must be...Ch. 8 - Phosphate buffers are important in regulating the...Ch. 8 - Carbonate buffers are important in regulating the...Ch. 8 - When a person exercises, muscle contractions...Ch. 8 - Which of the following mixtures would result in a...Ch. 8 - Which of the following mixtures would result in a...Ch. 8 - Calculate the pH of a solution formed by mixing...Ch. 8 - Consider the acids in Table 7.2. Which acid would...Ch. 8 - Consider the bases in Table 7.3. Which base would...Ch. 8 - A solution contains 1.0106MHOCl and an unknown...Ch. 8 - In Section 8.3 an equation was derived for the...Ch. 8 - Consider a weak acid HA with a Ka value of 1.6107....Ch. 8 - Consider the following pH curves for 100.0mL of...Ch. 8 - An acid is titrated with NaOH. The following...Ch. 8 - Consider the titration of a generic weak acid HA...Ch. 8 - Sketch the titration curve for the titration of a...Ch. 8 - Draw the general titration curve for a strong acid...Ch. 8 - Consider the following four titrations:...Ch. 8 - A student titrates an unknown weak acid HA to a...Ch. 8 - The following plot shows the pH curves for the...Ch. 8 - The figure in the preceding exercise shows the pH...Ch. 8 - Consider the titration of...Ch. 8 - Prob. 64ECh. 8 - Prob. 65ECh. 8 - Prob. 66ECh. 8 - Prob. 67ECh. 8 - Prob. 68ECh. 8 - Prob. 69ECh. 8 - Prob. 70ECh. 8 - Calculate the pH at the halfway point and at the...Ch. 8 - You have 75.0mLof0.10MHA. After adding...Ch. 8 - A student dissolves 0.0100mole of an unknown weak...Ch. 8 - What is an acid—base indicator? Define the...Ch. 8 - Two drops of indicator HIn(Ka=1.0109), where HIn...Ch. 8 - A certain indicator HIn has a pKa of 3.00 and a...Ch. 8 - Estimate the pH of a solution in which bromcresol...Ch. 8 - A solution has a pHof7.0. What would be the color...Ch. 8 - Which of the indicators in Fig. 8.8 could be used...Ch. 8 - Which of the indicators in Fig. 8.8 could be used...Ch. 8 - Which of the indicators in Fig. 8.8 could be used...Ch. 8 - Which of the indicators in Fig. 8.8 could be used...Ch. 8 - Methyl red has the following structure: It...Ch. 8 - Indicators can be used to estimate the pH values...Ch. 8 - When a diprotic acid, H2A, is titrated with NaOH,...Ch. 8 - A student was given a 0.10M solution of an unknown...Ch. 8 - Prob. 87ECh. 8 - Consider 100.0mLofa0.100M solution of...Ch. 8 - A 0.200-g sample of a triprotic acid...Ch. 8 - Consider the titration of 100.0mLof0.100MH3A...Ch. 8 - The titration of Na2CO3 with HCl has the following...Ch. 8 - Consider 100.0 mL of a solution of 0.200MNa2A,...Ch. 8 - For which of the following is the Ksp value of the...Ch. 8 - Ag2S(s) has a larger molar solubility than CuS...Ch. 8 - When Na3PO4(aq) is added to a solution containing...Ch. 8 - The common ion effect for ionic solids (salts) is...Ch. 8 - Prob. 97ECh. 8 - Calculate the solubility of each of the following...Ch. 8 - Use the following data to calculate the Ksp value...Ch. 8 - The concentration of Pb2+ in a solution saturated...Ch. 8 - The concentration of Ag+ in a solution saturated...Ch. 8 - The solubility of the ionic compound M2X3, having...Ch. 8 - For each of the following pairs of solids,...Ch. 8 - The solubility rules outlined in Chapter 4 say...Ch. 8 - Calculate the molar solubility of...Ch. 8 - The Ksp for silver sulfate (Ag2SO4) is 1.2105....Ch. 8 - Calculate the solubility (inmol/L) of Fe(OH)3...Ch. 8 - Prob. 108ECh. 8 - Calculate the solubility of solid Ca3(...Ch. 8 - The solubility of Ce( IO3)3 in a 0.20MKIO3...Ch. 8 - What mass of ZnS(Ksp=2.51022) will dissolve in...Ch. 8 - The concentration of Mg2+ in seawater is 0.052M....Ch. 8 - For the substances in Exercises 97and98, which...Ch. 8 - Explain the following phenomenon: You have a test...Ch. 8 - For which salt in each of the following groups...Ch. 8 - A solution is prepared by mixing 75.0mL of...Ch. 8 - Calculate the final concentrations of...Ch. 8 - A solution is prepared by mixing 50.0mLof0.10M Pb(...Ch. 8 - The Ksp of Al(OH)3 is 21032. At what pH will a...Ch. 8 - A solution is 1104M in NaF,Na2S, and Na3PO4. What...Ch. 8 - A solution contains 1.0105MNa3PO4. What is the...Ch. 8 - A solution contains 0.25MNi( NO3)2 and 0.25MCu(...Ch. 8 - Describe how you could separate the ions in each...Ch. 8 - If a solution contains either Pb2+(aq)orAg+(aq),...Ch. 8 - Sulfide precipitates are generally grouped as...Ch. 8 - Nanotechnology has become an important field, with...Ch. 8 - Prob. 127ECh. 8 - As a sodium chloride solution is added to a...Ch. 8 - The overall formation constant for HgI42is1.01030....Ch. 8 - A solution is prepared by adding 0.090mole of...Ch. 8 - Prob. 131ECh. 8 - Kf for the complex ion Ag( NH3)2+is1.7107. Ksp for...Ch. 8 - a. Using the Ksp for Cu(OH)2(1.61019) and the...Ch. 8 - The copper(I) ion forms a chloride salt that has...Ch. 8 - Solutions of sodium thiosulfate are used to...Ch. 8 - a. Calculate the molar solubility of AgI in pure...Ch. 8 - A series of chemicals was added to some...Ch. 8 - Will a precipitate of Cd(OH)2 form if 1.0mLof1.0M...Ch. 8 - Tris(hydroxymethyl)aminomethane, commonly called...Ch. 8 - Amino acids are the building blocks for all...Ch. 8 - The solubility of copper(II) hydroxide in water...Ch. 8 - The salts in Table 8.5, with the possible...Ch. 8 - You have the following reagents on hand: What...Ch. 8 - Prob. 144AECh. 8 - One method for determining the purity of aspirin...Ch. 8 - Another way to treat data from a pH titration is...Ch. 8 - Potassium hydrogen phthalate, known as KHP...Ch. 8 - sample of the ionic compound NaA, where A is the...Ch. 8 - What mass of Ca( NO3)2 must be added to 1.0L of a...Ch. 8 - The equilibrium constant for the following...Ch. 8 - Calculate the concentration of Pb2+ in each of the...Ch. 8 - Consider saturated solutions of the following...Ch. 8 - A certain acetic acid solution has pH=2.68 ....Ch. 8 - Calculate the volume of 1.5010-2MNaOH that must be...Ch. 8 - A 0.400M solution of ammonia was titrated with...Ch. 8 - A student intends to titrate a solution of a weak...Ch. 8 - The active ingredient in aspirin is...Ch. 8 - A solution is formed by mixing 50.0mL of 10.0MNaX...Ch. 8 - When phosphoric acid is titrated with a NaOH...Ch. 8 - Consider the following two acids: In two separate...Ch. 8 - Consider 1.0L of a solution that is 0.85MHOC6H5...Ch. 8 - What concentration of NH4Cl is necessary to buffer...Ch. 8 - Consider the following acids and bases:...Ch. 8 - Consider a buffered solution containing CH3NH3Cl...Ch. 8 - Consider the titration of 150.0mL of 0.100MHI by...Ch. 8 - Prob. 166AECh. 8 - Prob. 167AECh. 8 - Prob. 168AECh. 8 - Assuming that the solubility of Ca3( PO4)2(s) is...Ch. 8 - Order the following solids (ad) from least soluble...Ch. 8 - The Ksp for PbI2(s) is 1.410-8 . Calculate the...Ch. 8 - Prob. 172AECh. 8 - A 50.0-mL sample of 0.0413MAgNO3(aq) is added to...Ch. 8 - The Hg2+ ion forms complex ions with I as follows:...Ch. 8 - A buffer is made using 45.0mL of...Ch. 8 - What volume of 0.0100MNaOH must be added to 1.00L...Ch. 8 - For solutions containing salts of the form NH4X ,...Ch. 8 - Prob. 178CPCh. 8 - The copper(I) ion forms a complex ion with CN...Ch. 8 - Calcium oxalate (CaC2O4) is relatively insoluble...Ch. 8 - a. Calculate the molar solubility of SrF2 in...Ch. 8 - What is the maximum possible concentration of Ni2+...Ch. 8 - Prob. 183CPCh. 8 - Consider 1.0L of an aqueous solution that contains...Ch. 8 - Calculate the solubility of AgCN(s)(Ksp=2.21012)...Ch. 8 - Consider the titration of 100.0mL of a 1.00104M...Ch. 8 - Consider a solution formed by mixing 200.0mL of...Ch. 8 - Prob. 188CPCh. 8 - Calculate the pH of a solution prepared by mixing...Ch. 8 - Consider the titration of 100.0mL of 0.10M...Ch. 8 - In the titration of 100.0mL of a 0.0500M solution...Ch. 8 - Consider the titration curve in Exercise91 for the...Ch. 8 - Consider a solution prepared by mixing the...Ch. 8 - Prob. 194MP
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- Consider all acid-base indicators discussed in this chapter. Which of these indicators would be suitable for the titration of each of these? (a) NaOH with HClO4 (b) acetic acid with KOH (c) NH3 solution with HBr (d) KOH with HNO3 Explain your choices.arrow_forwardDoes the pH of the solution increase, decrease, or stay the same when you (a) Add solid sodium oxalate, Na2C2O4, to 50.0 mL of 0.015-M oxalic acid? (b) Add solid ammonium chloride to 100. mL of 0.016-M HCl? (c) Add 20.0 g NaCl to 1.0 L of 0.012-M sodium acetate, NaCH3COO?arrow_forwardWhat is the pH of a solution that consists of 0.20 M ammonia, NH3, and 0.20 M ammonium chloride, NH4Cl?arrow_forward
- Phenol, C6H5OH, is a weak organic acid. Suppose 0.515 g of the compound is dissolved in enough water to make 125 mL of solution. The resulting solution is titrated with 0.123 M NaOH. C6H5OH(aq) + OH(aq) C6H5O(aq) + H2O() (a) What is the pH of the original solution of phenol? (b) What are the concentrations of all of the following ions at the equivalence point: Na+, H3O+, OH, and C6H5O? (c) What is the pH of the solution at the equivalence point?arrow_forwardMalic acid is a weak diprotic organic acid with Ka1 = 4.0 104 and Ka2 = 9.0 105. a Letting the symbol H2A represent malic acid, write the chemical equations that represent Ka1 and Ka2. Write the chemical equation that represents Ka1 Ka2. b Qualitatively describe the relative concentrations of H2A, HA, A2, and H3O+ in a solution that is about one molar in malic acid. c Calculate the pH of a 0.0175 M malic acid solution and the equilibrium concentration of [H2A]. d What is the A2 concentrationin in solutions b and c?arrow_forwardA solution made up of 1.0 M NH3 and 0.50 M (NH4)2SO4 has a pH of 9.26. a Write the net ionic equation that represents the reaction of this solution with a strong acid. b Write the net ionic equation that represents the reaction of this solution with a strong base. c To 100. mL of this solution, 10.0 mL of 1.00 M HCl is added. How many moles of NH3 and NH4+ are present in the reaction system before and after the addition of the HCl? What is the pH of the resulting solution? d Why did the pH change only slightly upon the addition of HCl?arrow_forward
- Which of the acid-base indicators discussed in this chapter would be suitable for the titration of (a) HNO3 with KOH. (b) KOH with acetic acid. (c) HCl with NH3. (d) KOH with HNO2. Explain your answers.arrow_forwardThe simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid. CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. (a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. (b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)arrow_forwardWrite an equation for each of the following buffering actions. a. the response of a HPO42/PO43 buffer to the addition of OH ions b. the response of a HF/F buffer to the addition of OH ions c. the response of a HCN/CN buffer to the addition of H3O+ ions d. the response of a H3PO4/H2PO4 buffer to the addition of H3O+ ionsarrow_forward
- Given the acid-base indicators in Question 37, select a suitable indicator for the following titrations. (a) sodium formate (NaCHO2) with HNO3 (b) hypochlorous acid with barium hydroxide (c) nitric acid with HI (d) hydrochloric acid with ammoniaarrow_forwardFor conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)arrow_forwardIdentify the buffer system(s)the conjugate acidbase pair(s)present in a solution that contains equal molar amounts of the following: a. HF, KC2H3O2, NaC2H3O2, and NaF b. HNO3, NaOH, H3PO4, and NaH2PO4arrow_forward
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Acid-Base Titration | Acids, Bases & Alkalis | Chemistry | FuseSchool; Author: FuseSchool - Global Education;https://www.youtube.com/watch?v=yFqx6_Y6c2M;License: Standard YouTube License, CC-BY