Chemical Principles
8th Edition
ISBN: 9781337247269
Author: Steven S. Zumdahl; Donald J. DeCoste
Publisher: Cengage Learning US
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Chapter 8, Problem 155AE
A
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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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- The titration of 0.100 M acetic acid with 0.100 M NaOH is described in the text. What is the pH of the solution when 35.0 mL of the base has been added to 100.0 mL of 0.100 M acetic acid?arrow_forwardConsider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?arrow_forwardFollow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105). Beaker B has HCI. The volume and molarity of each acid in the beakers are the same. Both acids are to be titrated with a 0.1 M solution of NaOH. (a) Before titration starts (at zero time), the pH of the solution in Beaker A is the pH of the solution in Beaker B. (b) At half-neutralization (halfway to the equivalence point), the pH of the solution in Beaker A the pH of the solution in Beaker B. (c) When each solution has reached its equivalence point, the pH of the solution in Beaker A the pH of the solution in Beaker B. (d) At the equivalence point, the volume of NaOH used to titrate HCI in Beaker B the volume of NaOH used to titrate the weak acid in Beaker A.arrow_forward
- Two samples of 1.00 M HCl of equivalent volumes are prepared. One sample is titrated to the equivalence point with a 1.00 M solution of sodium hydroxide, while the other sample is titrated to the equivalence point with a 1.00 M solution of calcium hydroxide. a Compare the volumes of sodium hydroxide and calcium hydroxide required to reach the equivalence point for each titration. b Determine the pH of each solution halfway to the equivalence point. c Determine the pH of each solution at the equivalence point.arrow_forwardThe three flasks shown below depict the titration of an aqueous NaOH solution with HCl at different points. One represents the titration prior to the equivalence point, another represents the titration at the equivalence point, and the other represents the titration past the equivalence point. (Sodium ions and solvent water molecules have been omitted for clarity.) a Write the balanced chemical equation for the titration. b Label each of the beakers shown to indicate which point in the titration they represent. c For each solution, indicate whether you expect it to be acidic, basic, or neutral.arrow_forwardA monoprotic organic acid that has a molar mass of 176.1 g/mol is synthesized. Unfortunately, the acid produced is not completely pure. In addition, it is not soluble in water. A chemist weighs a 1.8451-g sample of the impure acid and adds it to 100.0 mL of 0.1050 M NaOH. The acid is soluble in the NaOH solution and reacts to consume most of the NaOH. The amount of excess NaOH is determined by titration: It takes 3.28 mL of 0.0970 M HCl to neutralize the excess NaOH. What is the purity of the original acid, in percent?arrow_forward
- A 25.0-mL sample of hydroxylamine is titrated to the equivalence point with 35.8 mL of 0.150 M HCl. a What was the concentration of the original hydroxylamine solution? b What is the pH at the equivalence point? c Which indicators, bromphenol blue, methyl red, or phenolphthalein, should be used to detect the end point of the titration? Why?arrow_forwardA buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?arrow_forwardA 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where the total volume was 1.50 times the original volume. At what pH does the equivalence point occur?arrow_forward
- Calculate the pH of these buffers.arrow_forwardSketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.arrow_forwardA buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?arrow_forward
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