EBK CHEMICAL PRINCIPLES
8th Edition
ISBN: 9781305856745
Author: DECOSTE
Publisher: CENGAGE LEARNING - CONSIGNMENT
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Chapter 8, Problem 169AE
Assuming that the solubility of
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Chapter 8 Solutions
EBK 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 solubility of Mg(OH)2 in water is approximately 9.6 mg/L at a given temperature. Calculate the Ksp of magnesium hydroxide. Calculate the hydroxide concentration needed to precipitate Mg2+ ions such that no more than 5.0 μg Mg2+ per liter remains in the solution.arrow_forwardSufficient sodium cyanide, NaCN, was added to 0.015 M silver nitrate, AgNO3, to give a solution that was initially 0.108 M in cyanide ion, CN. What is the concentration of silver ion, Ag+, in this solution after Ag(CN)2 forms? The formation constant Kf for the complex ion Ag(CN)2 is 5.6 1018.arrow_forwardSolubility is an equilibrium position, whereas Ksp is an equilibrium constant. Explain the difference.arrow_forward
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