Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 17, Problem 115SCQ
Interpretation Introduction
Interpretation:
The reason for increased solubility of
Concept introduction: The solubility of insoluble salts containing anions (conjugate base of a weak acid) such as hydroxide, acetate, carbonate, phosphate, and sulfide is greater than the value calculated using
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Chapter 17 Solutions
Chemistry & Chemical Reactivity
Ch. 17.1 - You have a 0.30 M solution of formic acid (HCO2H)...Ch. 17.2 - What is the pH of a buffer solution composed of...Ch. 17.2 - Use the Henderson-Hasselbalch equation to...Ch. 17.2 - Using an acetic acid/sodium acetate buffer...Ch. 17.2 - Calculate the pH of 0.500 L of a buffer solution...Ch. 17.3 - The titration of 0.100 M acetic acid with 0.100 M...Ch. 17.3 - Calculate the pH after 75.0 mL of 0.100 M HO has...Ch. 17.4 - The barium ion concentration, [Ba2+], in a...Ch. 17.4 - Calculate the solubility of AgCN in moles per...Ch. 17.4 - Calculate the solubility of Ca(OH)2 in moles per...
Ch. 17.4 - Calculate the solubility of BaSO4 (a) in pure...Ch. 17.5 - Solid Pbl2 (Ksp = 9.8 109) is placed in a beaker...Ch. 17.5 - Prob. 17.13CYUCh. 17.5 - Prob. 17.14CYUCh. 17.6 - Silver nitrate (0.0050 mol) is added to 1.00 L of...Ch. 17.6 - Calculate the value of the equilibrium constant,...Ch. 17.6 - Prob. 1.1ACPCh. 17.6 - What is the minimum volume of 0.0071 M NaCN(aq)...Ch. 17.6 - Use the formation constant of [Au(CN)2] in...Ch. 17.6 - Silver undergoes similar reactions as those shown...Ch. 17.6 - Write a balanced chemical equation for the...Ch. 17.6 - Phosphate ions are abundant in cells, both as the...Ch. 17.6 - A typical total phosphate concentration in a cell,...Ch. 17 - Does the pH of the solution increase, decrease or...Ch. 17 - Does the pH of the solution increase, decrease, or...Ch. 17 - What is the pH of a solution that consists of 0.20...Ch. 17 - What is the pH of 0.15 M acetic acid to which 1.56...Ch. 17 - What is the pH of the solution that results from...Ch. 17 - What is the pH of the solution that results from...Ch. 17 - What is the pH of the buffer solution that...Ch. 17 - Lactic acid (CH3CHOHCO2H) is found in sour milk,...Ch. 17 - What mass of sodium acetate, NaCH3CO2, must he...Ch. 17 - What mass of ammonium chloride, NH4Cl, must be...Ch. 17 - Calculate the pH of a solution that has an acetic...Ch. 17 - Calculate the pH of a solution that has an...Ch. 17 - What must the ratio of acetic acid to acetate ion...Ch. 17 - What must the ratio of H2PO4 to HPO42 be to have a...Ch. 17 - A buffer is composed of formic acid and its...Ch. 17 - A buffer solution is composed of 1.360 g of KH2PO4...Ch. 17 - Which of the following combinations would be the...Ch. 17 - Which of the following combinations would be the...Ch. 17 - Describe how to prepare a buffer solution from...Ch. 17 - Describe how to prepare a buffer solution from NH3...Ch. 17 - Determine the volume (in mL) of 1.00 M NaOH that...Ch. 17 - Determine the volume (in mL) of 1.00 M HC1 that...Ch. 17 - A buffer solution was prepared by adding 4.95 g of...Ch. 17 - You dissolve 0.425 g of NaOH in 2.00 L of a buffer...Ch. 17 - A buffer solution is prepared by adding 0.125 mol...Ch. 17 - What is the pH change when 20.0 mL of 0.100 M NaOH...Ch. 17 - Phenol, C6H5OH, is a weak organic acid. Suppose...Ch. 17 - Assume you dissolve 0.235 g of the weak acid...Ch. 17 - You require 36.78 mL of 0.0105 M HCl to reach the...Ch. 17 - A titration of 25.0 mL of a solution of the weak...Ch. 17 - Without doing detailed calculations, sketch the...Ch. 17 - Without doing detailed calculations, sketch the...Ch. 17 - You titrate 25.0 mL of 0.10 M NH3 with 0.10 M HCl....Ch. 17 - Using Figure 17.11, suggest an indicator to use in...Ch. 17 - Using Figure 17.11, suggest an indicator to use in...Ch. 17 - Name two insoluble salts of each of the following...Ch. 17 - Prob. 38PSCh. 17 - Using the solubility guidelines (Figure 3.10),...Ch. 17 - Predict whether each of the fallowing is insoluble...Ch. 17 - For each of the following insoluble salts, (1)...Ch. 17 - Prob. 42PSCh. 17 - When 1.55 g of solid thallium(I) bromide is added...Ch. 17 - At 20 C, a saturated aqueous solution of silver...Ch. 17 - When 250 mg of SrF2, strontium fluoride, is added...Ch. 17 - Calcium hydroxide, Ca(OH)2, dissolves in water to...Ch. 17 - You add 0.979 g of Pb(OH)2 to 1.00 L of pure water...Ch. 17 - You place 1.234 g of solid Ca(OH)2 in 1.00 L of...Ch. 17 - Estimate the solubility of silver iodide in pure...Ch. 17 - What is the molar concentration of Au+(aq) in a...Ch. 17 - Prob. 51PSCh. 17 - Estimate the solubility of lead(II) bromide (a) in...Ch. 17 - The Ksp value for radium sulfate, RaSO4, is 4.2 ...Ch. 17 - If 55 mg of lead(II) sulfate is placed in 250 mL...Ch. 17 - Prob. 55PSCh. 17 - Prob. 56PSCh. 17 - Calculate the molar solubility of silver...Ch. 17 - Calculate the solubility of silver bromide, AgBr,...Ch. 17 - Compare the solubility, in milligrams per...Ch. 17 - What is the solubility, in milligrams per...Ch. 17 - Calculate the solubility, in moles per liter, of...Ch. 17 - Calculate the solubility, in moles per liter, of...Ch. 17 - Which insoluble compound in each pair should be...Ch. 17 - Which compound in each pair is more soluble in...Ch. 17 - You have a solution that has a lead(II) ion...Ch. 17 - Sodium carbonate is added to a solution in which...Ch. 17 - If the concentration of Zn2+ in 10.0 mL of water...Ch. 17 - You have 95 mL of a solution that has a lead(II)...Ch. 17 - Prob. 69PSCh. 17 - Will a precipitate of Mg(OH)2 form when 25.0 mL of...Ch. 17 - Zinc hydroxide is amphoteric (Section 16.10). Use...Ch. 17 - Solid silver iodide, AgI, can be dissolved by...Ch. 17 - What amount of ammonia (moles) must be added to...Ch. 17 - Can you dissolve 15.0 mg of AuCl in 100.0 mL of...Ch. 17 - What is the solubility of AgCl (a) in pure water...Ch. 17 - Prob. 76PSCh. 17 - Prob. 77GQCh. 17 - Prob. 78GQCh. 17 - Prob. 79GQCh. 17 - Calculate the hydronium ion concentration and the...Ch. 17 - Calculate the hydronium ion concentration and the...Ch. 17 - For each of the following cases, decide whether...Ch. 17 - Prob. 83GQCh. 17 - A sample of hard water contains about 2.0 103 M...Ch. 17 - What is the pH of a buffer solution prepared from...Ch. 17 - Prob. 86GQCh. 17 - Describe the effect on the pH of the following...Ch. 17 - What volume of 0.120 M NaOH must be added to 100....Ch. 17 - A buffer solution is prepared by dissolving 1.50 g...Ch. 17 - What volume of 0.200 M HCl must be added to 500.0...Ch. 17 - What is the equilibrium constant for the following...Ch. 17 - Calculate the equilibrium constant for the...Ch. 17 - Prob. 93GQCh. 17 - The solubility product constant for calcium...Ch. 17 - In principle, the ions Ba2+ and Ca2+ can be...Ch. 17 - A solution contains 0.10 M iodide ion, I, and 0.10...Ch. 17 - A solution contains Ca2+ and Pb2+ ions, both at a...Ch. 17 - Prob. 98GQCh. 17 - Prob. 99GQCh. 17 - Prob. 100GQCh. 17 - Each pair of ions below is found together in...Ch. 17 - Each pair of ions below is found together in...Ch. 17 - The cations Ba2+ and Sr2+ can be precipitated as...Ch. 17 - You will often work with salts of Fe3+, Pb2+, and...Ch. 17 - Aniline hydrochloride, (C6H5NH3)Cl, is a weak...Ch. 17 - The weak base ethanolamine. HOCH2CH2NH2, can be...Ch. 17 - For the titration of 50.0 mL of 0.150 M...Ch. 17 - A buffer solution with it pH of 12.00 consists of...Ch. 17 - To have a buffer with a pH of 2.50, what volume of...Ch. 17 - What mass of Na3PO4 must be added to 80.0 mL of...Ch. 17 - You have a solution that contains AgNO3, Pb(NO3)2,...Ch. 17 - Prob. 112ILCh. 17 - Suggest a method for separating a precipitate...Ch. 17 - Prob. 114SCQCh. 17 - Prob. 115SCQCh. 17 - Two acids, each approximately 0.01 M in...Ch. 17 - Composition diagrams, commonly known as alpha...Ch. 17 - The composition diagram, or alpha plot, for the...Ch. 17 - The chemical name for aspirin is acetylsalicylic...Ch. 17 - Prob. 120SCQ
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- The grid has six lettered boxes, each of which contains an item that may be used to answer the questions that follow. Items may be used more than once and there may be more than one correct item in response to a question. Place the letter(s) of the correct selection(s) on the appropriate line. Could dissolve Zn(OH)2 _____________ Could be used to prepare a buffer from __________ Halfway to the equivalence point in the titration of a weak, monoprotic acid with strong base ________ SO2-related atmospheric phenomenon __________ Species formed by a Lewis acid-base reaction ________ General condition required for precipitation to occur ________ [conj. base] = [conj. acid] in a buffer ___________arrow_forwardThe Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)arrow_forwardThe solubility of Ag3PO4 is measured and found to be 2.00×10-3 g/L. Use this information to calculate a Ksp value for silver phosphate.arrow_forward
- The concentration of Ag+ ion in a saturated solution of Ag2C2O4 is 2.3 x 10-4 mol/L. Calculate the solubility product Ksp for this salt.arrow_forwardWhich of the following is the expression for the solubility product of Fe2(CrO4)3? Ksp 2[Fe2+13 +3[CrO4³-1² O O Ksp=3[Fe2+]2[CrO4³-] OKsp=[2x Fe2+13[3 x CrO4³-12 Ksp [Fe2+]³[CrO43-1² Ksp=[Fe3+12[CrO4²-1³arrow_forwardGiven that Ksp for AgCl is 1.6E-10 and Kf for Ag(CN)2- is 5.6E8, calculate the concentration of Ag+ when 0.15 M AgNO3 is reacted with 0.25 M KCN.arrow_forward
- The solubility of Ag2SO4 is measured and found to be 4.94 g/L. Use this information to calculate a Ksp value for silver sulfate.arrow_forwardHow many grams of CaF2 (molar mass 78.077) will dissolve in 250 mL of 0.20 M NaF solution? The Ksp for CaF2 is 3.8904e-11.arrow_forwardA 0.2585 gram amount of H₂C₂O4 is dissolved in approximately 100 mL of 0.5 M H₂SO4. A KMnO4 solution is added to a burette and added to the H₂C₂O₂ solution. A faint colour persists when 22.35 mL of KMnO solution has been added. slowly Calculate the molarity of the KMnO4 solution. A) 0.2294 M B) 0.02235 C) 0.05139 M 0.02927 Marrow_forward
- What is the solubilty of PbF2 in water? the Ksp for PbF2 is 2.7 x 10^-8arrow_forward2. What is the solubility of aqueous Ag3PO4? What is the concentration of Ag+ ions in water saturated with Ag3PO4 (Ksp = 1.60 × 10-18)?arrow_forwardCalculate the solubility of CO2 gas under 3.68 atm partial pressure of CO2 if 0.179 g of CO2 dissolves in 100 mL of solution under 1.00 atm partial pressure.arrow_forward
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