Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 16, Problem 19Q
You have two salts, AgX and AgY, both with very similar Ksp values. You know that the Ka for HX is much greater than the Ka for HY. Which salt is more soluble in acidic solution? Explain.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
The Ksp values for two sparingly soluble salts, MX and QX2, are both equal to 4.0 x 10-18. Which of these two salts are more soluble?
2.) The Ksp values for AgCl and Mg(OH)2 respectively are 1.0 x 10-10 and 1.2 x 10-11. Which of these sparingly soluble salts is actually more soluble?
3.) Calculate the solubility of AgCl in a 0.20 M AgNO3 solution. Does the solubility of this salt increase or decrease, compared to its solubility in pure water?
1. The concentration of an unknown weak acid solution is 0.20M, and the solution has a pH of 3.89. What is Ką for this weak acid?
The concentration of an unknown weak base solution is 0.35M, and the solution has a pH of 11.26. What is Kp for this weak base?
Write the balanced chemical equation associated with the formation constant, Kf , for each complex ion. Include phase symbols.
AgI_-(2):
−⇀↽−↽−−⇀
Hg(NH3)2+4:
−⇀↽−↽−−⇀
Chapter 16 Solutions
Chemistry
Ch. 16 - To what reaction does the solubility product...Ch. 16 - Under what circumstances can you compare the...Ch. 16 - What is a common ion and how does its presence...Ch. 16 - List some salts whose solubility increases as the...Ch. 16 - What is the difference between the ion product, Q,...Ch. 16 - Mixtures of metal ions in aqueous solution can...Ch. 16 - Prob. 7RQCh. 16 - What is a complex ion? The stepwise formation...Ch. 16 - When 5 M ammonia is added to a solution containing...Ch. 16 - Figure 15-3 outlines the classic scheme for...
Ch. 16 - Which of the following will affect the total...Ch. 16 - Prob. 2ALQCh. 16 - You are browsing through the Handbook of...Ch. 16 - A friend tells you: The constant Ksp of a salt is...Ch. 16 - Explain the following phenomenon: You have a test...Ch. 16 - What happens to the Ksp value of a solid as the...Ch. 16 - Which is more likely to dissolve in an acidic...Ch. 16 - Two different compounds have about the same molar...Ch. 16 - Sodium chloride is listed in the solubility rules...Ch. 16 - For which of the following is the Ksp value of the...Ch. 16 - Ag2S(s) has a larger molar solubility than CuS...Ch. 16 - Solubility is an equilibrium position, whereas Ksp...Ch. 16 - Prob. 13QCh. 16 - Prob. 14QCh. 16 - The common ion effect for ionic solids (salts) is...Ch. 16 - Sulfide precipitates are generally grouped as...Ch. 16 - List some ways one can increase the solubility of...Ch. 16 - The solubility of PbCl2 increases with an increase...Ch. 16 - You have two salts, AgX and AgY, both with very...Ch. 16 - The stepwise formation constants for a complex ion...Ch. 16 - Silver chloride dissolves readily in 2 M NH3 but...Ch. 16 - If a solution contains either Pb2+(aq) or Ag+(aq),...Ch. 16 - Write balanced equations for the dissolution...Ch. 16 - Write balanced equations for the dissolution...Ch. 16 - Prob. 25ECh. 16 - Use the following data to calculate the Ksp value...Ch. 16 - Approximately 0.14 g nickel(II) hydroxide,...Ch. 16 - The solubility of the ionic compound M2X3, having...Ch. 16 - The concentration of Pb2+ in a solution saturated...Ch. 16 - The concentration of Ag+ in a solution saturated...Ch. 16 - Calculate the solubility of each of the following...Ch. 16 - Calculate the solubility of each of the following...Ch. 16 - Cream of tartar, a common ingredient in cooking,...Ch. 16 - Barium sulfate is a contrast agent for X-ray scans...Ch. 16 - Calculate the molar solubility of Cd(OH)2, Ksp =...Ch. 16 - The solubility rules outlined in Chapter 4 say...Ch. 16 - Calculate the molar solubility of Al(OH)3, Ksp = 2...Ch. 16 - Calculate the molar solubility of Co(OH)3, Ksp =...Ch. 16 - For each of the following pairs of solids,...Ch. 16 - For each of the following pairs of solids,...Ch. 16 - Calculate the solubility (in moles per liter) of...Ch. 16 - Calculate the solubility of Co(OH)2(s) (Ksp = 2.5 ...Ch. 16 - The Ksp for silver sulfate (Ag2SO4) is 1.2 105....Ch. 16 - The Ksp for lead iodide (PbI2) is 1.4 108....Ch. 16 - Calculate the solubility of solid Ca3(PO4)2 (Ksp =...Ch. 16 - Calculate the solubility of solid Pb3(P04)2 (Ksp =...Ch. 16 - Prob. 47ECh. 16 - The solubility of Pb(IO3)(s) in a 0.10-M KIO3...Ch. 16 - Which of the substances in Exercises 27 and 28...Ch. 16 - For which salt in each of the following groups...Ch. 16 - What mass of ZnS (Ksp = 2.5 1022) will dissolve...Ch. 16 - The concentration of Mg2+ in seawater is 0.052 M....Ch. 16 - Will a precipitate form when 100.0 mL of 4.0 104...Ch. 16 - A solution contains 1.0 105 M Ag+ and 2.0 106 M...Ch. 16 - A solution is prepared by mixing 100.0 mL of 1.0 ...Ch. 16 - If 10.0 mL of 2.0 103 M Cr(NO3)3 is added to 10.0...Ch. 16 - Calculate the final concentrations of K+(aq),...Ch. 16 - A solution is prepared by mixing 75.0 mL of 0.020...Ch. 16 - A 50.0-mL sample of 0.00200 M AgNO3 is added to...Ch. 16 - Prob. 60ECh. 16 - A solution contains 1.0 105 M Na3PO4. What is the...Ch. 16 - A solution is 1 104 M in NaF, Na2S, and Na3PO4....Ch. 16 - A solution contains 0.25 M Ni(NO3)2 and 0.25 M...Ch. 16 - Write equations for the stepwise formation of each...Ch. 16 - Write equations for the stepwise formation of each...Ch. 16 - In the presence of CN, Fe3+ forms the complex ion...Ch. 16 - In the presence of NH3, Cu2+ forms the complex ion...Ch. 16 - Prob. 69ECh. 16 - Prob. 70ECh. 16 - The overall formation constant for HgI42 is 1.0 ...Ch. 16 - A solution is prepared by adding 0.10 mole of...Ch. 16 - A solution is formed by mixing 50.0 mL of 10.0 M...Ch. 16 - A solution is prepared by mixing 100.0 mL of 1.0 ...Ch. 16 - a. Calculate the molar solubility of AgI in pure...Ch. 16 - Solutions of sodium thiosulfate are used to...Ch. 16 - Kf for the complex ion Ag(NH3)2+ is 1.7 107. Ksp...Ch. 16 - Prob. 78ECh. 16 - Prob. 79ECh. 16 - The solubility of copper(II) hydroxide in water...Ch. 16 - A solution contains 0.018 mole each of I, Br, and...Ch. 16 - Magnesium hydroxide, Mg(OH)2, is the active...Ch. 16 - Tooth enamel is composed of the mineral...Ch. 16 - The U.S. Public Health Service recommends the...Ch. 16 - What mass of Ca(NO3)2 must be added to 1.0 L of a...Ch. 16 - Calculate the mass of manganese hydroxide present...Ch. 16 - Prob. 87AECh. 16 - The active ingredient of Pepto-Bismol is the...Ch. 16 - Consider saturated solutions of die following...Ch. 16 - Silver cyanide (AgCN) is an insoluble sail with...Ch. 16 - Nanotechnology has become an important field, with...Ch. 16 - The equilibrium constant for the following...Ch. 16 - Calculate the concentration of Pb2+ in each of the...Ch. 16 - Will a precipitate of Cd(OH)2 form if 1.0 mL of...Ch. 16 - a. Using the Ksp value for Cu(OH)2 (1.6 1019) and...Ch. 16 - Describe how you could separate the ions in each...Ch. 16 - Nitrate salts are generally considered to be...Ch. 16 - In the chapter discussion of precipitate...Ch. 16 - Assuming that the solubility of Ca3(PO4)2(s) is...Ch. 16 - Order the following solids (ad) from least soluble...Ch. 16 - The Ksp for PbI2(s) 1.4 108. Calculate the...Ch. 16 - The solubility of Pb(IO3)2(s) in a 7.2 102-M KIO3...Ch. 16 - A 50.0-mL sample of 0.0413 M AgNO3(aq) is added to...Ch. 16 - Prob. 105CPCh. 16 - Prob. 106CPCh. 16 - a. Calculate the molar solubility of AgBr in pure...Ch. 16 - Calculate the equilibrium concentrations of NH3,...Ch. 16 - Calculate the solubility of AgCN(s) (Ksp = 2.2 ...Ch. 16 - Calcium oxalate (CaC2O4) is relatively insoluble...Ch. 16 - The salt MX has a solubility of 3.17 108 mol/L in...Ch. 16 - Consider 1.0 L of an aqueous solution that...Ch. 16 - A solution saturated with a salt of the type M3X2...Ch. 16 - What mass of Ca(NO3O)2 must be added to 1.0 L of a...Ch. 16 - The Ksp for Q, a slightly soluble ionic compound...Ch. 16 - Aluminium ions react with the hydroxide ion to...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Write the balanced chemical equation associated with the formation constant, Kf, for each complex ion. Include phase symbols. Agl,: Hg(NH, );*: 1L 1Larrow_forwardPredict the products of each reaction, and whether the solution at equilibrium will be acidic, basic, or neutral. At equilibrium the solution is...? reaction acidic N,0,(s) + 3H,0(1) → 0 basic neutral O acidic co, (g) + H,0(1) basic neutral acidic Na, 0 (s) + H,0(1) - 0 basic neutralarrow_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_forward
- Without doing any calculations (just compare the correct Ksp values) complete the following statements: 1. magnesium fluoride is MORE soluble than A 2. magnesium fluoride is LESS soluble than B A. PbBr2 B. Ni(CN)2 C. COCO3 D. COSarrow_forwardClassify each statement as true or false. Statement a. AgCl with a Ksp of 1.6E-10 has a higher molar solubility than Ag2CrO4 with a Ksp of 2.0E-12. b. The solubility of AgCI(s) in water is higher than its solubility in 0.10M NaCI(ag). The Ksp of AgCl is 1.6E-10. c. In a galvanic cell made by connecting a Zn/Zn2+ half cell to a Au/Au3+ half cell, the cations in the salt bridge flow into the Au half cell. Zn2+ + 2e- Zn E° = -0.76V Au3++ 3e- → Au E° = 1.498V d. Consider a three-bulb system. Given six gaseous atoms, putting two atoms in each bulb has a lower entropy than distributing all six atoms in the middle bulb. |le. For the reaction O2(g) → 02(1) the reaction is spontaneous at low temperatures. > > >arrow_forward(this is a multiple choice question with an explanation portion) Which of the following compounds has the lowest solubility in water at 25°C? Explain. A. Zn(OH) 2 , K sp = 4.5 x 10 -17B. AgBr, K sp = 5.0 x 10 -13C. MnCO 3 , K sp = 8.8 x 10 -11D. PbSO 4 , K sp = 1.3 x 10 -8E. More information is needed.arrow_forward
- Scott prepares a solution which contains a large excess of iron and a small amount of thiocyanate. He notices a faint orange color appear in the solution once mixed. He repeats this process with a higher concentration of thiocyanate and notices a deepening of the orange color in the solution once mixed. Explain what has happened to the equilibrium in this case. Has the value of Keq changed? Explain.arrow_forwardA solution contains 0.04500.0450 M Ca2+ and 0.09500.0950 M Ag+. If solid Na3PO4 is added to this mixture, which of the phosphate species would precipitate out of solution first? -Ca3(PO4)2 -Ag3PO4 -Na3PO4 When the second cation just starts to precipitate, what percentage of the first cation remains in solution?arrow_forwardWhat is the equilibrium concentration of H2C2O4 in a 0.542 M oxalic acid, H2C2O4, solution? For oxalic acid, Ka1 = 6.1 x 10–2 and Ka2 = 5.1 x 10–5. a. 1.4 x 10–1 M b. 1.1 x 10–1 M c. 2.3 x 10–1 M d. 3.88 x 10–1 M e. 8.9 x 10–2 Marrow_forward
- What is the order of solubility of the Group Il cations (from 1= most soluble to 4 = least soluble)? Sr2+Ca2+Mg2+Ba2+arrow_forwardIn which of the following aqueous solutions would you expect AgF to have the lowest solubility? pure water 0.023 M NaF 0.030 M LiF 0.015 M KF 0.0075 M AgNO3arrow_forward0.20 moles of CuSO4 are added to 1L of NH3 1.20M solution. Calculate the concentration of Cu2+ in the equilibrium.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
The Bohr Model of the atom and Atomic Emission Spectra: Atomic Structure tutorial | Crash Chemistry; Author: Crash Chemistry Academy;https://www.youtube.com/watch?v=apuWi_Fbtys;License: Standard YouTube License, CC-BY