Chemical Principles
8th Edition
ISBN: 9781305581982
Author: Steven S. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Textbook Question
Chapter 4, Problem 40E
How would you separate the following ions in aqueoussolution by selective precipitation?
a.
b.
c.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
Consider the titration 40mL of 0.10M NaI with 0.05M Ag+. What is the major species present in the solution when 10mL of Ag+ has been reached?
a. Ag+
b. I-
c. AgI(s)
d. AgI(aq)
Calculate the equilibrium constant Kc for the net reaction shown below.
AgCl (s) ⇌ Ag+ (aq) + Cl− (aq) Ksp = 1.6 x 10-10
Ag+ (aq) + 2 NH3 (aq) ⇌ Ag(NH3)2+ (aq) Kf = 1.5 x 107
AgCl (s) + 2 NH3 (aq) ⇌ Ag(NH3)2+ (aq) + Cl− (aq) Kc = ?
Using net reaction, determine the molar solubility of silver iodide in 1.0 M NH3.
A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The H3O+ concentration after the addition of 10.0 mL of KOH is ________ M.
A 0.430
B 0.273
C 0.0181
D 0.439
E none of the above
Chapter 4 Solutions
Chemical Principles
Ch. 4 - Prob. 1DQCh. 4 - Prob. 2DQCh. 4 - Prob. 3DQCh. 4 - Prob. 4DQCh. 4 - Prob. 5DQCh. 4 - The exposed electrodes of a light bulb are placed...Ch. 4 - Prob. 7DQCh. 4 - Prob. 8DQCh. 4 - Consider separate aqueous solutions of HCland...Ch. 4 - Prob. 10DQ
Ch. 4 - Prob. 11DQCh. 4 - Characterize strong electrolytes versus weak...Ch. 4 - The figures below are molecular-level...Ch. 4 - Prob. 14ECh. 4 - Differentiate between what happens when the...Ch. 4 - Commercial cold packs and hot packs are available...Ch. 4 - Prob. 17ECh. 4 - Prob. 18ECh. 4 - Prob. 19ECh. 4 - Prob. 20ECh. 4 - Prob. 21ECh. 4 - Prob. 22ECh. 4 - Prob. 23ECh. 4 - Prob. 24ECh. 4 - Prob. 25ECh. 4 - Prob. 26ECh. 4 - Prob. 27ECh. 4 - Prob. 28ECh. 4 - Prob. 29ECh. 4 - A stock solution containing Mn2+ ions is prepared...Ch. 4 - Prob. 31ECh. 4 - Prob. 32ECh. 4 - List the formulas of three soluble bromide salts...Ch. 4 - Prob. 34ECh. 4 - Prob. 35ECh. 4 - Prob. 36ECh. 4 - Prob. 37ECh. 4 - Prob. 38ECh. 4 - Write the balanced molecular, complete, and net...Ch. 4 - How would you separate the following ions in...Ch. 4 - Prob. 41ECh. 4 - Prob. 42ECh. 4 - Prob. 43ECh. 4 - What volume of 0.100 M Na3PO4 is required to...Ch. 4 - Prob. 45ECh. 4 - Prob. 46ECh. 4 - Prob. 47ECh. 4 - The following drawings represent aqueous...Ch. 4 - Prob. 49ECh. 4 - Prob. 50ECh. 4 - Prob. 51ECh. 4 - Prob. 52ECh. 4 - Saccharin (C7H5NO3S) is sometimes dispensed in...Ch. 4 - Prob. 54ECh. 4 - A 1.42-g sample of a pure compound with formula...Ch. 4 - Prob. 56ECh. 4 - Prob. 57ECh. 4 - Prob. 58ECh. 4 - Prob. 59ECh. 4 - Prob. 60ECh. 4 - Prob. 61ECh. 4 - Prob. 62ECh. 4 - Prob. 63ECh. 4 - Sodium hydroxide solution is usually standardized...Ch. 4 - Prob. 65ECh. 4 - Prob. 66ECh. 4 - Prob. 67ECh. 4 - A student titrates an unknown amount of...Ch. 4 - Prob. 69ECh. 4 - Prob. 70ECh. 4 - Hydrochloric acid (75.0 mL of 0.250 M) is added...Ch. 4 - Prob. 72ECh. 4 - Prob. 73ECh. 4 - Prob. 74ECh. 4 - Prob. 75ECh. 4 - Prob. 76ECh. 4 - Prob. 77ECh. 4 - Prob. 78ECh. 4 - Prob. 79ECh. 4 - Balance each of the following oxidationreduction...Ch. 4 - Prob. 81ECh. 4 - Prob. 82ECh. 4 - Prob. 83ECh. 4 - Prob. 84ECh. 4 - Prob. 85ECh. 4 - Prob. 86ECh. 4 - Prob. 87ECh. 4 - Prob. 88ECh. 4 - Prob. 89ECh. 4 - Prob. 90ECh. 4 - Prob. 91AECh. 4 - Prob. 92AECh. 4 - Consider a 1.50-g mixture of magnesium nitrate...Ch. 4 - Suppose 50.0 mL of 0.250 M CoCl2 solution is added...Ch. 4 - Prob. 95AECh. 4 - A mixture contains only NaCland Fe(NO3)3 . A...Ch. 4 - A mixture contains only sodium chloride and...Ch. 4 - Prob. 98AECh. 4 - A student added 50.0 mL of an NaOH solution...Ch. 4 - In a 1-L beaker, 203 mL of 0.307 M ammonium...Ch. 4 - It took 25.060.05 mL of a sodium hydroxide...Ch. 4 - You wish to prepare 1 L of a 0.02 M potassium...Ch. 4 - Citric acid, which can be obtained from lemon...Ch. 4 - Acetylsalicylic acid is the active ingredient in...Ch. 4 - A 6.50-g sample of a diprotic acid requires 137.5...Ch. 4 - Prob. 106AECh. 4 - Chlorisondamine chloride (C14H20Cl6N2) is a drug...Ch. 4 - Calculate the concentration of all ions present...Ch. 4 - A solution is prepared by dissolving 0.6706 g...Ch. 4 - For the following chemical reactions, determine...Ch. 4 - What volume of 0.100 M NaOH is required to...Ch. 4 - Prob. 112AECh. 4 - A 450.0-mL sample of a 0.257-M solution of silver...Ch. 4 - Prob. 114AECh. 4 - A 50.00-mL sample of aqueous Ca(OH)2 requires34.66...Ch. 4 - When organic compounds containing sulfur are...Ch. 4 - Assign the oxidation state for the element listed...Ch. 4 - The blood alcohol (C2H5OH) level can be determined...Ch. 4 - Zinc and magnesium metal each react with...Ch. 4 - A 10.00-g sample consisting of a mixture of...Ch. 4 - Consider the reaction of 19.0 g of zinc with...Ch. 4 - Consider an experiment in which two burets, Y and...Ch. 4 - A sample is a mixture of KCl and KBr. When 0.1024...Ch. 4 - You made 100.0 mL of a lead(II) nitrate solution...Ch. 4 - Polychlorinated biphenyls (PCBs) have been used...Ch. 4 - Prob. 126CPCh. 4 - Prob. 127CPCh. 4 - Chromium has been investigated as a coating for...Ch. 4 - Prob. 129CPCh. 4 - Three students were asked to find the identity of...Ch. 4 - A sample is a mixture of AgNO3,CuCl2,andFeCl3...Ch. 4 - Prob. 132MPCh. 4 - You have two 500.0-mL aqueous solutions. Solution...
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
- Potassium hydrogen phthalate, known as KHP (molar mass = 204.22 g/mol), can be obtained in high purity and is used to determine the concentration of solutions of strong bases by the reaction HP(aq)+OH(aq)H2O(l)+P2(aq) If a typical titration experiment begins with approximately 0.5 g KHP and has a final volume of about 100 mL, what is an appropriate indicator to use? The pKa for HP is 5.51.arrow_forwardConsider 0.0010-M solutions of these sparingly soluble solutes in equilibrium with their ions. Predict the effect on each equilibrium if a saturated solution of sodium iodide were added. Explain your prediction in each case. AgI(s) ⇌ Ag+(aq) + I−(aq) PbI2(s) ⇌ Pb2+(aq) + 2 I−(aq)arrow_forwardA buffer solution is composed of 1.360 g of KH2PO4 and 5.677 g of Na2HPO4. (a) What is the pH of the buffer solution? (b) What mass of KH2PO4 must be added to decrease the buffer solution pH by 0.50 unit from the value calculated in part (a)?arrow_forward
- What is the equilibrium constant for the following reaction? AgCl(s)+I(aq)AgI(s)+Cl(aq) Does the equilibrium lie predominantly to the left or to the right? Will AgI form if iodide ion. I, is added to a saturated solution of AgCl?arrow_forwardCalculate the Ni2+ concentration of the standard solution if 3.0 mL of 0.20 M NiSO4 is added to 7.0 mL of H2O.arrow_forwardA basic solution contains the iodide and phosphate ions that are to be separated via selective precipitation.The I– concentration, which is 7.60×10-5 M, is 10,000 times less than that of the PO43– ion at 0.760 M.A solution containing the silver(I) ion is slowly added. Answer the questions below. Calculate the minimum Ag+ concentration required to cause precipitation of AgI. mol/L Calculate the minimum Ag+ concentration required to cause precipitation of Ag3PO4. mol/Larrow_forward
- a solution is prepared by mixing 5.00ml of 0.00200-M KSCN, 6.00 mL of 0.200-M Fe(NO3)3, and 14.00 mL of 0.050M HNO3 . Calculate the initial concentration of SCN- ions and Fe^3+ ions after mixing but before any reaction has occurred.arrow_forward25. Consider a system that includes both the Al(OH)3(s) (Ksp = 3 x 10-34) and the complex ion [Al(OH)4]- (Kf = 3 x 1033). What would be the effect of decreasing the pH of the solution? A. The mass of Al(OH)3 would increase. B. The concentration of [Al(OH)4]-would increase. C. The concentration of [OH-] (aq) would increase. D. Adjusting the pH would not impact the concentration of any of the species in solution. The answer is A, but can youp lease help explain why this is true? Thanks!arrow_forwardThe titration of a 20.0 mL sample of an H2SO4 solution of unknown concentration requires 22.92 mL of a 0.160 M KOH solution to reach the equivalence point. What is the concentration of the unknown H2SO4 solution? Express your answer to three significant figures.arrow_forward
- A solution of 0.0490 M HCl is used to titrate 29.0 mL of an ammonia solution of unknown concentration. The equivalence point is reached when 16.0 mL HCl solution have been added. (Assume KW = 1.01 e−14.) What was the original pH of the ammonia solution?arrow_forwardBegin by making a titration curve for the precipitation titration of 30.00 mL of 0.070 M SCN- using 0.10 M Ag+ solution. The titration curve is a plot of pAg+ vs volume of Ag+ solution added. What controls the concentration of Ag+ in the solution for the various regions of the titration curve?arrow_forwardSilver cyanide (AgCN) is an insoluble sail with Ksp = 2.2 1012. Compare the effects on the solubility of silver cyanide by addition of HNO3(aq) or by addition of NH3(aq).arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Acid-Base Equilibrium; Author: Bozeman Science;https://www.youtube.com/watch?v=l5fk7HPmo5g;License: Standard YouTube License, CC-BY
Introduction to Titrimetric analysis; Author: Vidya-mitra;https://www.youtube.com/watch?v=uykGVfn9q24;License: Standard Youtube License