Chemistry with Access Code, Hybrid Edition
9th Edition
ISBN: 9781285188492
Author: Steven S. Zumdahl
Publisher: CENGAGE L
expand_more
expand_more
format_list_bulleted
Question
Chapter 16, Problem 7RQ
Interpretation Introduction
Interpretation: The figure showing the separation of common cations by selective precipitation is given. The chemistry involved with each step in Figure
Concept introduction: The qualitative analysis for the detection of cations present in a mixture involves the categorization of common cations into five groups and then these groups are further treated for the separation of cations present in the mixture and for their identification.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Solid iron II hydroxide, Fe(OH)2, has a solubility product constant of Ksp = 4.87 x 10-17. What is
%3D
[OH-] in a saturated solution?
Show your work to be eligible for partial credit. If you have calculator issues, just write down what
you intend to plug-in and explain what you would do with the resulting numbers. Please do not
leave this problem blank - write down anything you think is relevant.
Edit
View
Insert
Format
Tools Table
12pt v
Paragraph v B IU
4.87x10^-17
3.65x10^-6
Ph 8.66
pOH 5.44 basic
6-39. An acidic solution containing 0.010 M Lat is treated with NaOH until La(OH),
precipitates. At what pH does this occur?
The solubility-product constants, Kp, at 25 °C for two
compounds [iron(II) carbonate, FeCO3, and cadmium(II)
carbonate, CdCO3] are given by the table
Substance
Кар
FeCO3 2.10 x 10-11
CdCO3 1.80 x 10-14
Part A
A solution of Na2CO3 is added dropwise to a solution that contains 1.03x10-2 M Fe2+ and 1.52x10-2 MCd2+. What concentration of CO² is need to
initiate precipitation? Neglect any volume changes during the addition.
Express your answer with the appropriate units.
▸ View Available Hint(s)
[CO32] = Value
Units
Submit
Part B Complete previous part(s)
Part C Complete previous part(s)
Provide Feedback
?
Next >
Chapter 16 Solutions
Chemistry with Access Code, Hybrid Edition
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 - 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. 11QCh. 16 - Prob. 12QCh. 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 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. 21ECh. 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 Mg (OH)2, Ksp =...Ch. 16 - Prob. 32ECh. 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. 43ECh. 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 - Prob. 52ECh. 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. 56ECh. 16 - A solution contains 1.0 105 M Na3PO4. What is the...Ch. 16 - The Ksp of Al(OH)3 is 2 1032. At what pH will a...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. 65ECh. 16 - Prob. 66ECh. 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. 74ECh. 16 - Prob. 75ECh. 16 - The solubility of copper(II) hydroxide in water...Ch. 16 - A solution contains 0.018 mole each of I, Br, and...Ch. 16 - You have two salts, AgX and AgY, with very similar...Ch. 16 - Tooth enamel is composed of the mineral...Ch. 16 - The U.S. Public Health Service recommends the...Ch. 16 - Prob. 81AECh. 16 - Calculate the mass of manganese hydroxide present...Ch. 16 - Prob. 83AECh. 16 - The active ingredient of Pepto-Bismol is the...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 - The solubility rules outlined in Chapter 4 say...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. 99CPCh. 16 - Prob. 100CPCh. 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 - A solution saturated with a salt of the type M3X2...Ch. 16 - Consider 1.0 L of an aqueous solution that...Ch. 16 - The Ksp for Q, a slightly soluble ionic compound...Ch. 16 - Aluminium ions react with the hydroxide ion to...
Knowledge Booster
Similar questions
- The 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) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mLarrow_forwardThe Ksp of AgBr is 7.7 x 10-13 . Calculate its solubility in grams per 100 mL.arrow_forwardJust b (i-ii)arrow_forward
- pH The following plot shows the pH curves for the titrations of various acids by 0.10 M NaOH (all of the acids were 50.0-mL samples of 0.10 M concentration). Which pH curve corresponds to an acid with Ka 1 x 10-6 12.0 10.0 8.0 6.0 4.0 2.0 e с b a 0 10 20 30 40 50 60 Vol 0.10 M NaOH added (mL) |arrow_forwardThe solubility-product constants, Ksp, at 25 °C for two compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate, CdCO3] are given by the table Substance Ksp FeCO3 2.10 x 10-11 CdCO3 1.80 × 10-14 Part A A solution of Na2CO3 is added dropwise to a solution that contains 1.02x10-2 MFe²+ and 1.48x10-2 M Cd²+. What concentration of CO3²- is need to initiate precipitation? Neglect any volume changes during the addition. Express your answer with the appropriate units. ► View Available Hint(s) [CO3²- ] = Submit μA Value Part B Complete previous part(s) Part C Complete previous part(s) Units ?arrow_forwardAn aqueous solution contains Cu+, Tl+, Hg+, and Ti+ with each ion at a concentration of 0.15M. Chloride ion is slowly added to the solution. Using the Ksp information below, determine the order in which the ions would precipitate. AgCl = 1.8 x 10−10TiCl = 1.8 x 10−4PbCl2 = 1.7 x 10−5CuCl = 6.73 x 10−7TlCl = 3.7 x 10−4HgCl2 = 17.91 x 10−18arrow_forward
- Tue Apr 11 TA ... B HO + 1. Write the chemical reaction for the titration of the filtered KHT solution in pure water.arrow_forwardDetermine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your answer. 1 3 4 NEXT > Two solutions are mixed: 40.0 mL of 0.500 M NH3 and 25.0 mL of 0.300 M HCI. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. Before (mol) Change (mol) After (mol) -0.0075 Initial (M) Change (M) Equilibrium (M) E 0.313 - x 0 0.0100 0 0.500 + x 40.0 0.115 + x NH3(aq) -0.0100 NH3(aq) + 0.500 2 0.500 - x 0.115-x 0.500 2 0.0125 : on by constructing a BCA table, constructing an ICE table, ant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your answer. -■· 0.300 +arrow_forwardAccording to Demostration 6-1 in p. 133 of your textbook, when Q< Ksp, no precipitation is observed. Given that the Ksp of NaCl is 13.7, calculate the Q when 1/3 of a test tube of 6 M of HCI is added to an identical volume of saturated solution of NaCl. Assume that volumes are additive. The Q is 7 which is smaller than 13.7. [Just write answer in one significant figure]arrow_forward
- The concentration of Mg2+ in seawater is 0.053 M. At what pH will 99% of the Mg2+ be precipitated as the hydroxide salt? (Ksp for Mg(OH)2 = 8.9 ✕ 10−12. Assume that all solutions are at 25°C.) I have tried solving for the pOH and then subtracting that from 14 to find the pH, but it is wrong everytime. I don't understand where I'm going wrong.arrow_forwardCan you please set up the ice tablearrow_forward5mL of 0.150 M ammonia (NH3) is titrated with 0.100 M hydrochloric acid (HCl) The Kb for ammonia is 1.75 x 10-5 1)Write a balanced chemical equation for the reaction of ammonia and hydrochloric acid and a balanced chemical equation for the equilibrium of ammonia in water. 2) What is the pH of the ammonia solution prior to the addition of any HCl?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 Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author: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:OpenStax
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
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