Which of the following anions will separate Ag* from Pb** by precipitating one of them, leaving the other insolution? (A)CATIONSHighSolubility(aq)LowSolubility(s)OOH™O crO C₂H30₂3-PO4³-Cl, Br, IHalidesSO4²-MostAg+, Pb²+,Tl+, Hg₂²+,Hg, CuSolubility Table$2.Group 1,Nhì,Group 2MostANIONSOHGroup 1,NH4*, Sr²⁰,Ba²+, Tl.MostSO4²-MostAg+, Pb²+,Ca²+, Ba²+,Sr², Ra²CO32, C₂H3O2 NO3PO4³-,SO3²-Group 1,NH4MostAll Group 1 compounds, including acids, and all ammonium compounds are assumed to have high solubility inwater.Most AllAg+None

According to the given solubility table, C2H3O2- anion has low solubility with Ag+ cation.

Which of the following anions will separate Ag* from Pb**by precipitating one of them, leaving the other in solution? (A) CATIONS O cr High Solubility (aq) Low Solubility (s) OH™ C₂H30₂ Cl, Br, I Halides O PO4³- O SO4²- 2- Most Ag+, Pb²+, Tl+, Hg₂²+, Hg, Cu 52- Solubility Table Group 1, NHỎ, Group 2 Most ANIONS OH Group 1, NH₂", Sr²", Ba2+, TL- Most SO4²- Most Ag+, Pb²+, Ca²+, Ba²+, Sr², Raz All Group 1 compounds, including acids, and all ammonium compounds are assumed to have high solubility in water. CO3², C₂H₂O₂ NO3 PO4³, SO3²- Group 1, Most All NH₂ Most Ag None

Which of the following anions will separate Ag* from Pb**by precipitating one of them, leaving the other in solution? (A) CATIONS O cr High Solubility (aq) Low Solubility (s) OH™ C₂H30₂ Cl, Br, I Halides O PO4³- O SO4²- 2- Most Ag+, Pb²+, Tl+, Hg₂²+, Hg, Cu 52- Solubility Table Group 1, NHỎ, Group 2 Most ANIONS OH Group 1, NH₂", Sr²", Ba2+, TL- Most SO4²- Most Ag+, Pb²+, Ca²+, Ba²+, Sr², Raz All Group 1 compounds, including acids, and all ammonium compounds are assumed to have high solubility in water. CO3², C₂H₂O₂ NO3 PO4³, SO3²- Group 1, Most All NH₂ Most Ag None

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What mass of precipitate will form if 1.50 L of highly concentrated Pb(ClO3)2 is mixed with 0.0850 L 0.240M NaI? Assume the reaction goes to completion.
In one experiment, an 80.0-mL sample of hydrocyanic cid (HCN) was titrated with 20.0 mL of triiodide (I3-) in the reaction: HCN (aq) + I3- (aq) --> ICN (aq) + 2 I- (aq) + H+ (aq) 40.0 mL of the same triiodide solution were required to titrate 0.200 mol of H3AsO3 (aq) in the reaction: H3AsO3 (aq) + I3- (aq) + H2O (l) --> H3AsO4 (aq) + 3 I- (aq) + 2H+ (aq) What is the molar concentration of HCN (aq)? (Answer in sig figs)
You have an aqueous solution of 0.01 M HNO2. What would you expect to happen if you dissolve solid KNO2 in the solution of HNO2? Be sure you canexplain your answer.
Consider an analyte solution of 50.0 mL of 0.050 M hydrochloric acid, HCl, titrated against 0.10 M sodium hydroxide, NaOH (d) After adding 12.50 mL of the NaOH, halfway to the equivalence point, what ions or molecules are present in the solution? (e) At the equivalence point, after adding 25.00 mL of NaOH, what ions or molecules are present in the solution? (f) Which of the species you identified in part (e) will determine the pH of the solution?
(Multi answers) Find soluble compounds using the solubility rules. TABLE 9.7 Solubility Rules for lonic Compounds in Water An ionic compound is soluble in water if it contains one of the following: Li, Na, K, Rb, Cs. NH₂* NO₂, C₂H₂O₂ CI, Br, I except when combined with Ag*, Pb, or Hg₂²+ SO except when combined with Ba, Pb, Ca, Sr, or Hg₂+ lonic compounds that do not contain at least one of these ions are usually insoluble. Positive lons Negative lons Select 5 correct answer(s) Question 8 options: KCI Na₂S CaSO4 BaSO4 AgNO3 KNO3 CuS AgCl RbBr
A solution contains 7.27x103 M lead nitrate and 1.16x102 M calcium acetate. Solid ammonium sulfate is added slowly to this mixture. What is the concentration of lead ion when calcium ion begins to precipitate? [Pb2*] =| M
What is the solid product when the following reagents ar mixed: AgNO3 (aq) + KCl (aq) --> * AgCl (s) * KNO3 (s) * AgK (s) * Everything would dissolve, no solid is formed
A chemist combines 53.9 mL of 0.372 M potassium bromide with 23.1 mL of 0.451 M silver nitrate. (a) How many grams of silver bromide will precipitate? (b) What is the final molarity of the K* ion? (c) What is the final molarity of the silver or bromide ion, whichever one is in excess? (а) g AgBr (b) M K* (c) Мехсess ion
There is a solution containing two metal cations. The goal is to separate them by slowly and carefully adding a solution of an anion, until one mental cation precipitates as a compound with that anion, leaving the other metal cation still in solution. M+ is Ag+, M2+ is Ca2+, anion is SO4 2-, first Ksp is 1.2 x 10-5, second Ksp is 6.1 x 10-5, and the starting concentrations of M+ is 1.50 x 10-2 M and M2+ is 3.50 x 10-2M. Using these values, predict which metal will precipitate first and what concentration of anion the precipitation will begin.
Many salts of Pb2+ are sparingly soluble, and the difference in their solubility can be used to separate anions from solution.A solution is 0.0151 M in both Br– and SO42–. A 0.257 M solution of lead(II) nitrate is slowly added to it with a buret.The (pick one: Br^- or SO_4^2-) anion will precipitate from the solution first.(Ksp for PbBr2 = 6.60 ×× 10–6; Ksp for PbSO4 = 2.53 ×× 10–8) What is the concentration in the solution of the first anion when the second one starts to precipitate at 25°C? ___ M
4.) Regarding the fırst preliminary test, what concentration of AGNO3 is required to just cause SO32 ions to precipitate? Assume the concentration of SO32 is 0.10 M. [AGNO3] = _х 107 м
How do you do part D of the question?