In this experiment, you will be given a number of tests that you can perform and you will need to figure out which test is useful for the determining the presence of which ion. An example is provided below. One test that can be used to determine some ions is to add a solution of Pb(NO3)2 (aq) to an aqueous solution of your unknown. In this example, Pb(NO3)2 (aq) is added to 4 different solutions and the following results are recorded:When Pb(NO3)2 (aq) is added to an aqueous solution of NaCl, a yellow precipitate forms immediately.When Pb(NO3)2 (aq) is added to an aqueous solution of NaNO3, no change is observed. When Pb(NO3)2 (aq) is added to an aqueous solution of KCl, a yellow precipitate forms immediately.When Pb(NO3)2 (aq) is added to an aqueous solution of KNO3, no change occurs. Based on these results, select all of the following that are consistent with this data using the solubility table when necessary. Solubility Rules ExceptionsAll Group IA and ammonium compounds are soluble. --All Acetates and nitrates are soluble. --Most chlorides, bromides, and iodides are soluble.AgCl, Hg2Cl2, PbCl2, AgBr, HgBr2, Hg2Br2, PbBr2, AgI, HgI2,Hg2I2, PbI2Most sulfates are soluble.CaSO4, SrSO4, BaSO4, Ag2SO4, Hg2SO4, PbSO4Most carbonates are insoluble.Group IA carbonates, (NH4)2CO3Most phosphates are insoluble.Group IA phosphates, (NH4)2PO4Most sulfides are insoluble.Group IA sulfides, (NH4)2SMost hydroxides are insoluble.Group IA hydroxides, Ca(OH)2, Sr(OH)2, Ba(OH)2Group of answer choicesAddition of Pb(NO3)2 to a solution containing chloride ions will result in a precipitate.Addition of Pb(NO3)2 to a solution containing potassium ions will result in a precipitate.Addition of Pb(NO3)2 to a solution containing sodium ions will result in a precipitate.Addition of Pb(NO3)2 would be a good test for chloride ions.Addition of Pb(NO3)2 would be a good test for sodium ions.Addition of Pb(NO3)2 would be a good test for potassium ions.The net ionic equation that explains what is happening in this test is: NO3- (aq) + Na+(aq) --> NaNO3(s)The net ionic equation that explains what is happening in this test is: Pb2+(aq) + 2Na+(aq) --> PbNa(s)The net ionic equation that explains what is happening in this test is: Pb2+ (aq) + 2Cl-(aq) --> PbCl2(s)The net ionic equation that explains what is happening in this test is: Pb2+ (aq) +2 NO3-(aq) --> Pb(NO3)2(s)

Qualitative inorganic analysis is a method by which the different cations and anions present in a…

Answered: n this experiment, you will be given a…

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

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

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

Chapter7: Chemical Reactions: An Introduction

Section: Chapter Questions

Problem 10A

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In this experiment, you will be given a number of tests that you can perform and you will need to figure out which test is useful for the determining the presence of which ion. An example is provided below. One test that can be used to determine some ions is to add a solution of Pb(NO₃)₂ (aq) to an aqueous solution of your unknown.

In this example, Pb(NO₃)₂ (aq) is added to 4 different solutions and the following results are recorded:

When Pb(NO₃)₂ (aq) is added to an aqueous solution of NaCl, a yellow precipitate forms immediately.
When Pb(NO₃)₂ (aq) is added to an aqueous solution of NaNO₃, no change is observed.
When Pb(NO₃)₂ (aq) is added to an aqueous solution of KCl, a yellow precipitate forms immediately.
When Pb(NO₃)₂ (aq) is added to an aqueous solution of KNO₃, no change occurs.

Based on these results, select all of the following that are consistent with this data using the solubility table when necessary.

Solubility Rules	Exceptions
All Group IA and ammonium compounds are soluble.	--
All Acetates and nitrates are soluble.	--
Most chlorides, bromides, and iodides are soluble.	AgCl, Hg₂Cl₂, PbCl₂, AgBr, HgBr₂, Hg₂Br₂, PbBr₂, AgI, HgI₂,Hg₂I₂, PbI₂
Most sulfates are soluble.	CaSO₄, SrSO₄, BaSO₄, Ag₂SO₄, Hg₂SO₄, PbSO₄
Most carbonates are insoluble.	Group IA carbonates, (NH₄)₂CO₃
Most phosphates are insoluble.	Group IA phosphates, (NH₄)₂PO₄
Most sulfides are insoluble.	Group IA sulfides, (NH₄)₂S
Most hydroxides are insoluble.	Group IA hydroxides, Ca(OH)₂, Sr(OH)₂, Ba(OH)₂

Group of answer choices

Addition of Pb(NO₃)₂ to a solution containing chloride ions will result in a precipitate.

Addition of Pb(NO₃)₂ to a solution containing potassium ions will result in a precipitate.

Addition of Pb(NO₃)₂ to a solution containing sodium ions will result in a precipitate.

Addition of Pb(NO₃)₂ would be a good test for chloride ions.

Addition of Pb(NO₃)₂ would be a good test for sodium ions.

Addition of Pb(NO₃)₂ would be a good test for potassium ions.

The net ionic equation that explains what is happening in this test is: NO₃^- (aq) + Na⁺(aq) --> NaNO₃(s)

The net ionic equation that explains what is happening in this test is: Pb²⁺(aq) + 2Na⁺(aq) --> PbNa(s)

The net ionic equation that explains what is happening in this test is: Pb²⁺ (aq) + 2Cl^-(aq) --> PbCl₂(s)

The net ionic equation that explains what is happening in this test is: Pb²⁺ (aq) +2 NO₃^-(aq) --> Pb(NO₃)₂(s)

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