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Stock Solutions AgNO,/NaCl AgNO,/ Nal AgNO,/ Na₂SO Pb(NO₂)₂/NaCl *Pb(NO₂)₂/Nal Pb(NO₂)₂/Na₂SO, Precip? Net Ionic Equation Yes Dissolves w/ heat? Ag+ Cl AgCl(s) No

Stock Solutions AgNO,/NaCl AgNO,/ Nal AgNO,/ Na₂SO Pb(NO₂)₂/NaCl *Pb(NO₂)₂/Nal Pb(NO₂)₂/Na₂SO, Precip? Net Ionic Equation Yes Dissolves w/ heat? Ag+ Cl AgCl(s) No

Chemistry
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...
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III Anion Precipitation Reactions All nitrate salts are soluble in water. The Cl- and I salts of the cations in this experiment are also soluble except for those of Ag+ and Pb2+. Thus if you mix the silver stock solution (AgNO,) and the chloride stock solution (NaCl), precipitation of AgCl(s) will occur. PbCl, and Pbl, differ from AgCl and AgI in that they are soluble in hot water. All sulfate salts of the cations studied here are soluble except PbSO which does not dissolve in hot water. PROCEDURE: Combine 1 mL portions of the following pairs of stock solutions, mix well, and note formation of precipitates. Heat each mixture containing a precipitate in boiling water, mix well, and note those precipitates which dissolve. Exception*: For the Pb(NO3)₂/Nal reaction, use 3 drops of each test solution and add 10 mL of H₂O. 1.0 Precip? Stock Solutions AgNO,/NaCl AgNO,/Nal AgNO,/ Na₂SO, Pb(NO₂)₂/NaCl *Pb(NO₂)₂/Nal Pb(NO₂)₂/Na₂SO, Yes Net Ionic Equation Ag+ + Cl → AgCl(s) Dissolves w/ heat? No
Transcribed Image Text:III Anion Precipitation Reactions All nitrate salts are soluble in water. The Cl- and I salts of the cations in this experiment are also soluble except for those of Ag+ and Pb2+. Thus if you mix the silver stock solution (AgNO,) and the chloride stock solution (NaCl), precipitation of AgCl(s) will occur. PbCl, and Pbl, differ from AgCl and AgI in that they are soluble in hot water. All sulfate salts of the cations studied here are soluble except PbSO which does not dissolve in hot water. PROCEDURE: Combine 1 mL portions of the following pairs of stock solutions, mix well, and note formation of precipitates. Heat each mixture containing a precipitate in boiling water, mix well, and note those precipitates which dissolve. Exception*: For the Pb(NO3)₂/Nal reaction, use 3 drops of each test solution and add 10 mL of H₂O. 1.0 Precip? Stock Solutions AgNO,/NaCl AgNO,/Nal AgNO,/ Na₂SO, Pb(NO₂)₂/NaCl *Pb(NO₂)₂/Nal Pb(NO₂)₂/Na₂SO, Yes Net Ionic Equation Ag+ + Cl → AgCl(s) Dissolves w/ heat? No
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