What solid forms during the reaction of silver nitrate with sodium chloride? Solubility Rules Compounds of these ions tend to be soluble Alkali metals Ammonium Nitrate Acetate Chloride, Bromide lodide Sulfate Compounds of these ions tend to be insoluble Carbonate Chromate Phosphate Exceptions Pb2+, Hg₂2+, Ag+ Hg2+, Pb2+, Hg22+, Ag+ Ca2+, Sr2+, Ba2+, Pb2+, and Hg₂2+ Exceptions Alkali metal and ammonium Alkali metal and ammonium Alkali metal and ammonium

What solid forms during the reaction of silver nitrate with sodium chloride? Solubility Rules Compounds of these ions tend to be soluble Alkali metals Ammonium Nitrate Acetate Chloride, Bromide lodide Sulfate Compounds of these ions tend to be insoluble Carbonate Chromate Phosphate Exceptions Pb2+, Hg₂2+, Ag+ Hg2+, Pb2+, Hg22+, Ag+ Ca2+, Sr2+, Ba2+, Pb2+, and Hg₂2+ Exceptions Alkali metal and ammonium Alkali metal and ammonium Alkali metal and ammonium

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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QUESTION 9 TABLE 4.1 Solubility Guidelines for Common Ionic Compounds in Water Soluble Ionic Compounds Important Exceptions Compounds containing NO3 C2H3O2 None None 2+ Compounds of Ag*, Hg,² Compounds of Ag*, Hg2²+, and Pb2+ Compounds of Ag*, Hg2²+, and Pb²+ Compounds of Sr2+, Ba²+, and Pb²+ Br I 2+ SO,2- Hg2 and Pb2+ Insoluble Ionic Compounds Important Exceptions Compounds of NH4*, the alkali metal cations, and Ca2+, Sr²+, and Ba²+ Compounds of NH4* and the alkali metal Compounds containing s2- CO,?- cations PO,3– Compounds of NH,* and the alkali metal
The addition of 0.351 L of 1.25 M KCl to a solution containing Ag+ and Pb2+ ions is just enough to precipitate all of the ions as AgCl and PbCl2. The total mass of the resulting precipitate is 61.60 g. Find the mass of PbCl2 and AgCl in the precipitate. mass of PbCl2 ________g mass of AgCl: ____________g *someone answered already as 41.96 and 19.63 and that was wrong. I really need help.
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Can i know the solution for this? It's answer is 99.0 mL
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In the reaction between lead (II) iodide and potassium nitride to yield lead (II) nitride and potassium iodide, the coefficient in front of the potassium iodide is __________. 3 5 6 2 4
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As an undergraduate we used a lot of silver nitrate solutions in analytical chemistry lab to analyze solutions. Silver nitrate is a soluble silver salt. Silver halides (silver chloride, silver iodide, silver bromide) are not soluble in water. One week our deionized water machine was broken and we had to buy distilled water from a local grocery store. When we went to make our silver nitrate solutions for our analysis, the solutions immediately turned a milky white. Our instructor was irate. Using your knowledge of precipitation chemistry and the scenario I have laid out before you, does the instructor have a legitimate complaint against the retailer? Why or why not?