3. Based on the solubility rules in your textbook (Section 8.4), decide if each of the following compounds is soluble (S), or insoluble (1): Compound Solubility Compound Solubility silver chloride calcium carbonate manganese (II) hydroxide potassium hydroxide calcium nitrate ammonium nitrate sodium carbonate potassium chloride nickel (II) sulfate aluminum hydroxide magnesium sulfide calcium sulfide

3. Based on the solubility rules in your textbook (Section 8.4), decide if each of the following compounds is soluble (S), or insoluble (1): Compound Solubility Compound Solubility silver chloride calcium carbonate manganese (II) hydroxide potassium hydroxide calcium nitrate ammonium nitrate sodium carbonate potassium chloride nickel (II) sulfate aluminum hydroxide magnesium sulfide calcium sulfide

Introductory Chemistry: A Foundation

8th Edition

ISBN:9781285199030

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter7: Reactions In Aqueous Solutions

Section: Chapter Questions

Problem 16QAP

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Relative solubilities of salts in liquid ammonia can differsignificantly from those in water. Thus, silver bromide issoluble in ammonia, but barium bromide is not (thereverse of the situation in water). Write a balanced equation for the reaction of anammonia solution of barium nitrate with an ammoniasolution of silver bromide. Silver nitrate is soluble inliquid ammonia. What volume of a 0.50 M solution of silver bromidewill react completely with 0.215 L of a 0.076 M solutionof barium nitrate in ammonia? What mass of barium bromide will precipitate fromthe reaction in part (b)?
Potassium acid phthalate, KNaC8H4O4, or KHP, is used in many laboratories, including general chemistry laboratories, to standardize solutions of base. KHP is one of only a few stable solid acids that can be dried by warming and weighed. A 0.3420-g sample of KNaC8H4O4 reacts with 35.73 mL of a NaOH solution in a titration. What is the molar concentration of the NaOH? KNaC8H4O4(aq)+NaOH(aq)KNaC8H4O4(aq)+H2O(aq)
There are many ionic compounds that dissolve in water to a very small extent. One example is lead(II) chloride. When it dissolves an equilibrium is established between the solid salt and its component ions. Suppose you stir some solid PbCl2 into water. Explain how you would prove that the compound dissolves but to a small extent? Is the dissolving process product-favored or reactant-favored? pbcl2(s)pb2+(aq)+2cl(aq)
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
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What mass of silver chloride can be prepared by the reaction of 100.0 mL of 0.20 M silver nitrate with 100.0 mL of 0.15 M calcium chloride? Calculate the concentrations of each ion remaining in solution after precipitation is complete.
Write the balanced net ionic equation for the reaction that takes place when aqueous solutions of the following solutes are mixed. If no reaction is likely, explain why no reaction would be expected for that combination of solutes. l type='a'> potassium nitrate and sodium chloride calcium nitrate and sulfuric acid ammonium sulfide and lead(II) nitrate sodium carbonate and iron(III) chloride mercurous nitrate and calcium chloride silver acetate and potassium chloride i>phosphoric acid and calcium nitrate sulfuric acid and nickel(II) sulfate
What is the solid that precipitates, and how much of it forms, when an excess of sodium chloride solution is mixed with 10.0 mL of a 2.10 M silver nitrate solution?
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