Potassium iodide reacts with lead(ll) nitrate in this precipitation reaction:
What minimum volume of 0.200 M potassium iodide solution is required to completely precipitate all of the lead in 155.0 mLof a 0.112 M lead(ll) nitrate solution?
- 43.4 mL
- 86.8 mL
- 174 mL
- 348 mL
Want to see the full answer?
Check out a sample textbook solutionChapter 8 Solutions
CHEM: STRUC & PROP (LL) VOL 2 >C PKG<
- A 25.0-mL sample of sodium sulfate solution was analyzed by adding an excess of barium chloride solution to produce barium sulfate crystals, which were filtered from the solution. Na2SO4(aq)+BaCl2(aq)2NaCl(aq)+BaSO4(s) If 5.719 g of barium sulfate was obtained, what was the molarity of the original Na2SO4 solution?arrow_forwardSeparate samples of a solution of an unknown soluble ionic compound are treated with KCl, Na2SO4, and NaOH. A precipitate forms only when Na2SO4 is added. Which cations could be present in the unknown soluble ionic compound?arrow_forwardA soluble iodide was dissolved in water. Then an excess of silver nitrate, AgNO3, was added to precipitate all of the iodide ion as silver iodide, AgI. If 1.545 g of the soluble iodide gave 2.185 g of silver iodide, how many grams of iodine are in the sample of soluble iodide? What is the mass percentage of iodine, I, in the compound?arrow_forward
- A 10.0-mL sample of potassium iodide solution was analyzed by adding an excess of silver nitrate solution to produce silver iodide crystals, which were filtered from the solution. KI(aq)+AgNO3(aq)KNO3(aq)+AgI(s) If 2.183 g of silver iodide was obtained, what was the molarity of the original KI solution?arrow_forwardBone was dissolved in hydrochloric acid, giving 50.0 mL of solution containing calcium chloride, CaCL2. To precipitate the calcium ion from the resulting solution, an excess of potassium oxalate was added. The precipitate of calcium oxalate, CaC2O4, weighed 1.437 g. What was the molarity of CaCl2 in the solution?arrow_forwardA 10.00-mL sample of a 24.00% solution of ammonium bromide (NH4Br) requires 23.41 mL of 1.200 molar silver nitrate (AgNO3) to react with all of the bromide ion present. (a) Calculate the molarity of the ammonium bromide solution. (b) Use the molarity of the solution to find the mass of ammonium bromide in 1.000 L of this solution. (c) From the percentage concentration and the answer to part b, find the mass of 1.000 L ammonium bromide solution. (d) Combine the answer to part c with the volume of 1.000 L to express the density of the ammonium bromide solution (in g/mL).arrow_forward
- When 10. L of water is added to 3.0 L of 6.0 M H2SO4, what is the molarity of the resulting solution? Assume the volumes are additive.arrow_forwardA 0.608-g sample of fertilizer contained nitrogen as ammonium sulfate, (NH4)2SO4. It was analyzed for nitrogen by heating with sodium hydroxide. (NH4)2SO4(s)+2NaOH(aq)Na2SO4(aq)+2H2O(l)+2NH3(g) The ammonia was collected in 46.3 mL of 0.213 M HCl (hydrochloric acid), with which it reacted. NH3(g)+HCl(aq)NH4Cl(aq) This solution was titrated for excess hydrochloric acid with 44.3 mL of 0.128 M NaOH. NaOH(aq)+HCl(aq)NaCl(aq)+H2O(l) What is the percentage of nitrogen in the fertilizer?arrow_forwardA 300.0-g sample of a solid is made up of a uniform mixture of NaNO3, MgCl2, and BaCl2. A 100.0-g sample of the mixture is dissolved in water and treated with an excess of KOH. The precipitate from the reaction has a mass of 13.47 g. The remaining 200.0-g sample is also dissolved in water and treated with an aqueous solution of AgNO3. The resulting precipitate has a mass of 195.8 g. What are the masses of NaNO3, MgCl2, and BaCl2 in the 300.0-g sample?arrow_forward
- Arsenic acid, H3AsO4, is a poisonous acid that has been used in the treatment of wood to prevent insect damage. Arsenic acid has three acidic protons. Say you take a 25.00-mL sample of arsenic acid and prepare it for titration with NaOH by adding 25.00 mL of water. The complete neutralization of this solution requires the addition of 53.07 mL of 0.6441 M NaOH solution. Write the balanced chemical reaction for the titration, and calculate the molarity of the arsenic acid sample.arrow_forwardSodium chloride is used in intravenous solutions for medical applications. The NaCl concentration in such solutions must be accurately known and can be assessed by reacting the solution with an experimentally determined volume of AgNO3 solution of known concentration. The net ionic equation is Ag+(aq)+Cl(aq)AgCl(s) Suppose that a chemical technician uses 19.3 mL of 0.200-M AgNO3 to convert all the NaCl in a 25.0-mL sample of an intravenous solution to AgCl. Calculate the molarity of NaCl in the solution.arrow_forwardA 8.50 g sample of KCl is dissolved in 66.0 mL of water. The resulting solution is then added to 72.0 mL of a 0.280 M CaCl2(aq) solution. Assuming that the volumes are additive, calculate the concentrations of each ion present in the final solution.arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning