Apply the concepts of stoichiometry and solution concentration in this section. Potassium iodide reacts with lead (II) nitrate in the following precipitation reaction2 KI (aq) + Pb(NO3)2 (aq)  KNO3 (aq) + PbI2 (s). What volume of 0.200 M KI solution is required to completely precipitate all of the lead in 255mL of a 0.312 M Pb(NO3)2 solution? An solution is made by dissolving 28.4 g of glucose (C6H12O6) in 355 g of water. The final volume of the solution is 378 mL. Calculate the molarity, molality, mole fraction, mole percent and mass percent of the solution, Hydrochloric acid is usually purchased in a concentrated form that is 37.0 % HCl by mass and has a density of 1.20 g/mL. Describe exactly how to prepare 2.85 L of a 0.500 M HCl to be used in Dr. Henary’s CHEM1211K lab from the concentrated solution. Hint (Find molarity of concentrated solution and use dilution equation. This is how your solution are prepared)

Answer: volume of KI Solution required is 795.6 mL.

Answered: Apply the concepts of stoichiometry and…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.107QE

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Apply the concepts of stoichiometry and solution concentration in this section.

Potassium iodide reacts with lead (II) nitrate in the following precipitation reaction

2 KI (aq) + Pb(NO₃)₂ (aq)  KNO₃ (aq) + PbI₂ (s). What volume of 0.200 M KI solution is required to completely precipitate all of the lead in 255mL of a 0.312 M Pb(NO₃)₂ solution?

An solution is made by dissolving 28.4 g of glucose (C₆H₁₂O₆) in 355 g of water. The final volume of the solution is 378 mL. Calculate the molarity, molality, mole fraction, mole percent and mass percent of the solution,

Hydrochloric acid is usually purchased in a concentrated form that is 37.0 % HCl by mass and has a density of 1.20 g/mL. Describe exactly how to prepare 2.85 L of a 0.500 M HCl to be used in Dr. Henary’s CHEM1211K lab from the concentrated solution. Hint (Find molarity of concentrated solution and use dilution equation. This is how your solution are prepared)

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