The iodide ion concentration in a solution may be determined by the precipitation of lead iodide. Pb2+ (aq) + 21 (aq) →→→→PbI₂(s) A student finds that 22.10 mL of 0.5530 M lead nitrate is needed to precipitate all of the iodide ion in a 25.00-mL sample of an unknown. What is the molarity of the iodide ion in the student's unknown? M

The iodide ion concentration in a solution may be determined by the precipitation of lead iodide. Pb2+ (aq) + 21 (aq) →→→→PbI₂(s) A student finds that 22.10 mL of 0.5530 M lead nitrate is needed to precipitate all of the iodide ion in a 25.00-mL sample of an unknown. What is the molarity of the iodide ion in the student's unknown? M

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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A solution is prepared by dissolving 2.95 g Co2(SO4)3 in enough water to make 1.00 L of red solution; the red color is due to the presence of the cobalt ions. To this solution was added 1.52 g of magnesium powder. A redox reaction occurred, in which the magnesium atoms lose all of their valence electrons and the red color of the solution fades. (a) Write the total reaction that occurs and the net ionic equation for the redox process. (Assume that one of the products of the redox reaction is a metal.) (b) Calculate the initial concentration of cobalt ions, the final concentration of cobalt ions, and the final concentration of magnesium ions.
A 8.92 g sample of an aqueous solution of hydroiodic acid contains an unknown amount of the acid. If 11.7 mL of 2.79 M potassium hydroxide are required to neutralize the hydroiodic acid, what is the percent by mass of hydroiodic acid in the mixture?
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A student mixes 100.0 mL of 0.500 M AgNO3 with 100.0 mL of 0.500 M CaCl2. Write the balanced molecular equation for the reaction. Write the net ionic equation for the reaction. How many grams of precipitate will form? What is the concentration of Ag+, NO3‒, Ca2+, and Cl‒ in the final solution (assume volumes are additive).
A solution contains Cr3+ and Mg2+. The addition of 1.00 L of 1.51 M NaF solution is required to cause the complete precipitation of these ions as CrF3(s) and MgF2(s). The total mass of the precipitate is 50.1 g . Find the mass of Cr3+ in the original solution.
copper (II) ion is precipitated from solution by adding 3.00 M NaOH(aq) resulting in a blue precipitate. What volume in milliliters would be necessary to fully precipitate the copper (II) ion from 100.0 mL of a 0.288 M solution of copper (II) nitrate.
when 100.0 mL of a 2.00 M solution of KOH(aq) is added to 100.0 mL of a 2.00 M solution of Mg(NO3)2 what is the mass of the precipitate(s) that form?
Barium can be analyzed by precipitating it as BaSO4BaSO4 and weighing the precipitate. When a 0.265 gg sample of a barium compound was treated with excess H2SO4H2SO4 8.50×10−2 gg of BaSO4BaSO4 formed. What is the percentage of barium in the compound?
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A 10.4 g sample of an aqueous solution of perchloric acid contains an unknown amount of the acid. If 24.3 mL of 0.481 M potassium hydroxide are required to neutralize the perchloric acid, what is the percent by mass of perchloric acid in the mixture?
d) A 38.5mL sample of 0.875M AgNO, solution is mixed with 51.0mL sample of 0.744M NaCl solution. The AgCl precipitated has a mass of 2.06g. Calculate the limiting reactant, the theoretical yield, and percent yield. AGNO3(aq) + NaClaq) → AGCI6) + NaNO3(aq)
A precisely measured volume of 250.0 mL of a saturated NaCl(aq) solution at room temperature is heated to evaporate the solvent and crystallize the solute.The mass of the dry solute is measured to be 88.8 g. What is the solubility of the sodium chloride solution?