when you mix osmium (III) nitrate solution and rubidium suulfide solution a precipitation Teae occurs. a) What are the chemical formulas for osmium (III) nitrate and rubidium sulfide? What are their molar masses? (5 sig figs) b) Write a balanced molecular equation for the precipitation reaction. Make sure to include physical states. c) If you have 65.0 mL of 3.85 M solution of each, which is the limiting reagent? What is theoretical yield of precipitate (in grams)? d) If you obtain 35.1 g of precipitate, what is your percent yield?

when you mix osmium (III) nitrate solution and rubidium suulfide solution a precipitation Teae occurs. a) What are the chemical formulas for osmium (III) nitrate and rubidium sulfide? What are their molar masses? (5 sig figs) b) Write a balanced molecular equation for the precipitation reaction. Make sure to include physical states. c) If you have 65.0 mL of 3.85 M solution of each, which is the limiting reagent? What is theoretical yield of precipitate (in grams)? d) If you obtain 35.1 g of precipitate, what is your percent yield?

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...

See similar textbooks

Similar questions

if 38.0 g of KCl (MM=74.55 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of KCi in the resulting solution?
What mass of Naz CrO4 is required to precipitate all of the silver ions from 20.0 mL of a 0.200 M solution of AgNO, ? Mass =
A sample of an unknown sulfate compound has a mass of 0.100 g. Addition of excess barium chlo- ride solution to the sample forms a barium sulfate precipitate of mass 0.0676 g. What is the mass % of sulfate ion in the unknown sample?
1.) What volume in mL of 0.220 M HBr solution is required to produce 0.0185 moles of HBr? 2.) If 11.3 g of KBr (MM = 119.00 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of KBr in the resulting solution? 3.) If 25.0 mL of a 7.90 M HCl solution is diluted to 2.00 L, what is the molarity of the new solution? 4.) What quantity in moles of KBr are there in 225.0 mL of 0.155 M KBr?
3. A student mixes 100.0 mL of a 0.100 M solution of potassium phosphate with 100.0 mL of a 0.125 M solution of copper (II) sulfate and obtains a blue solid. (a) Write the balanced chemical equation for the reaction including physical states. (b) Determine the limiting reagent. (c) Calculate the number of moles of the excess reagent after the reaction is completed. Record servation
1. When the following cations and anions react, if the product is insoluble in water, write the net ionic equation for the precipitate reaction.(a) Ag+ and Cl- (b) Ba2+ and SO42- (c) Na+ and Cl-, (d) Zn2+ and NO3-
If 40.7 g of CH₃OH (MM = 32.04 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of CH₃OH in the resulting solution?
Write the balanced molecular chemical equation for the reaction in aqueous solution for copper(1) chloride and lithium carbonate. If no reaction occurs, simply write
Translate each word equation into a balanced chemical euqation, including phyical states for all reactants and products. a) potassium iodide + chlorine (aq) → iodine + potassium chloride b) ammonium carbonate → ammonia gas + carbn dioxide gas + steam c) In the preparation of alum, sulfuric acid is added to a mixture containing excess potassium hydroxide. Write a balanced chemical equation for the reaction of sulfuric acid with potassium hydroxide.