Several alloys that contained only silver and copper were analyzed by dissolving weighed quantities in nitric acid, introducing an excess of iodate ions, and bringing the filtered mixture of silver iodate and copper (II) iodate to constant mass. Calculate the percentage composition of the alloy if 0.8165 alloy sample gives 2.176 gram of precipitate. %Ag %Cu

Several alloys that contained only silver and copper were analyzed by dissolving weighed quantities in nitric acid, introducing an excess of iodate ions, and bringing the filtered mixture of silver iodate and copper (II) iodate to constant mass. Calculate the percentage composition of the alloy if 0.8165 alloy sample gives 2.176 gram of precipitate. %Ag %Cu

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

Mark and John, two vinegar enthusiasts, are each tasked to determine the acetic acid content of their respective vinegar concoctions by titration. First, a 1 M-labeled KOH solution was standardized against the KHP (MW = 204.22 g/mol) standard that is 99.4% pure. In the process, 0.540 g KHP was found to require 2.80 mL of the KOH solution to completely react up to the phenolphthalein endpoint. Then, Mark and John both prepared their samples by taking 10.0-mL aliquots of each vinegar and diluting them to 25.0 mL. Using the same titrant and indicator, Mark’s vinegar required 18.60 mL of the standardized titrant to reach the endpoint, while John’s vinegar required 16.50 mL of the same titrant to reach the same endpoint. Question: What is the acetic acid concentration of Mark’s and John’s vinegar in molarity given that the Concentration of KOH is 9386 M?
25 ml of 0.515 M K2S solution is mixed with 30 ml of 0.833 M HNO3 solution to give the following reaction : K2S (aq) + 2HNO3 (aq) > 2KNO3(aq) + H2S (g) 1. Calculate concentration of [ K+ ] and [S2- ] in the mixture when the reaction is complete
2. A 0.4912-g sample of a petroleum product was burned in a tube furnace, and the SO2 produced was collected in H2O2. SO2(g) + H2O2 → H2SO4 A 25.00-mL portion of 0.00873 M NaOH was introduced into the solution of H2SO4, following which the excess base was back-titrated with 15.17 mL of 0.01102 M HCl. Calculate the sulfur concentration in parts per million.
A 1.00 gram sample of anhydrous cerium sulfate was dissolved in water. Barium nitrate solution was then added until no further precipitation occurred. The precipitate was filtered from the solution then dried and was found to weigh 1.41 g. Determine the formula of the cerium sulfate. Encom calt is hydrated
A solution containing KCl (74.551 g/mol) is analyzed by the Mohr method. A 0.5863 g sample is dissolved in 100 mL of water and titrated to the Ag2CrO4 end point, requiring 42.20 mL of 0.0350 M AgNO3. A blank titration requires 0.80 mL of titrant to reach the same end point. Report the %KCl in the sample
A 4.908-g sample of a petroleum product was burned in a tube furnace, and the SO2 produced was collected in 2% H2 O2. Reaction: SO2 (g) + H2O2 → H2SO4 A 27.00-mL portion of 0.00826 M NaOH was introduced into the solution of H2 SO4, following which the excess base was back-titrated with 15.15 mL of 0.01165 M HCl. Calculate the sulfur concentration in the sample in parts per million. Concentration ppm
When 50.0mL of a 0.335M potassium carbonate solution is mixed with 0.045L of a 0.390M nickel(II) chloride solution the following reaction occurs: K2CO3 (aq) + NiCl2 (aq) → a. Complete the reaction equation b. Calculate the mass of precipitate formed c. Calculate the concentration of each ion in the mixture when the reaction is complete
part b
Analytical chemistry
3) When excess sliver nitrate was added to 25.00 ml of barium chloride, a precipitate of sliver chloride formed at the bottom of the beaker. If the mass of the precipitate was 4.30g, calculate the initial concentration of barium chloride.
During the titration, 25.0 mL of the 0.0233 M saturated calcium hydroxide solution was titrated with 32.0 mL of 0.0182 M sulfuric acid. What concentration of CaSO4 forms during the reaction? Ca(OH)2 (aq) + H₂SO4 (aq) →>> CaSO4(s) + 2H₂O(1) [CaSO4] = [?] M [Caso] Enter
If 30.0 g of LiOH is added to 0.650 L of 1.00 M Cd(NO₃)₂, how many grams of precipitate will be formed in the following precipitation reaction? a) Write a balanced equation. Identify a precipitate. Include states of matter. b) Determine how much precipitate would form if all reactant 1 ( LiOH) would be used up. c) Determine how much precipitate would form if all reactant 2 ( Cd(NO3 )2 would be used up. d) State Limiting reactant , and theoretical yield ( in grams) of the precipitate that would form from the given amounts.