chloride does the sample contain? (CI. JJ.J 7. Arsenic in a 5.0 gram sample is converted to H3ASO4 by appropriate procedures. After the acid is neutralized and converted to AsO ion, 35.0 mL, 0.04952 M AGNO3 is added to precipitate Ag3AsO4(s) 3Ag* + AsO,-→ Ag3AsO4(s) 1,73mmol 8.88 mL of 0.1110 M KSCN was used to titrate excess Ag* Ag* +SCN AgSCN(5) 0,9856nmol Calculate the mass percentage of As2O3 in the sample? (As203: 198)

chloride does the sample contain? (CI. JJ.J 7. Arsenic in a 5.0 gram sample is converted to H3ASO4 by appropriate procedures. After the acid is neutralized and converted to AsO ion, 35.0 mL, 0.04952 M AGNO3 is added to precipitate Ag3AsO4(s) 3Ag* + AsO,-→ Ag3AsO4(s) 1,73mmol 8.88 mL of 0.1110 M KSCN was used to titrate excess Ag* Ag* +SCN AgSCN(5) 0,9856nmol Calculate the mass percentage of As2O3 in the sample? (As203: 198)

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

What’s the answer in mol
5. For each of the following equations, balance them, put in the missing solubility states and then write the net ionic equations. CdCl2( Ednanou Cd(s) + HCI(aq) - H2(g) + a. slueeloM ebrsled bns elolgmo nge acnom b. Fe(CIO3)2() + NaBr(L) → FeBr2( NaCIO3 (L)
A 50.0 ml solution contains only Na2SO4 (MW 142.04 g/mole). If 40.0 ml of 0.25 M BaCl2 is needed to precipitate all the SO42- as BaSO4, what mass of Na2SO4 was in the original solution? What is the concentration of Cl- in the final solution?
! ( please ans with explanation )
solution after precipitation is complete. 68. The drawings below represent aqueous solutions. Solution A is 2.00 L of a 2.00-M aqueous solution of copper(II) nitrate. Solution B is 2.00 L of a 3.00-M aqueous solution of potas- sium hydroxide. (0) suiro Cu²+ ebro NO3 БО K+ OH™ A B a. Draw a picture of the solution made by mixing solutions A and B together after the precipitation reaction takes place. Make sure this picture shows the correct relative volume compared to solutions A and B, and the correct relative number of ions, along with the correct relative amount of solid formed. b. Determine the concentrations (in M) of all ions left in solution (from part a) and the mass of solid formed.
4. When a solutions of aluminum sulfate and potassium hydroxide are mixed, a precipitate forms. a. Write a balanced net ionic equation for the reaction. b. Calculate the mass of the precipitate when 3.89 g of aluminum sulfate in 100mL of solution is combined with 50 mL of the o.300 M KOH. c. What is the molarity of the ion in excess? (Ignore the spectator ions and assume that volumes are additive)
Gg.168.
6. The purity of a sample of sodium oxalate, NazC2O4, is determined by titrating with a standard solution of KMNO4. If a 0.5116-g sample requires 35.62 mL of 0.0400 M KMnO4 to reach the titration's end point, what is the %w/w Na2C2O4 in the sample.
What volume of 0.416M Mg(NO3)2 should be added to 255 mL of 0.102 M KNO3 to produce a solution with a concentration of 0.278 M NO3– ions?
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)
Typewritten for upvote. No upvote for handwritten. Thank you
Three aqueous solutions are mixed, 1.0 M (NH4)2SO4, 1.0 M Sr(OH)2 and 1.0 M CoCl3. The two precipitates are ____ and ____.