How do I calculate % in this? The arsenic in a 1.010 g sample of pesticide was converted to H3ASO4 by appropriate means. The acidwas neutralized and the arsenate precipitated quantitatively as Ag3AsO4 with exactly 40.00 mL of0.06222 M AgNO3.3Ag* + AsO4 → Ag3AsO4The excess Ag" was titrated with SCN , requiring 10.76 mL of 0.1000 M KSCN; the reaction being:Ag* + SCN→ A SCN(s).Calculate the percentage of As2O3 (MM = 197.841 g/mol) in the original sample.

Answered: Image /qna-images/answer/6ba518fc-7fed-44a6-b5fc-0341c5b05301.jpg

arsenic in a 1.010 g sample of pesticide was converted to H3ASO4 by appropriate means. The acid neutralized and the arsenate precipitated quantitatively as Ag3As04 with exactly 40.00 mL of 22 M AgNO3. 3Ag* + AsO4→ Ag3AsO4 xcess Ag* was titrated with SCN , requiring 10.76 mL of 0.1000 M KSCN; the reaction being: Ag* + SCN → A SCN(s). late the percentage of As2O3 (MM = 197.841 g/mol) in the original sample.

arsenic in a 1.010 g sample of pesticide was converted to H3ASO4 by appropriate means. The acid neutralized and the arsenate precipitated quantitatively as Ag3As04 with exactly 40.00 mL of 22 M AgNO3. 3Ag* + AsO4→ Ag3AsO4 xcess Ag* was titrated with SCN , requiring 10.76 mL of 0.1000 M KSCN; the reaction being: Ag* + SCN → A SCN(s). late the percentage of As2O3 (MM = 197.841 g/mol) in the original sample.

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

True or false: the determination of a molar mass of a compound by the titration method used today depends on having a pure sample of the unknown compound? Explain.
3. You have dissolved 5 g of a rock containing a mixture of calcium carbonate and inert sand in 100 mL of 1 mol L-1 HCI. You measure the calcium concentration of the resulting solution as 0.03 mol L-1 in that 100 mL solution. Calculate the percentage calcium carbonate by weight in the rock sample.
Use the data below to determine the % by mass of Fe to TWO decimal places, if a 0.019 M KMnO4 solution was used for the titration. (MM Fe = 56 g/mol) mass of iron compound (g) 0.637 initial buret reading (mL) 0.86 16.60 final buret reading (mL) Type your answer...
1. A 500-ml volumetric flask contains 150 ml of 0.200 N H2SO4. By adding a more concentrated H2SO4, the solution is brought to the mark and after mixing is found to be 0.150 M . What was the normalityof the acid solution?
O SIMPLE REACTIONS Ghaya Determining the volume of base needed to titrate a given mass... A chemistry student weighs out 0.0544 g of acrylic acid (HCH,CHCO,) into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1900 M NAOH solution. Calculate the volume of NAOH solution the student will need to add to reach the equivalence point. Round your answer to 3 significant digits. mL x10 18 Ar Explanation Check © 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use I Privacy Accessibility 7:37 PM ») ENG 2/27/2021 P Type here to search DELL PrtScr Insert Home End Delet Esc F8 F9 F10 F11 F12 F1 F2 F3 F4 F5 F6 F7 # 24 & Back 2 ĭ 3 ř 4{5 0 6 7 7 Y 8 A 9 q o
a sample of sodium carbonate is being dried. after 1 hour of drying the mass of the sample was 0.337 g. after an additional 30 minutes of drying the mass of the sample is 0.333g what is the percent change
How many moles of Agl will be formed when 75.0ml of 0.300 M AgNo3 is completely reacted according to the balanced chemical equation
Question &.. When answering this problem, report the answer with the appropriate number of significant figures. When entering units, use proper abbreviated units with proper capitalization. A titration is performed to determine the amount of sulfuric acid, H2SO4, in a 6.5 mL sample taken from car battery. About 50 mL of water is added to the sample, and then it is titrated with 43.37 mL of a standard 0.5824 molar NaOH solution. You balanced this reaction in a previous problem. How what is the molar concentration of sulfuric acid in the original sample? Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer units
3. In a given dilution, the volume of the solution increases from 10.00 mL to 50.00 mL. We can conclude that: LIf the molarity of the final solution is o.0045oo M, the molarity of the original solution is o.02250 M II. The dilution factor is 5
If 10. g of AgNO3 is available, what volume of 0.35 M AgNO3solution can be prepared?
Fill in the blank with the appropriate term: A .. is an insoluble solid that comes out of a liquid solution.
A 0.415 g sample of aspirin prepared in the laboratory is dissolved in 95% ethanol, diluted with water, and titrated to the endpoint with 18.5 mL of a 0.135 M NaOH, what is the % purity of the aspirin.