If you use [KMnO4]=0.0252 M,Concentration of FeSO4 7 H2O = 5.70 g/LUsing a 100-mL graduated cylinder, 50 mL sample of FeSO4*7 H₂O will be measured out.To each sample of FeSO4 7 H2O, add 10.0 mL of H2SO4 and 10 mL of H3PO4Concentration of SnCl2 2 H2O 2.85 g/mLUsing a 100-mL graduated cylinder, 50.0 mL sample of SnCl2 2 H₂O will be measured out.No additional acid is needed.#1 KMnO4#1 KMnO4Sample #Initial buret, mLFinal buret, mLFeSO4*7 H2O12.0521.51SnCl2 2 H₂O0.079.54Question) Answer the following questions.b) Determine mol of electron lost per mol of Sn ion.1) In this case, your answer should be in decimal notation (for example, 0.123, not 1.23*10^-1) with the correct number of significant figures. Also follow the unit specified ineach question. Do NOT put its unit in your answer because its unit is shown already in the questions.

Conc of SnCl2.H20 = 2.85 gm/ml Molecular weight of SnCl2.2H20 = 225.65 gm.So, Conc of SnCl2.H20 =…

Answered: If you use [KMnO4]=0.0252 M,…

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter3: Statistical Tests With Excel

Section: Chapter Questions

Problem 6P

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You need 300. mL of 0.500-M K2Cr2O7. Which method is best to prepare this solution? Explain your choice. (a) Dilute 250. mL of 0.600-M K2Cr2O7 to 300. mL. (b) Add 50.0 mL water to 250. mL of 0.250-M K2Cr2O7. (c) Dilute 125 mL of 1.00-M K2Cr2O7 to 300. mL. (d) Add 30.0 mL of 1.50-M K2Cr2O7 to 270. mL of water.
As part of this experiment you will need to determine the concentrations of Fe* and SCN ions present in test tubes 1-9. These values can be calculated using the volumes and concentrations provided in Tables 1 and 2 of the Equilibrium Lab - Procedure and the dilution equation (M,V1 = M2V2). Note: the solutions provided in the lab, and therefore the tables in the lab document, are the compounds used to prepare the solution. You must determine the concentration of the ions based on how these compounds díssociate in solution Complete the following table by filling the the calculated initial concentrations of each substance. Be sure to: Pay attention to significant figures • Round appropriately Use decimal notation (not scientific) Do not include units Test Initial [Fe3*] (M) Initial [SCN'] (M) Tube 1 3 4. 6. 7 8. 2.
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How much amount of solids (in grams) do you need to prepare the following solutions? 1. 500.0 mL 0.1000 M stock EDTA solutiona. Weigh an appropriate amount of Na2H2EDTA2H2O (FW=372.24) to the nearest 0.1 mg 2. 100.0 mL 0.0500 M stock Ca2+ solutiona. Weigh appropriate amount of pure CaCO3 (FW=100.09) to the nearest 0.1 mg into a 250 mL beaker.
Precipitimetry The chloride in a 4.321-g food sample was precipitated through the addition of 50.00 mL of a standard AgNO3 solution (10.00 mL AgNO3 = 11.22 mL KSCN). The precipitate was coated with nitrobenzene and the mixture was diluted to 250.0 mL. A 50.00 mL aliquot was taken from the diluted solution and required 4.56 mL back titration with a %3D standard KSCN solution (22.33 mL KSCN = 0.9758 g AgNO3). %3D Formula Masses: AgNO3 = 169.87; CI = 35.45 Calculate the following: 1. Molar concentration of KSCN solution M %3D 2. Molar concentration of AgNO3 solution M %3D 3. % (w/w) chloride in the original sample =
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chemical equation: What mass of precipitate will form if 1.50 L of highly concentrated Pb(ClO3)₂ is mixed with 0.500 L 0.300 M Nal? Assume the reaction goes to completion. the Balanced equation for the reaction of aqueous Pb(ClO3)2 with aqueous Nal. Include phases. $ 4 mass of precipitate: R F4 V % 5 T F5 G B ^ 6 MacBook Air F6 Y H & 7 N F7 U * 00 8 M DII F8 ( 9 DD F9 O V ) 0 F10 P ^. 1 F11 + g F12 20 del
ock Esc B 1. Brightspace F1 Q A C D ☐app.101edu.co Walmart - Hiring Ce... N 100.0 mL of a 0.775 M solution of KBr is diluted to 500.0 mL. What is the new concentration of the solution? + F2 @ 2 W S Alt X 4 F3 - # 3 E D FA с 144 $ 4 F5 R F 4 11 % 5 V F6 T G A 6 F7 B Y H F8 & 7 2 Question 9 of 9 N DELL FO * D 8 F10 3 9 K F11 O ) F12 Ait P 4 7 +/- PrtScr Ciri
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