<5 of 12Constants I Periodic TablePart BCalculate the number of moles of Cl atoms in 3.01 x102 formula units of magnesium chloride,MgCl2.Express your answer numerically in moles.View Available Hint(s)ΑΣφ?moles ClSubmitProvide FeedbackNext>P Pearsonion Inc. All rights reserved. | Terms of Use | Privacy Policy Permissions | Contact UsMacBook AirDIIDD)F7F8F9F10F11F12&t

Calculation for number of moles of MgCl2:

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Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter11: Solving Equilibrium Problems For Complex Systems

Section: Chapter Questions

Problem 11.3QAP

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answe all 3 parts as the policy allows us to asl 3 questions each time please and thank you:))
A mixture containing only Al2O3 (FM 101.96) and Fe2O3 (FM 159.69) weighs 2.019 g. When heated under a stream of H2, the Al2O3 is unchanged, but the Fe2O3is converted to metallic Fe plus H2O(g). If the residue weighs 1.774 g, what is the weight percent of Al2O3 in the original mixture?
7. Consider a1Msolution ofNa3AsO4. Write the charge and mass balance equations for this system. (please type answer not write by hend)
What is the concentration of a 62.0 % (w/w) concentrated nitric acid (HNO3, Mr = 63.0 g/mol) solution (density: 1.32 g/cm3) in mol/dm3 (molarity) and g/dm3 (mass concentraion) units? How many cm3 do you need to dilute into 200.0 cm3 from that concentrated nitric acid if you would like to have a solution with a concentration of 3.0 mol/dm3 ?
Stock iron(II) solution (200Ug mL-1 Fe) ferrous ammonium sulfate hexahydrate mass= 0.1437g, transfer it to a 100 ml beaker. add 15 ml approx of water and 15m1 'approx of dilute sulphuric acid (2M H2SO.). then transfer FeII to 100 ml flask makeup to the mark with water. calculate the moles of ferrous ammonium sulfate hexahydrate solution in unit ug/mL.
An aqueous solution of sucrose (C12H22O11) is prepared by dissolving 7.4045 g in sufficient deionized water to form a 100.00 mL solution. Calculate the molarity of the solution. Do you mind showing work? I would assume that (given) gram weight (times moles present/divided by mole(s) of compound) then divided - again by compound weight will give a percentage, then divded by the .....that's where I'm a little lost. thanks
Vanadic ion, V3+, forms green salts and is a good reducingagent, being itself changed in neutral solutions to thenearly colorless ion V(OH)4+. Suppose that 15.0 mL of a0.200-M solution of vanadic sulfate, V2(SO4)3, was neededto reduce completely a 0.540-g sample of an unknownsubstance X. If each molecule of X accepted just oneelectron, what is the molecular weight of X? Suppose thateach molecule of X accepted three electrons; what wouldbe the molecular weight of X then?
Please show steps and states (aq),(s).. etc thank you
Magnesium +Acetic Acid --> C2HG5+ O2 ---> Iron (III) carbonate -->
The mercury in a 0.8142-g sample was precipitated with an excess of paraperiodic acid, H5IO6: 5 Hg 2+ + 2 H5IO6 ---> Hg5(IO6)2 (s) + 10 H + The precipitate (MW = 1448.8 g/mol) was filtered, washed free of precipitating agent, dried, and weighed, and 0.4114 g was recovered. Calculate the a) % Hg (200.6 g/mol) b) % Hg2Cl2 (472.1 g/mol)
What is the density of 47.0 wt% aqueous NaOH (FM 40.00) if 17.6 mL of the solution diluted to 1.80 L give 0.172 M NaOH?
Chemistry pls help, I dont understand how this software wants me to enter the answer. its asking lfr the starting amount but its not taking it in the way Im putting it

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