LJ Labflow - report: Report and Dat: xN Mylab and MasteringCourse Homeb Answered: zinc metal is added to X->A openvellum.ecollege.com/course.html?courseld=16418591&OpenVellumHMAC=013628d899c889f48948ece53ef3ebff#10001First, write the balanced equation for the reaction.ScoresAGNO3 (aq) + KCI(aq) → AgCl(s) + KNO3(aq)Pearson eTextNext, calculate the moles of the known substance, KCI, by dividing the given mass, after converting from mg to g (1000 mg =1g), by its molar mass, 74.55 g/mmultiply by the mole ratio from the balanced equation, 1:1, to convert from mol KCl to mol AGNO3. Finally, convert mol AgNO3 to M AgN03 using its given voconverting from mL to L (1000 mL =1L).Study Area1 mot KÇI1000 nLMolarity of AgNO3 = 0.765 mg KCI ×1 mol AgNO31 motKCIDocument Sharing= 3.86 x 101000 ng74.55 KCI26.6 mL AGNO31LUser SettingsCourse Tools>Part DIf 45.3 mL of 0.116 M HCl solution is needed to neutralize a solution of KOH, how many grams of KOH must be present in the solution??тSubmitRequest AnswerProvide FeedbackNext >P PearsonCopyright © 2021 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy. | Permissions | Contact Us |https://session.masteringchemistry.com/myct/itemView?assignmentProblemID=1629177142:03 PMP Type here to search3/12/2021

Given volume of solution = 45.3 mL molarity of HCl = 0.116 M Required data - molar mass of…

Answered: If 45.3 mL of 0.116 M HC1 solution is…

If 45.3 mL of 0.116 M HC1 solution is needed to neutralize a solution of KOH, how many grams of KOH must be present in the solution? ? m = Submit Request Answer

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter23: Potentiometry

Section: Chapter Questions

Problem 23.26QAP

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Iron corrodes to produce rust, Fe2O3, but other corrosionproducts that can form are Fe(O)(OH), iron oxyhydroxide,and magnetite, Fe3O4. (a) What is the oxidation numberof Fe in iron oxyhydroxide, assuming oxygen’s oxidationnumber is -2? (b) The oxidation number for Fe in magnetitewas controversial for a long time. If we assume thatoxygen’s oxidation number is - 2, and Fe has a uniqueoxidation number, what is the oxidation number for Fein magnetite? (c) It turns out that there are two differentkinds of Fe in magnetite that have different oxidationnumbers. Suggest what these oxidation numbers are andwhat their relative stoichiometry must be, assuming oxygen’soxidation number is -2.
Given: Fe+2 + 2e- ? Fe E red o = - 0.44 V Ag+ + e- ? Ag E red o = 0.80 V Fe+2 (aq) + 2Ag(s) ? Fe(s) + 2Ag+(aq) What is E o for the reaction? Is the reaction spontaneous at standard state conditions? What is ΔG o for this reaction? What is the value of the equilibrium constant for this reaction?
please show weather its a S,l,g or aq in the chemical equation
For Redox Analysis of Iron... ~0.02 M of potassium dichromate is prepared as titrant for dried unknown. ~.3 g of sample, 50ml of 6M HCl, 20mL SnCl2, 10 mL of saturated HgCl2 solution, 60 mL of 3M H2SO4, 15mL of concentrated H3PO4, 100mL DI water. HCl (+ heat in fumehood until samples dissolves), SnCl2 (added with pipet until solution changes from yellow to colorless/light green with 3 drops in excess), HgCl2 (after cooling), H2SO4, H3PO4, DI Water, is added to the sample solution with 8 drops of diphenylamine sulfonate indicator then titrated with the potassium dichromate to a violet blue endpoint. 4. Why is it necessary to carry out the reduction of iron and then the titration, before going on to the next sample 5. If you look carefully, there are pieces of tin metal on the bottom of the SnCl2 reagent solution. Why is it there?
For Redox Analysis of Iron... ~0.02 M of potassium dichromate is prepared as titrant for dried unknown. ~.3 g of sample, 50ml of 6M HCl, 20mL SnCl2, 10 mL of saturated HgCl2 solution, 60 mL of 3M H2SO4, 15mL of concentrated H3PO4, 100mL DI water. HCl (+ heat in fumehood until samples dissolves), SnCl2 (added with pipet until solution changes from yellow to colorless/light green with 3 drops in excess), HgCl2 (after cooling), H2SO4, H3PO4, DI Water, is added to the sample solution with 8 drops of diphenylamine sulfonate indicator then titrated with the potassium dichromate to a violet blue endpoint. 1. What is the purpose of the phosphoric acid in this experiment? Please be specific. 2. How does the Diphenylamine sulfonate indicator work? What chemical reaction causes the color change? How is an indicator chosen in a redox reaction?
For Redox Analysis of Iron... ~0.02 M of potassium dichromate is prepared as titrant for dried unknown. ~.3 g of sample, 50ml of 6M HCl, 20mL SnCl2, 10 mL of saturated HgCl2 solution, 60 mL of 3M H2SO4, 15mL of concentrated H3PO4, 100mL DI water. HCl (+ heat in fumehood until samples dissolves), SnCl2 (added with pipet until solution changes from yellow to colorless/light green with 3 drops in excess), HgCl2 (after cooling), H2SO4, H3PO4, DI Water, is added to the sample solution with 8 drops of diphenylamine sulfonate indicator then titrated with the potassium dichromate to a violet blue endpoint. 3. How would you prepare a complete anlaysis procedure using KMnO4 as the oxidant instead of K2CrO7? Include sample and solution preparation, approximate weights of samples and reagents, procedure and chemical reactions. In particular what is the purpose of the Zimmerman Reinhardt Reagent?
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Many applications of electrochemistry have been in chemical analysis.Suppose a Fe|Fe2+ concentration cell is set-up in which the [Fe2+] = 1.0 x10¯2 M in one compartment but the concentration in the othercompartment is unknown. The Ecell was measured at 0.024V when thehalf-cells were connected.(i) Without doing a numerical calculation, is the unknown more orless concentrated than the 1.0 x 10¯2 M solution? Justify youranswer(ii) Calculate the unknown concentration.(iii) Does your calculated answer agree with your original answer?Why?
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(c)Ions that react with Ag+ like SCN- can be determined electrogravimetricallyby deposition on a silver working anode:Ag(s) + SCN- ≤ AgSCN(s) + eA silver anode with initial mass of 12.4730 g was used to electrolyse 85.00 mL of asolution of 0.0245 M KSCN. At the end of the experiment, the anode weighed12.5767 g. How long did the experiment take, if a current of 100 mA was used?