2. When making the calibration curve in Part 1 of the experiment, it was assumed that the reactionmixture went to completion. That is, you assumed that [SCN] = [FeNCS2+]eq when the [Fe3+]o was inlarge excess. Using your average Keq (Part 2), calculate the equilibrium concentrations of each speciesin the last mixture (2mL Fe3+ and 225μL SCN-) of Part 1.a. [Fe3+]eq (M)b. [SCN]eq (M)c. [FeNCS²+]eq (M) Average Keq2000225Info (110)Try 1: ✓₤.02E-4Try 1:1522 2Info (320)110.844EditInfo (120)

See the images belowExplanation: Fe3+ = (0.001M)×(2,000μ(L/1,000 )μ (L/m)…

Answered: 2. When making the calibration curve in…

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter8: Polyfunctional Acids And Bases

Section: Chapter Questions

Problem 3P

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The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mL
In a reaction mixture 20.0mL of 0.010M KI, 10.0mL of 0.040M KBrO3, 10.0mL of 0.040M Na2S2O3, and 20.0mL of 0.10M HCl were mixed. What is the concentration of [I-], [BrO3-], and [H+]?
It is found that 8.70e-09 g of Ga(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Ga(OH)3.The Ksp of Y2(CO3)3 at 25 oC is 1.03e-31. What is the molar solubility of Y2(CO3)3?
Each equilibria has several disturbances. Each one needs to be addressed separately. For each disturbance to the equilibrium reaction, state how the disturbance affected the equilibrium (shifting it left or shifting it right). Explain specifically what occurred and how it pairs with the observation. Pour about 1 milliliter of deionized water to each of three test tubes. Add 1 drop of 0.1 M Fe(NO3)3 and 1 drop of 0.1 M KSCN to each test tube. Add two more drops of 0.1 M Fe(NO3)3 to one of the tubes, and two more drops of 0.1 M KSCN to another of the test tubes. Try to compare the colors of the solutions as quantitatively as possible. Record your observations and explain what happened using Le Châtelier's principle. Part 5: Iron/Thiocyanate Equilibrium Fe,* {pale yellow} + SCNFe(SCN)2²*{deep red) Add 1 drop of 0.1 M Fe(NO₂), to each test tube Add 1 drop of 0.1 M KSCN to each test tube. Add two more drops of 0.1 M Fe(NO3)3 to one of the tubes. Add two more drops of 0.1 M KSCN to the other…
. A solution was prepared by mixing 4.00mL of 2.00 x 10-3 M Fe(NO3)3 and 3.00mL of 5.00 x 10-3 M NaSCN and diluting the mixture with water to a total of 10.00mL. Use your average value of Kc to calculate the equilibrium concentration of FeSCN2+ in the mixture. [Hint: Use as many significant figures as you legitimately can in your calculations] my average you can find on the picture below PLS HELP ASAP!!
How will mistakenly using solution 1 to calibrate the spectrophotometer, instead of the blank affect the calcualted concentration of FESCN2+ at equilibrium and the calculated concentrations of Fe3+ and SCN- uncomplexed at equilibrium? The blank contained 5.00mL of 0.00200 M Fe(NO3)3 (in 0.1M HNO3) and 5.00mL of 0.1 M HNO3. Solution 1 contained 5.00mL of Fe(NO3)3 (in 0.1M HNO3), 1.00mL of 0.00200 M NaSCN (in 0.1 M HNO3) and 4.00mL 0.1M HNO3. Fe3+(aq)+SCN-(aq)->FeSCN2+(aq)
. 29) The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated: (a) TlCl: [Tl+] = 1.21 ×× 10–2 M, [Cl–] = 1.2 ×× 10–2 M (b) Ce(IO3)4: [Ce4+] = 1.8 ×× 10–4 M, [IO3−][IO3−] = 2.6 ×× 10–13 M (c) Gd2(SO4)3: [Gd3+] = 0.132 M, [SO42−][SO42−] = 0.198 M (d) Ag2SO4: [Ag+] = 2.40 ×× 10–2 M, [SO42−][SO42−] = 2.05 ×× 10–2 M (e) BaSO4: [Ba2+] = 0.500 M, [SO42−][SO42−] = 4.6 ×× 10−8 M
In following these steps . Complete the table and provide th given chemical reactions in the qualitative analaysis of Group 3 Cations. Procedure 1. Place 20 drops of each of the following aqueous solutions to separate centrifuge tubes: 0.1M Cr (NO3)3, 0.1M Al (NO3)3, 0.1M Co (NO3)2, 0.1M Zn (NO3)2, 0.1M Mn (OH)2, 0.1M Ni (NO3)2, 0.1 M Fe (NO3)3. Make each solution basic by adding few drops of 6M NH4OH. Confirm using a litmus paper. 2. Add 5 drops of freshly prepared 6M (NH4)2S to each centrifuge tube. Place the samples in thecentrifuge machine for 3 mins. After centrifuge record results. Decant the supernatant liquid of all the samples. 3. Add one drop of NH4OH in each centrifuge tubes. Add 20 drops of distilled water in eachcentrifuge tubes. Then add a few drops of 6M HCl in each solution. Place the samples in the water bath for 10 mins. After water bath, centrifuge the samples for 3 mins. 4. After centrifuge, add a few drops of 6M NH4Cl in each sample. Decant the supernatant liquid…
1. Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, CH3COOH. For 20.0 cm3 of the vinegar, 26.7 cm3of 0.60 mol dm-3 NaOH solution was required.What was the concentration of acetic acid in the vinegar if no other acid was present? (Thanks for your help) A. 0.45 mol dm-3B. 0.60 mol dm-3C. 0.80 mol dm-3D. 1.60 mol dm-3
3. Calculate the [Zn²+] in two solutions and compare the results (ZnS, Ksp = 2.5 X 10-22). (a) a solution that is in equilibrium with ZnS(s) and in which [H3O+] = 1.0 X 10-5 M and [H₂S] = 0.10 M. (b) a solution that is in equilibrium with ZnS(s) and in which [H3O+] = 1.0 X 10-³ M and [H₂S] = 0.10 M.
Zn2+ forms two complexes with acetate, with the given overall formation constants. 1. Zn? + (aq) + CH,CO,(aq) = Zn(CH,CO,)*(aq) Kj = B1 = 19 2. Zn² + (aq) + 2 CH,CO,(aq) = Zn(CH;CO,),(aq) B2 = 120 Find the stepwise formation constant, K2, for the reaction 3. Zn(CH;CO,)*(aq) + CH,CO, (aq)= Zn(CH;CO,),(aq) K2 =? K2 = %3D You prepare 1.00 L of solution containing 2.00 x 10-4 mol Zn(CIO,), and 0.100 mol CH, CO, Na. Calculate the fraction of zinc in the form Zn2+. + ||
What mass of ZnS (Ksp = 2.5 x 10-22) will dissolve in 325.0 mL of 0.050 M Zn(NO3)2? Ignore the basic properties of S2-.

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