A solution in part C initially contains (4.2100x10^-4) molar SCN¯ and (3.1700x10^-3)molar Fe3+This solution was then measured using the colorimeter, and an absorbance of(5.01x10^-1) was recorded.The constant determined in part A of the experimentwas found to be (3.4800x10^3).Using the data provided above, determine the equilibrium concentration of Fe3+[Fe3+ ]e in this solution.Note: Your answer is assumed to be reduced to the highest power possible.Your Answer:x10Answerunits

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Answered: A solution in part C initially contains…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter20: Molecular Spectroscopy And Photochemistry

Section: Chapter Questions

Problem 67CP

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A solution is prepared such that the initial concentration of A2+ is 1.50x103 M and the initial concentration of X is 4.60x10-3 M. A2+ and X are allowed to react as shown below to establish equilibrium with the complex AX2+. In a colorimetry experiment, the equilibrium concentration of the complex AX2+ is determined to be 8.9x10-4 M. A2* (aq) + X (aq) =Ax2+ (aq) %3D Complete the ICE table below by selecting the correct value or expression to place in the ICE table from the drop-down menu. A2+ (aq) X (ад) АХ2+ (aq) Initial concentration Change in concentration Equilibrium concentration expression Equilibrium concentration value
Calculate the equilibrium isothiocyanatoiron(III) ion concentration, [FENCS2*leg• you will report when making your standard curve. Give your answer to three decimal places. Also give your answer in millimolar (mM) (because you won't be able to enter an answer in scientific notation here). Fe(NO3)3 0.10 M HNO3 NaSCN 0.194 M 1.97 x 10-3 M initial buret reading (mL) final buret reading (mL) 0.02 0.03 0.01 1.87 0.39 7.57
. 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!!
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lodine is sparingly soluble in pure water. However, it does 'dissolve' in solutions containing excess iodide ion because of the following reaction: |¯ (aq) + 1₂(aq) --> 13¯ (aq) K = 699. For each of the following cases calculate the equilibrium ratio of [13] to [1₂]. 2.00×10-2 mol of l2 is added to 1.00 L of 2.00×10-¹ M KI solution The solution above is diluted to 6.00 L.
[Ni(NH₂)]²+ complex K, = 5.50×108 at 25°C. Suppose equal volumes of 0.0046M Ni(NO3), solution and 0.76M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Ni™ ion. ..2+ For the aqueous Round your answer to 2 significant digits. Пм □ x10 X Ś
How many moles of Fe(OH)2 (Ksp = 1.82 x 10-15) will dissolve in 1.5 liter of water buffered at pH = 8.14?
Calcium ion forms a weak 1:1 complex with nitrate ion with a formation constant of 2.0. Whatwould be the equilibrium concentrations of Ca2+ and Ca(NO3)+ in a solution prepared byadding 10 mL each of 0.010 M CaCl2 and 2.0 M NaNO3? Neglect diverse ion effects. 6. The formation constant of the silver–ethylenediamine complex, Ag(NH2CH2CH2NH2)+, is5.0 × 104. Calculate the concentration of Ag+ in equilibrium with a 0.10 M solution of thecomplex. (Assume no higher order complexes.)7. What would be the concentration of Ag+ in Problem 6 if the solution contained also 0.10 Methylenediamine, NH2CH2CH2NH2? 8. Silver ion forms stepwise complexes with thiosulfate ion, S2O32−, with Kf 1 = 6.6 × 108 andKf 2 = 4.4 × 104. Calculate the equilibrium concentrations of all silver species for 0.0100 MAgNO3 in 1.00 M Na2S2O3. Neglect diverse ion effects.
Consider the insoluble compound silver bromide, AgBr. The silver ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of AgBr (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Ag(NH3)₂, K-1.6x107. Use the pull-down boxes to specify states such as (aq) or (s). +
provide explanation of formula.
1 Determine the solubility of Al(OH) 3 (ksp-1 (Ksp = 1.8 x 10-337 in a solution with pH = 2.00
Given the values of K and Kb below, which of the systems given would be most suitable to use to construct a buffer of pH 97 HCOOH, K, = 1.8 x 104 CH3COOH, K3=18x105 H3ASO4. Ka1 = 6.0 x 10, Ka2 = 1.1 x 10, Ka3 = 3 x 1012 C5H5N, Kp = 1,7x10-9 NH3 КЬ - 1.3 х. 10-5 OA H3ASO4/NaH2As04 eB. HCOOH/NAHCOO OC. C5H5N/ C5H5NHCI OD.CH3COOH/KCH3CO0 FOE NH4C/NH3

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