Part II: Determination of the Equilibrium ConstantE2E3E4E5E61) Volume of 0.002M Fe(NO)added, mL5,2.2) Volume of 0.002M NASCNadded, mL0.0020.0023) Initial [SCN] of solution, M O.00200024) Initial [Fes-] of solution, M O. 00 2 0.002 6.0020.002 0.002O.002160348. S43-710-8515) Absorbance6) Equilibrium [Fe(SCN)-), M7) Equilibrium [Fes-], M8) Equilibrium [SCN:J, M9) Equilibrium constant, Ke10) Average K. Sample caleulationsShow your work for the following calculations using data from sample ESa) Initial solution concentrations of Fe and SCN.b) Equilibrium concentration of Fe(SCN)c) Equilibrium concentrations of Fer and SCN- (include an ICE table)d) Equilibrium constant

Answered: Image /qna-images/answer/42814934-d63e-4f93-b852-52a75ea44938.jpg

Sample.sakulatim Show your work for the following caleulations uning data from sample E a) Initial solution concentrations of Fes and SCN b) Equilibrium concentration of Fe(SCN)- e) Equilibrium concentrations of Fes- and SCN (include an ICE table) d) Equilibrium constant

Sample.sakulatim Show your work for the following caleulations uning data from sample E a) Initial solution concentrations of Fes and SCN b) Equilibrium concentration of Fe(SCN)- e) Equilibrium concentrations of Fes- and SCN (include an ICE table) d) Equilibrium constant

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.35PAE: In the reaction in Exercise 12.33, another trial was carried out. The reaction began with an initial...

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The following question is taken from a Chemistry Advanced Placement Examination and is used with the permission of the Educational Testing Service. Solve the following problem: MgF2(s)Mg2+(aq)+2F(aq) In a saturated solution of MgF2 at 18 C, the concentration of Mg2+ is 1.21103M . The equilibrium is represented by the preceding equation. (a) Write the expression for the solubility-product constant, Ksp, and calculate its value at 18 C. (b) Calculate the equilibrium concentration of Mg2+ in 1.000 L of saturated MgF2 solution at 18 C to which 0.100 mol of solid KF has been added. The KF dissolves completely. Assume the volume change is negligible. (c) Predict whether a precipitate of MgF2 will form when 100.0 mL of a 3.00103 -M solution of Mg(NO3)2 is mixed with 200.0 mL of a .2.00103 -M solution of NaF at 18 C. Show the calculations to support your prediction.. (d) At 27 C the concentration of Mg2+ in a saturated solution of MgF2 is 1.17103M . Is the dissolving of MgF2 in water all endothermic or an exothermic process? Give an explanation to support your conclusion.
Hydrogen iodide gas decomposes to hydrogen gas and iodine gas: 2HI(g)H2(g)+I2(g)To determine the equilibrium constant of the system, identical one-liter glass bulbs are filled with 3.20 g of HI and maintained at a certain temperature. Each bulb is periodically opened and analyzed for iodine formation by titration with sodium thiosulfate, Na2S2O3. I2(aq)+2S2O32(aq)S4O62(aq)+2 I(aq)It is determined that when equilibrium is reached, 37.0 mL of 0.200 M Na2S2O3 is required to titrate the iodine. What is K at the temperature of the experiment?
. Under what circumstances can we compare the solubilities of two salts by directly comparing the values of their solubility products?
How is the strength of an acid related to the position of its ionization equilibrium? Write the equations for the dissociation (ionization) of HCI, HNO3, and HClO4in water. Since all these acids are strong acids, what does this indicate about the basicity of the Cl-, NO3, and ClO4ions? Are aqueous solutions of NaCl, NaNO3, or NaClO4basic?
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. What is meant by the solubility product for a sparingly soluble salt? Choose a sparingly soluble salt and show how the salt ionizes when dissolved in water, and write the expression for its solubility product.
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