2) Analysis of dissolved Ni in solution may be accomplished by complexation with DMG (dimethylglyoxime) via:.Ni²+ (aq) + 2 DMG (aq) ---------> Ni(DMG)2(s)red precipitate(Ni(DMG)2=288.91 g/mol)Excess DMG was added to 25.00 mL of a Ni²+ solution and produced 0.145 g Ni(DMG)2. What is the [Ni2+] in the originalsolution?

Given:Mass of Ni(DMG)2 = 0.145 g (3 significant figures)Volume of Ni2+ solution…

Answered: 2) Analysis of dissolved Ni in solution…

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter27: Relative Stabilities Of Complex Ions And Precipitates Prepared From Solutions Of Copper(ii)

Section: Chapter Questions

Problem 1ASA

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V15.
1. (Total 20 pts) Calculate a predominance diagram showing the solubility of Spertiniite - a rare Cu(II) hydroxide mineral, Cu(OH)2(s) - as a function of pH by plotting the logarithm of the concentration of each copper species against pH assuming the solution is in contact with Spertiniite. Consider only the following aqueous species: Cu²+; CuOH+; Cu(OH)2; Cu(OH)3. A. Write the reactions that form the aqueous species from Cu(OH)2(s) and the corresponding equilibrium relations. The equilibrium constants for the formation of the 4 aqueous species listed above are 108.68; K₂ = 100.98; K3 = 10–5; K4 = 10-18.2. (10 pt) B. Write the mass balance equation for the solution. (3 pt) C. Plot the total concentration of the dissolved species in a predominance diagram and indicate on the diagram the regions where the solution is oversaturated and undersaturated with Cu(II). Hint: The diagram can be drawn by hand. (7 pt) K₁ =
8.00mL aqueous suspension of elemental selenium is treated with 24.00mL ammonia 0.045M AgNO3 The reaction is as follows: 6Ag (NH3) 2 ++ 3Se (s) + 3H2O → 2Ag2Se (s) + Ag2SeO3 (s) + 6NH4 + After this reaction is completed, nitric acid is added to dissolve Ag2SeO3. However, Ag2Se does not dissolve during this time. Ag + consisting of dissolved Ag2SeO3 and the excess of the reagent requires 13.43mL 0.01294M KSCN in a Volhard titration. How many milligrams of Se are in each milliliter of sample? (Se = 78.96g / mol)
A 100-mL sulfide-containing water sample was titrated with 12.15 mL of 0.041 M AgNO3 to determine its S²- content. The titration resulted to the formation of Ag2S precipitate. Calculate the concentration of sulfides in ppm H₂S. (MW (g/mol): AgNO3=169.9; S=32.1; Ag2S=247.8; H₂S-34.1) Express your answer with 2 decimal places and do not encode the units.
a) What mass of Fe(NH4)2(SO4)2•2H2O(s) is required to prepare a 500 mL solution containing 100 ppm (m:v) in Fe? b) Using this stock solution, what aliquot must be used to prepare calibration solutions, 100 mL volume, of the following concentrations: 0.100 ppm, 0.500 ppm, 2.00 ppm, 4.00 ppm, and 7.00 ppm.
112. Solutions of sodium thiosulfate are used to dissolve unexposed AgBr (Kp and-white film. What mass of AgBr can dissolve in 1.00 L of 0.500 M Na,S,O;? Ag* reacts with S,O,- to form a complex ion: = 5.0 × 10-13) in the developing process for black- Ag*(aq) + 2S,O;²-(aq) = Ag(S,O;),-(aq) K = 2.9 X 1013
Directions: Solve the problem with a complete step-by-step solution. A 100.0-mL sample of brackish water was made ammoniacal, and the sulfide it contained was titrated with 16.47 mL of 0.02310 M AgNO3. The analytical reaction is 2Ag+ + S2- ---> Ag2S (s)Calculate the concentration of H2S in the water in parts per million, cppm.
76. Solutions of sodium thiosulfate are used to dissolve unexposed AgBr (ksp=5.0x10^-13) in the developing process for black-and-white film. What mass of AgBr can dissolve in 1L of .5M Na₂S₂O3? Ag+ reacts with S₂O3 2- to form a complex ion: Ag +(aq) + 2S₂O3 2-(aq) ← Ag (S₂O3)2 3- (aq) K=2.9x10^13
I got 0.626. That was incorrect. How much potassium oxalate can be added to 156.0 mL of 0.5 M [Cu(NH3)4]Cl2 before a precipitate of CuC2O4 begins to form? Ksp(CuC2O4)=2.9x10-8 and Kf(Cu(NH3)42+)=1.1x1012 Include 3 significant figures
The value of Ksp for Cd(OH)2 is 2.5 x 10-14. (a) Whatis the molar solubility of Cd1OH22? (b) The solubilityof Cd(OH)2can be increased through formation of thecomplex ion CdBr42 - (Kf = 5 x 103). If solid Cd(OH)2 isadded to a NaBr solution, what is the initial concentrationof NaBr needed to increase the molar solubility of Cd(OH)2to 1.0 x 10-3 mol/L?
A ferrous sulfate (BP) [FeSO4151.9g/mol] sample was analysed by titration using ammonium cerium (IV) nitrate (NH4)2Ce(NO3)6. The result shown 0.4980g of this sample used 25.50 ml 0.110M ammonium cerium (IV) nitrate. The BP specifies that ferrous sulfate material should contain not less than 86.0% and not more than 90.0% of FeSO4 Does the sample comply with the British Pharmacopoeia specification? A. The sample contains 85.6% ferrous sulfate thus does not comply with the British Pharmacopoeia specification B. The sample contains 85.6% ferrous sulfate thus complies with the British Pharmacopoeia specification C. The sample contains 86.0% ferrous sulfate thus complies with the British Pharmacopoeia specification D. The sample contains 89.0% ferrous sulfate thus complies with the British Pharmacopoeia specification E. The sample contains116.9% ferrous sulfate thus does not comply with the British Pharmacopoeia specification How do you work this out ?
How much potassium oxalate can be added to 156.0 mL of 0.5 M [Cu(NH3)4]Cl2 before a precipitate of CuC2O4 begins to form? Ksp(CuC2O4)=2.9x10-8 and Kf(Cu(NH3)42+)=1.1x1012Include at least 3 significant figures in your answer.

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