Suppose that you use 0.75 g of iron in this experiment. What is the minimum volume of 1.5 M CuSO4 solution required a) using eq. (5-1)? Fe(s) + Cu2+(aq) -> Fe2+(aq) + Cu(s) b) using eq. (5-2)? 2Fe(s) + 3Cu2+(aq) -> 2Fe3+(aq) + 3Cu(s)
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Suppose that you use 0.75 g of iron in this experiment. What is the minimum volume of 1.5 M CuSO4 solution required
a) using eq. (5-1)? Fe(s) + Cu2+(aq) -> Fe2+(aq) + Cu(s)
b) using eq. (5-2)? 2Fe(s) + 3Cu2+(aq) -> 2Fe3+(aq) + 3Cu(s)
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- 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 =The concentration of H2S in wastewater samples was determined by coulometric titration using Kl as mediator and I3 as "titrant". H2S(as) + 13 (ag) + 2H2Ou) --> 2H3O*(aq) + 31 (ag) + S(s) A 50 ml wastewater sample was placed in a coulometric cell, added with excess Kl and starch indicator. Electrolysis was carried out at a constant current of 84.6 mA for 386 s to reach the end point of the titration. What is the concentration of H2S in the sample (in ppm)?1. Calculate a predominance diagram showing the solubility of Ferric hydroxide [Fe(OH)3(s)] as a function of solution pH by plotting the logarithm of the concentration of each iron species against pH assuming the solution is in contact with ferric hydroxide mineral. (10 pts) Before beginning, answer these questions: i) Is this solution open or closed with respect to iron? (2 pts) ii) If open, what is the reservoir for iron? (2 pts) 2. Now plot the same diagram showing the logarithm of iron species concentration as a function of pH for a solution in equilibrium with Ferric hydroxide but that also contains 0.001 moles/kg of dissolved fluoride. Fluoride can form iron complexes via this reaction: FeF+2(aq) + 3 H₂O(1) = Fe(OH)3(s) + 3 H*(aq) + F¯(aq) Include this latter species FeF+2(aq) in the diagram. Ignore all other Fe-F complexes. (16 pts)
- 2+ as (6) A sample of an ore was analyzed for Cu* follows. A 1.25 g sample of the ore was dissolved in acid and diluted to volume in a 250 mL volumetric flask. A 20 mL portion of the resulting solution was transferred by pipet to a 50 ml volumetric flask and diluted to volume. An analysis showed that the concentration of 2+ Cu* in the final solution was 4.62 ppm. What is the weight percent of Cu in the original ore?A 22.41 mL of NaOH solution is required to reach the phenolphthalein endpoint in the standardization with 0.276 g of solid, monoprotic primary standard acid (MW 128.33) in a 25.00 mL solution. 12.34 mLof the same NaOH solution was added to titrate 5 mL of vinegar solution to the endpoint. Calculate the mass of acetic acid in this vinegar solution (d = 1.005 g/mL).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
- A water sample was analyzed for Fe content using the iron- phenanthroline method. The following data were obtained from the analysis: Reagent Blank Absorbance Absorbance (au) Reagent Blank Absorbance 0.003 Concentration of Stock Solution: 10 ppm Volume of Stock Solution (mL) Total Volume of Standard Solution Concentration of Standard Solution (ppm) Absorbance (au) (mL) 0.50 10.00 0.012 1.00 10.00 0.132 2.00 10.00 0.267 3.00 10.00 0.349 4.00 10.00 0.428 5.00 10.00 0.560 Volume of Unknown Solution Total Volume of Unknown Solution Trial Absorbance (au) (mL) (mL) 1 5.00 10.00 0.289 2 5.00 10.00 0.296 3 5.00 10.00 0.281 Determine the value of the slope (m), y-intercept (b), and the coefficient of determination (r²) A m = 0.1128; b = -4.0 x 10-5; r2 = 0.9880 B m = 0.1128; b = -4.0 x 10-5; r² = 0.9762 C) m = 0.1128; b = -3.0 x 10-³; r² = 0.9880 D m = 0.1128; b = -3.0 x 10-³; r² = 0.9762Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Volume of bleach titrated. 1ml Mass of commercial bleaching solution titrated ?Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Moles of OCl– in the diluted bleach titrated. ?
- Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Volume of bleach titrated. 1ml Mass of NaOCl in commercial bleach titrated. ?Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Mass of NaOCl in the diluted bleach titrated. ?The concentration of ammonia in a cleaning product was determined by back titration.Firstly, 10.00 cm3 of the cleaning product was pipetted into a large conical flask,containing 250.00cm3 of 0.50 mol/l HCl to give Solution A.Following a period of reaction and shaking, 50.00cm3 of Solution A was removed anddiluted to 250 cm3 with water in a volumetric flask to give Solution B.20 cm3 samples of Solution B were titrated against 0.05 mol/l Na2CO3 solution, givingan average titre of 12.45 cm3. i) Write equations for the reactions that have taken place.ii) Determine the concentration of NH3 in the original cleaning product in mol/l,g/l, ppm, and % w/v.