A method for the analysis of Ca2+ in water suffers from an interference in the presence of Zn2+. When the concentration of Ca2+ is 100 times greater than that of Zn2+, an analysis for Ca2+ gives a relative error of +0.5%. What is the selectivity coefficient for this method?
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A method for the analysis of Ca2+ in water suffers from an interference in the presence of Zn2+. When the concentration of Ca2+ is 100 times greater than that of Zn2+, an analysis for Ca2+ gives a relative error of +0.5%. What is the selectivity coefficient for this method?
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- Mixing the chelating reagent B with Ni(II) forms the highly colored NiB22+, whose solutions obey Beer’s lawat 395 nm overa wide range. Provided the analytical concentration of the chelating reagent exceeds that of Ni(II) by a factor of 5 (or more), the cation exists, within the limits of observation, entirely in the form of the complex. Use the accompanying data to evaluate the formation constant Kf for the process Ni2++2BNiB22+(Standard addition) Tooth enamel consists mainly of the mineral calcium hydroxyapatite, Ca10(PO4)6(OH)2. Trace elements in teeth of archeological specimen provide anthropologists with clues about diet and diseases of ancient people. Student at Dankook University measured the trace element strontium (Sr) in enamel from extracted wisdom teeth by atomic absorption spectroscopy. Solutions were prepared with a constant total volume of 10 mL containing 0.750 mg dissolved tooth enamel plus variable concentrations of added standard Sr. Added Standard Sr (ng/mL=ppb) 0 2.50 5.00 7.50 10.00 Emission Signal 28.0 34.3 42.8 51.5 58.6 (a) Make a graph showing the experimental data and the calculated straight line. (b) Find the concentration of Sr in the tooth ennamel in parts per million = μg/mL.Commercial Vanadyl Sulfate (VOSO4) is contaminated with H2SO4 and H2O. A solution was prepared dissolving 0.2447 g of impure VOSO4 in 50.00 mL of water. A spectrophotometric analysis indicated that the The concentration of vanadyl ions, VO2+ (blue) was 0.0243 M. A 5.00 mL sample was passed through a column filled with a cation exchange resin in H+ form, to retain the vanadyl ion and the eluent necessary for its titration 13.03 mL of NaOH 0.02274 M. Calculate the percentage by weight of each component (VOSO4, H2SO4, and H2O) in commercial vanadyl sulfate. (Pm VOSO4, 162.96; H2SO4, 97.94)
- Discuss the advantages, disadvantages, and limitations of the technique of cyclic voltammetry in both qualitative and quantitative measurements.The following data were obtained from the spectrophotometric titration of Cu(II) and Ca(II) in an unknown solution. A 25.00 mL aliquot of the unknown was taken to which 50.0 mL of ethanolamine buffer and 25.0 mL of distilled water were added. The solution was then titrated with standard 0.2508 M EDTA solution. Plot the recorded data, absorbance against volume of EDTA in mL. Correct the absorbance for volume changes. Calculate the number of moles of Ca(II) and Cu(II) in the unknown sample. Vol of Titrant, mL Vol of Titrant, mL Abs Abs 0.0 0.416 12.5 0.886 2.0 0.415 13.0 0.923 4.0 0.409 13.5 0.958 6.0 0.416 14.0 0.979 8.0 0.535 14.5 0.969 10.0 0.690 15.0 0.971 11.0 0.770 15.5 0.964 12.0 0.840For a solution in which μ = 7.0 x 10-2, calculate K'sp for a. AgSCN (Ksp (AgSCN) = 1.1 × 10-¹2, Ag+ = 0.25, ascN = 0.35) K's = sp b. Pbl₂ (Ksp (PbI2) = 7.9 x 10-9, apb²+ = 0.45, ar = 0.3) K'sp = c. La(103) 3 (Ksp (La(103) 3) = 1.0 x 10-¹¹, L²+ = 0.9, 10,- = 0.35) K'sp =
- Use the Debye-Hückel equation to calculate the activity coefficient (y) for each of the ions at the given ionic strength (μ) at 25 °C. Refer to the table for the ion size (a). SCN when = 0.278 M y = So when μ = 0.363 M Y = Ion Ca²+, Sn²+ Ba2+ SO² OH, SCN CN Rb+ Ion size (a, pm) 600 500 400 350 300 250The ionization constant (Ka ) equation of a monoportic weak, HA, acid is given by ca2 K, = (1-0) The use of conductivity meter to test a 0.106 M solution of this weak acid gives a specific conductance, K, 20.24 uS.cm-1. What would be the pKa, ( -long Ka), of the acid, if its limiting molar ionic conductivities are A+ = 243 and A. = 74 S.cm2 mol-1? OA 4.41 O B.6.00 OC.5.53 OD.3.12 OE.3,62Frankie determined the trendline for their Calibration Curve for the relationship between Absorbance and [FeSCN2+] was y = 3823.3 x − 0.0127 During Part B, Frankie measured the absorbance of Equilibrium Solution 3 as 0.292 a.u. (absorbance units). Question 1: What is the equilibrium concentration of the [FeSCN2+]? Anjelica used the absorbance of 0.449 a.u. to determine the equilibrium concentration of [FeSCN2+] for Run 5 was 1.17 x 10-4 M. Previously, Anjelica calculated the initial concentrations of [Fe3+] = 1.00 x 10-3 M and [SCN-] = 1.00 x 10-3 M. Question 2: What are the equilibrium concentrations of [Fe3+] and [SCN-]? Please answer completely all questions will give rating surely
- Exactly 6.00 ml of acetic acid (density = 1.05 g/mL), MW =60.05) was added to a 1 –liter volumetric flask, and the flask was filled to the mark with distilled water. A portion of the resulting solution was added to a conductance cell (k = 1.25 cm-1), and the conductance was found to be 416 μS. Calculate the dissociation constant Ka of acetic acid. ΛoH+= 349.8 Scm2/mole and ΛoCH3COO- = 41 Scm2/moleA student attempts to identify six solutions that contained either hydrogen peroxide (H202), calcium chloride, calcium acetate, lithium acetate, lithium hydroxide, or lithium permanganate. The tests performed were conductivity, solution colour, flame colour, and the addition of lead(II) nitrate solution. The following evidence was collected: Flame Solution Addition of Conductivity Solution Colour Colour РЬ NO3)2(ag) yellow- White precipitate yes colourless red forms hydrogen peroxide calcium chloride No precipitate yes red purple calcium acetate forms lithium acetate lithium hydroxide No precipitate none colourless lithium permanganate none forms White precipitate yes red colourless forms No precipitate yes red colourless forms No precipitate forms yellow- yes colourless redComplexometric titrations are generally conducted to determine divalent cations. The most important applications are the titration of calcium and magnesium with EDTA. (a) A supplement tablet containing about 300.00 mg of calcium ion was dissolved, filtered, and diluted to 100.00 ml volume. Several 2.00 ml samples of the total solution were titrated with 0.0100 M EDTA solution. The mean corrected titration volume was 13.65 mL. Calculate the calcium content of the supplement tablet in mg units. (b) A sample of Epsom Salt of mass 0.7567 g was dissolved uniformly in distilled water in a 250.00 mL volumetric flask. Portions of the magnesium ion solution of volume 10.00 mL were titrated using a 0.01000 M solution of EDTA. The mean corrected titration volume was 12.25 ml. Calculate the percentage by mass (% w / w) of the magnesium in the Epsom Salt sample. (c) A 100.00 mL sample of tap water was titrated with 0.0100 M EDTA solution. The mean corrected titration volume was 14.80 mL. Determine…
