A foot powder sample containing Zn was dissolved on 50.00 mL water and was titrated to the end point color with 22.57 mL of 0.01639 M EDTA at pH=4. (α= 3.61x109, KKzny2 = 3.2 x 1016). The pZn in the sample is:
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A foot powder sample containing Zn was dissolved on 50.00 mL water and was titrated to the end point color with 22.57 mL of 0.01639 M EDTA at pH=4. (α= 3.61x109, KKzny2 = 3.2 x 1016). The pZn in the sample is:
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- A cyanide solution with a volume of 12.99 ml was treated with 30.00 ml. of Ni" solution (containing excess Nit) to convert the cyanide into tetracyanonickelate(): 4 CN + Ni?+ Ni(CN) The excess Nit was then titrated with 11.96 ml. of 0.01357 M ethylenediaminetetraacetic acid (EDTA): Nit + EDTA Ni(EDTA)- Ni(CN) does not react with EDTA. If 39.40 ml. of EDTA were required to react with 30.65 ml. of the original Nit solution, calculate the molarity of CN in the 12.99 mL cyanide sample. 0.12055 (CN = IncorvectSolutions of cobalt (II) ions have a magenta color with a molar absorptivity constant (e) value at 511 nm of 5.87 M-1cm-1. A 0.500 mL sample is transferred from a 50.0 mL stock solution of Co(NO3)2 and diluted with water to a final volume of 7.50 mL. The dilution had an absorbance value at 511 nm in a standard cuvette (1.00 cm light path) of 0.382. Calculate the mass of Co(NO3)2 contained in the original 50.0 mL stock solution.A 0.937-g sample containing Ca²+ was dissolved to produce a 500-mL stock solution. A 50-mL aliquot was then obtained and titrated with 0.029 M EDTA. A volume of 23.15 mL was required to reach the endpoint. Calculate the amount of calcium (in %CaCO3) in the sample. (MW (g/mol): EDTA=292.24; CaCO3 = 100; Ca=40) Express your answer with 2 decimal places and do not encode the units.
- The total concentration of Ca²+ and Mg²+ in a sample of hard water was determined by titrating a 0.100-L sample of the water with a solution of EDTA. The EDTA chelates the two cations: Mg+ + [EDTA]+ Ca2+ + [EDTA]+ [Mg(EDTA)]²- [Ca(EDTA)]?- It requires 31.5 ml. of 0.0104 M[EDTA]* solution to reach the end point in the titration. A second 0.100-L sample was then treated with sulfate ion to precipitate Ca?+ as calcium sulfate. The Mg2+ was then titrated with 18.7 mL of 0.0104 M [EDTA]*. Calculate the concentrations of Mg²+ and Ca2 in the hard water in mg/L.5. (1) (ii) Ibuprofen (206.3 g/mol) absorbs at 255 nm and shows a molar absorptivity of 3010 L/mol.cm. A tablet of ibuprofen, 0.6654 g, was ground and 0.2203 g powder was dissolved in 20% methanol in a 100 mL volumetric flask (Solution A). Exactly 5.0 mL of Solution A was diluted in a 50.0 mL flask and the resulting solution showed an absorbance of 0.1228 AU in a 1.00 cm cell. (i) What is the concentration (mol/L) of ibuprofen in the 100 mL stock solution? (ii) Report the amount of ibuprofen in mg/Tablet. Ibuprofen H3C | HCCH; 1 H3C CH3 -CH-COOH(7 What is the value of pMg for 50.0 ml of a 0.0500 M Mg*2 solution buffered at pH l10.00 and titrated with 0.0500 m EDTA when 51.0 mL of EDTA is added (Kf = 6.2x108) (ay4. = 0.30 )? 1. O2.88 2. 04.94 3. 06.57 4. 01.39 5. 07.96
- A 25.0025.00 mL solution of 0.033000.03300 M Na2CO3Na2CO3 is titrated with 0.026300.02630 M Ba(NO3)2Ba(NO3)2. Calculate pBa2+pBa2+ following the addition of the given volumes of Ba(NO3)2Ba(NO3)2. The KspKsp for BaCO3BaCO3 is 5.0×10−95.0×10−9.A 0.6006-g sample of Ni/Cu condenser tubing was dissolved in acid and diluted to 100 mL in a volumetric flask. Titration of both ions in a 25.0ml aliquot of this solution required 45.81 mL of 0.052285M EDTA. Mercaptoacetic acid and NH3 were then introduced; production of the Cu complex with the former resulted in the release of an equivalent amount of EDTA, which required 22.85ml titration with 0.07238M Mg2+. Calculate the %Ni (59.693 g/mol) in the alloy.A foot powder sample containing Zn was dissolved on 50.00 ml water and was titrated to the end point color with 22.57 mL of 0,01639 M EDTA at pH=D4. (a4=3,61×10, KZNY = 3.2 x 10") The pzn in the sample is Please fill in the space with a numerical value with two digits or two decimal places without units
- For a solution in which µ = 6.5 × 10-2, calculate K'sp for a. AgSCN (Ksp (AgSCN) = 1.1 x 10-¹2, KSP b. PbI2 = = a Ag = -9 ², αpb²+ = 0.45, al- = 0.3) (Ksp (PbI₂) = 7.9 × 10¯ KSP c. La(IO3)3 -11 (Ksp (La(103)3) = 1.0 × 10¯ KSP = = 0.25, ascN- = 0.35) , αLa³+ 3+ =0.9, α103- - = 0.35) =A foot powder sample containing Zn was dissolved on 50.00 ml water and was titrated to the end point color with 22.57 mL of 0.01639 M EDTA at pH=4. (a4= 3.61x10-9, KZNY2- = 3.2 x 1016). The pZn in the sample is: Please fill in the space with a numerical value with two digits or two decimal places without units Answer:In the titration of MgSO4.nH2O (2g per litre) against a 0.01 M solution of the disodium salt of ethylenediamine tetraacetic acid (EDTA) the titres obtained were as follows ; titre 1: start - 0.7 ml and end - 13.3 ml (12.6ml) titre 2: start - 13.3 ml and end 25.7 ml (12.4ml) Q. Calculate the value of n