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Calculate the % KHP of the 1.294-g sample which consumed 48.25 mL in 0.09605 N NaOH solution in titration. (MW KHP = 204.22)
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- Calculate the Gibbs free energy of the reaction from mixing 50 mL each of 0.50 M Ag+(aq) solution and 1 M of NaCl(aq) to form AgCl(s) at 25°. The Ksp of AgCl is 6.0 × 10—11 at 25 °C.Describe in detail the steps involved to prepare following solution; a) 0.2% (v/v) , (v/w), (w/v) and (w/w) solution of acetic acid.what is the purpose of preparing of a standard sodium hydroxide solution in determination of purity of impure KHP?
- . At 250C, Ksp for AgBr is 5.0 x 10-13. Calculate the solubility of AgBr in g/L at 25 oC (a) in pure water; (b) In the presence of 0.2 mol L−1 NaBr solutionAt 25oC, Ksp for AgBr is 5.0 x 10-3 g. Calculate the solubility of AgBr in g L-1 at 25oC a) in pure water b) in the presence of 0.2mol L-1 NaBr solutionCalculate the Gibbs free energy of the reaction from mixing 50 mL each of 0.50 M AgNO3(aq) solution and 1 M of NaCl(aq) to form AgCl(s) at 25°. The Ksp of AgCl is 6.0 × 10—11 at 25 °C.
- Calculate the potential of the solution in the titration of 50.0 mL 0.100 M Fe2+ in 1.00 M HClO4 with 0.0167 M Cr2O72- at 10.00 mL titrant added.Calculate the solubility and molar solubility of Cu3(PO4)2 (MW=380.58 ; Ksp=1.4x10-37).The solubility of Fe(OH)2 is measured and found to be 1.15×10-3 g/L. Use this information to calculate a Ksp value for iron(II) hydroxide.
- Calculate the % relative error in solubility by using concentrations instead of activitiesfor Fe(OH)2 in 0.0500 M KNO3 (give the source for thermodynamic solubility).2) If 25g of NaCl is dissolved into a final volume of 500mL, what is the percent (w/v) concentration of NaCl in the solution? 3) How will you prepare 200mL of 0.3M NaCl prepared? Include a short instruction in the preparation. 4) From a stock solution of 1M Tris solution, how will you prepare 400mL of 0.2M? Do not forget to include a short instruction in the preparation.A piece of Gold weighing 12,359 Kg is suspected of being contaminated with Iron. To perform an instrumental analysis and To confirm whether or not it contains Fe, a portion of the sample (0.954 g) is taken from the piece and dissolved with 25 mL of aqua regia. Heats up For its complete dissolution, it is cooled and made up to 100 mL. A 10 mL aliquot is taken from this solution and made up to 50 mL. From This last solution is given the appropriate treatment to visualize Fe+2, for which the 1,10-phenanthroline reagent is added. (it forms a complex that is red in color) and is taken to a visible spectrophotometer and with a 12 mm cell a absorbance of 0.45. Previously, a calibration curve of Fe+2 was obtained under the same instrumental conditions obtaining the following data: (view table) Calculate the purity of the gold piece, assuming impurities only due to Fe.