being analysed. bservations: he initial solution of acetic acid (HC₂H₂O₂) is clear and colourless. A few drops of nenolphthalein indicator are added to each sample. A dilute solution of sodium hydroxide concentration 2.50 x 104 mol/L) is used as the titrant. As the mixture reaches the endpoint, ashes of pink colour are seen and the titrant is added drop by drop. The endpoint is eached when one drop of titrant turns the mixture a pale pink colour that does not fade. 2 3 Trial Volume of acetic acid (HC₂H₂O₂) (mL) 10.00 10.00 10.00 Initial burette reading (mL) 0.00 24.27 48.55 Final burette reading (mL) 24.27 48.55 72.81
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- Use the following experimental titration data to calculate the concentration of the acid being analysed. Observations: The initial solution of acetic acid (HC2H3O2) is clear and colourless. A few drops of phenolphthalein indicator are added to each sample. A dilute solution of sodium hydroxide (concentration 2.50 x 10-4 mol/L) is used as the titrant. As the mixture reaches the endpoint, flashes of pink colour are seen and the titrant is added drop by drop. The endpoint is reached when one drop of titrant turns the mixture a pale pink colour that does not fade.To determine the fluoride content in an aqueous and chloride-containing preparation of ammonium fluoride, the following analysis was performed. 105.2 mg of the preparation was dissolved in 100.0 mL of water. Then a 300 mL 40 mM lead chloride solution was added, whereby all fluoride ions were precipitated out of the solution in the form of the sparingly soluble salt PbClF (s). The precipitate was separated and washed at 15 degrees with a lead fluoride chloride saturated solution and dried at 130 degrees. The precipitate weighed 651.3 mg. a) Calculate the fluoride content (as % by weight F) in the preparation.b) Determine the purity of the ammonium fluoride preparation(TOPIC: Gravimetry multi-component analysis) A 0.8612-g sample of a mixture of sodium bromide, sodium iodide, and sodium nitrate is analyzed by adding silver nitrate and precipitating a 1.0186-g mixture of silver bromide and silver iodide. The precipitate is then heated in a stream of chlorine gas, which converts it to 0.7125 g of silver chloride. Calculate the %w/w nitrate in the sample.
- 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.The dissociation vapour pressure (the pressure of gaseous products in equilibrium with the solid reactant) of NH4CI at 427 °C is 608 kPa but at 459 °C it has risen to 1115 kPa. Calculate (a) the equilibrium constant. (b) the standard reaction Gibbs energy, (c) the standard enthalpy, (d) the standardentropy of dissociation, all at 427 °C. Assume that the vapour behaves as a perfect gas and that ΔHΘ and ΔSΘ are independent of temperature in the range given.In an experiment the equilibrium between ethanol, acetic acid, ethyl acetate, and water is studied, and the reaction is catalyzed by the addition of hydrochloric acid. Following mixtures were prepared and titrated with 0.953M NaOH solution to calculate equilibrium constant of the reaction. Mixture 1. 2.5ml 3M HCl+ 2.5ml Water Mixture 2. 2.5mL 3M HCl + 2ml Ethyl Acetate + 0.5ml Acetic Acid End points were reached at 6.68 ml and 24.36 ml, respectively. Calculate the equilibrium constant using mole fractions for the reaction (MWHCl: 36.46g/mol, MWCH3COOH: 60.05g/mol, MWH2O: 18.02g/mol, MWCH3COOC2H5: 88.11g/mol, ρwater = ρHCl =0.998g/ml, ρCH3COOH = 1.05g/ml, ρCH3COC2H5 =0.902g/ml)
- From information in the Resource section, calculate the standard Gibbs energy and the equilibrium constant at (i) 25 °C and (ii) 50 °C for the reaction CH4(g) + 3 Cl2(g) ⇋ CHCl3(l) + 3 HCl(g). Assume that the standard reaction enthalpy is independent of temperature. At 298.15 K ΔfG⦵ (CHCl3(l)) = −73.7 kJ mol−1 and ΔfH⦵ (CHCl3(l)) = −134.1 kJ mol−1.A saturated solution of magnesium hydroxide is prepared and the excess solid magneisum hydorixed is allowed to settle. A 25.0 mL aliquot of the saturated solution is withdrawn and transfered to a flask, two drops of inficator are added. A 0.00053 M HCL is dispensed from a buret into a solution. The solution changes color after the addition of 13.2 mL. What is the Ksp of magnesium hydroxide?The precipitation of Al(OH)3 (Ksp = 1.3 x 10-33) is sometimesused to purify water. (a) Estimate the pH at whichprecipitation of Al(OH)3 will begin if 5.0 lb of Al2(SO4)3is added to 2000 gal of water. (b) Approximately howmany pounds of CaO must be added to the water toachieve this pH?
- Calculate the solubility and molar solubility of Cu3(PO4)2 (MW=380.58 ; Ksp=1.4x10-37).Chitinase is a protein that breaks down chitin, a primary component of the cell wall in fungi, scales in fish and exoskeletons of arthropods. The activity of chitinase extracted from a plant was shown to be optimum at pH 5. You were tasked to prepare 300 mL of 150 mM buffer solution for further analysis of the extracted chitinase. REAGENTS Ka 2.5M Acetic acid Solid NaOAc•3H2O [136.08g/mol] 1.76 x 10-5 2.5M NH3 Solid NH4Cl [53.49g/mol] 5.6 x 10-10 2.5M Lactic acid Solid sodium lactate [112.06g/mol] 4.0 x 10-5 5 M HCl 5M NaOH What are the moles of the (1) acid and (2) base components, given the following reagents? What is the mass/volume of the components needed to prepare the buffer solution?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.