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- Assume that 1.00 mL (1.02 g) of crude product mixture is obtained from the reactionbefore the washing steps, and the distribution constant of the product mixture in brine isK = (Cmixture/Cbrine) = 50.0. Assuming that after mixing the product mixture volume isstill 1.00 mL (i.e., the volume lost is small), and the volume of the first brine wash layeris 2.00 mL. What mass (grams) of product mixture is lost (dissolves) in the first brinewash? (See Technique 13.2, p 53.) Show work.The percent nitrogen (N) in a protein sample can be determined by reacting the protein with sulfuric acid to produce ammonium sulfate. The ammonium sulfate is reacted with concentrated sodium hydroxide to form ammonia gas. The ammonia gas is collected by bubbling it through a known volume of standardized hydrochloric acid solution (all of the ammonia reacts in this step, is consumed). The unreacted hydrochloric acid is then back-titrated with standardized sodium hydroxide solution. The reactions involved are shown below: Protein-N + H2SO4 (aq) ⟶⟶ (NH4)2SO4 (aq) 2 NH4+(aq) + 2 NaOH (aq) 2 NH3 (g) + 2 H2O NH3 (g) + HCl (excess) NH4Cl (aq) + HCl (unreacted) HCl (unreacted) + NaOH (aq) NaCl (aq) + H2OA 1.85 g sample of the protein required 25.00 mL of 0.1535 M HCl and 21.55 mL of 0.0986 M NaOH. How many moles of NH3 were consumed by the standardized HCl? A. 8.55 x 10-4 B. 1.71 x 10-3 C. 2.13 x 10-3 D. 3.84 x 10-3 E. 5.97 x 10-3 What is the mass percent nitrogen in…Sample: Saline 0.900% (m/v), in sodium chloride (NaCl). Data: M.A. (g/mol): Na = 22.9898; K = 39.0983; Cr=51.9961; Ag = 107.8682; Cl = 35.453; N=14.0067; O = 15.9994. Material available in the laboratory's warehouse: Reagents: distilled water; standardized solution of silver nitrate (AgNO₃), at a concentration of 0.09980 mols/L; Potassium chromate solution (K₂CrO₄) 1%; ammoniacal ferric alum solution [Fe(NH₄)(SO₄)₂] and; nitrobenzene (or cooking oil, alternatively); 0.1000 mols/L potassium thiocyanate (KSCN) standard solution. Glassware: beakers of all sizes available on the market; 50, 100, 150, 200 and 250 ml Erlenmeyers; 10.00 and 25.00 mL volumetric pipettes; 15.00 mL burette; 30.00, 50.00 and 100.00 mL volumetric flasks Calculate the molarity of saline, in terms of the NaCl concentration (concentration in mols/L). (a) 0.900 mols/L (b) 5.84 mols/L (c) 0.154 mols/L (d) 0.0154 mols/L
- To determine , by gravimetric analysis, the concentration of barium ions (Ba2+) in a given solution, 25.00cm3 of it are pipetted into a beaker and an excess of dilute sulphuric acid is added to it. The precipitate then obtained (BaSO4) is filtered, dried and weighed. The mass of the precipitate is found to be 1.167g Calculate the concentration of barium ions in the solution? (only 2 decimal places). _________Mol/LThe concentration of arsenic in an insecticide can be determined gravimetrically by precipitating it as MgNH4AsO4. The precipitate is ignited and weighed as Mg2As2O7. Determine the %w/w As2O3 in a 1.627-g sample of insecticide that yields 106.5 mg of Mg2As2O7.State the experimental conditions for the following reactions:
- In the common process for the manufacture of nitric acid, sodium nitrate is treated with aq. sulphuric acid containing 95% H2SO4. In order that the resulting "niter cake" may be fluid; it is desirable to use sufficient acid so that there will be 34% H2SO4 by wt in the final cake. This excess H2SO4 will actually be in combination with the Na2SO4 in the cake, forming NaHSO4, although for purposes of computation it may be assumed to be free acid. The cake will contain 1.5% water and the reaction will go to completion, but 2% of the HNO3 formed will remain in the cake. Assume that the NaNO3 used is dry and pure. Calculate per 100 kg of NaNO3 charged: (a) wt and % composition of the niter cake (b) wt of aqueous acid to be used (c) wt of water vapor and nitric acid distilled from the niter cake.Is it conceivable to have both a limiting and an excess reactant in the presence of a perfect one to one ratio?A student is performing an experiment in the laboratory to determine the oxidation of copper (Cu). Cu reacts with oxygen in the air to formCuO in thefollowing reaction: Cu (s) + O2(g) →CuO (s) The student weighted 1.528gof Cu (s)powderin a crucible and heatedthe sample with a Bunsen burner.Even by using the Cuinpowderform and heating the sample there is unreacted Cu left in the crucible.After heating the student weighted the substance inside the crucible to be 3.647g. 1) If the student weighted 3.647 g of substance in the crucible. Calculate how much of this is unreacted Cu (s) and how much is CuO (s). (Hint: use the balanced chemical equation). 2) Once you know the amount of CuO (s) obtained in this experiment, calculate the percent yieldof CuO in this experiment.
- Federal regulations set an upper limit of 50 parts per million(ppm) of NH3 in the air in a work environment [that is, 50molecules of NH31g2 for every million molecules in the air].Air from a manufacturing operation was drawn through asolution containing 1.00 * 102 mL of 0.0105 M HCl. TheNH3 reacts with HCl according to: NH3(aq) + HCl(aq)-------->NH4Cl(aq) After drawing air through the acid solution for 10.0 min at arate of 10.0 L/min, the acid was titrated. The remaining acidneeded 13.1 mL of 0.0588 M NaOH to reach the equivalencepoint. (a) How many grams of NH3 were drawn into theacid solution? (b) How many ppm of NH3 were in the air?(Air has a density of 1.20 g/L and an average molar mass of29.0 g/mol under the conditions of the experiment.) (c) Isthis manufacturer in compliance with regulations?How is the terms, concentration and dillution related: Represent and quantify chemical reactions at the atomic level?The element carbon undergoes many inorganic reactions, as well as being the basis for the field of organic chemistry. Write balanced chemical equations for the reactions of carbon described below. l type='a'> Carbon burns in an excess of oxygen (for example. in the air) to produce carbon dioxide. If the supply of oxygen is limited, carbon will still burn but will produce carbon monoxide rather than carbon dioxide. molten lithium metal is treated with carbon, lithium car bide, Li2C2 , is produced. i>Iron(II) oxide reacts with carbon above temperatures of about 700 °C to produce carbon monoxide gas and molten elemental iron. i>Carbon reacts with fluorine gas at high temperatures to make carbon tetrafluoride.