Bottle Concentration of No Oxalic acid, N N initial N final 1 1 0.23 2 1 0.22 3 1 0.17 4 1 0.13 5 1 0.1 a C Weight of oxalic acid adsorbed (g/60ml) (X) Weight of activated carbon, g (m) 1 1 1 1 1 x/m Log(x/m) Log c
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- A sample may contain any combination of sodium hydroxide, sodium carbonate and sodium bicarbonate with inert matter. A 3.00g sample requires 57.57ml of 0.5N hydrochloric acid to reach phenolphthalein endpoint and a total of 105.4ml of acid was used until the methyl orange endpoint was reached. What is the percentage inerts in the mixture? What is the percentage sodium bicarbonate in the mixture? What is the percentage sodium hydroxide in the mixture? What is the percentage sodium carbonate in the mixture?An aqueous waste stream that has a maximum concentrationof 0.50 M H₂SO₄ (d=1.030 g/mL at 25C) will be neutralized by controlled addition of 40% caustic soda (NaOH; d=1.430 g/L) before it goes to the process sewer and then to the chemical plant waste treatment facility. However, a safety re-view finds that the waste stream could meet a small stream of animmiscible organic compound, which could form a flammable vapor in air at 40.°C. The maximum temperature of the causticsoda and the waste stream is 31°C. Could the temperature in-crease due to the heat of neutralization cause the vapor to ex-plode? Assume the specific heat capacity of each solution is 4.184 J/gK.Q3 / The solubility of sodium chloride NaCl in water at 290 Kis 35.8 kg / 100 kg of water. Express the solubility as the following: 1. Mass fraction and the mass percent of Naci 2. Mole fraction and mole percent of NaCl 3. kmol of NaCl per 1000 kg of water Note: molecular weight of NaCl = 135.8, and water = 18.016
- Study the tabulated data during an gravimetric analysis of BaSO4 experiment Trial T1 T2 T3 Mass of sample (g) 1.0040 1.0100 1.0050 Constant weight of empty crucible (g) 10.2453 10.2454 10.2454 Constant weight after ignition (g) 10.3253 10.3252 10.3253 1. Calculate the mean mass of precipitate as BaSO4 a. 0.0799 g b. 0.0800 c. 0.08 g 2. Calculate the mean weight of sulphate (MM BaSO4 = 233.39 g/mol, So42- = 176 g/mol)? a. 0.0603 g b. 0.06 g c. 0.06025 g 3. Calculate the mean % SO42- in the sample a. 6.00% b. 5.991% c. 5.9908%A 100-liter empty jar was spiked with 20 mg of TCE (C2HCl3) under room temperature condition. The jar was then closed tightly. What is the concentration (in atm.) of TCE in the air at 25 C? (TCE: MW: 131.4 g/mol; TCE solubility in water (Cs) = 1100 mg/L; Pv (pure liquid at 25oC) = 10^-1.01 atm. KH = 10^1.03 L atm mol-1; KOW = 102.42). if the jar was half filled with water and half filled with air, what were the concentrations of TCE in both air and water at 25C?Which of the following statements is INCORRECT? A. greater the density, faster particle sediments in centrifugal force. B. greater the mass, faster particle sediments in centrifugal force. C. greater the frictional coefficient, faster particle sediments in centrifugal force. D. All the choices are correct
- (a) One particular pungent gas is the toxic hydrogen sulphide (H2S). Hydrogen sulphide develops an odour of rotten eggs at a partial pressure of 0.13 ppm or 0.0132 Pa. If the aqueous concentration of hydrogen sulphide in the stream is 2.5 x 10–6 M, determine through calculations if the hydrogen sulphide in the water may be responsible for the odour detected near the vicinity of the stream. KH (H2S) = 0.087 M/atm) (b) In the leachate pond the conditions are more acidic causing NH3 to exist as NH4+. NH4+ can react with nitrites in the pond to form the less hazardous N2 and H2O as seen below: NH4+ + NO2– → N2 + 2H2O You want to investigate methods of speeding up this reaction but you first conducted an initial rates test to determine the rate law equation for the reaction. Using the data in the table below determine the rate law equation for the reaction above. Experiment Number Initial NH4+ M Initial NO2– Initial Rate (M/s) 1 0.0100 0.200 5.4 x 10 –7…Boiling Point Elevation/Freezing Point Depression T = m K where, for freezing point depression: T = T(pure solvent) - T(solution) and for boiling point elevation: T = T(solution) - T(pure solvent) m = (# moles solute / Kg solvent) Kb = boiling point elevation constant. Kf = freezing point depression constant. Kb and Kf depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow. Solvent Formula Kb(°C / m) Kf(°C / m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02A spent 1.0 percent caustic soda solution (ρNaOH = 8.42 lb/gal) with a volumetric flow rate of 3.0gpm is to be neutralized using either sulfuric acid or hydrochloric acid. First, determine the massflow rate (lb/day) of NaOH in the spent caustic soda solution, and then use that value todetermine the stoichiometric amounts (lb/day) of:1. H2SO4 required for neutralizing the OH− ions contributed by the spent caustic soda.[Hints: (1) write the balanced chemical equation for the acid-base reaction betweenNaOH and H2SO4, and use it to establish the stoichiometric weight ratio H2SO4 : NaOH.]2. HCl required for neutralizing the OH− ions contributed by the spent caustic soda. [Hints:(1) write the balanced chemical equation for the acid-base reaction between NaOH andHCl and use it to establish the stoichiometric weight ratio HCl : NaOH.]
- what is the correct volume of 2.5M PhMgBr in THF is needed to completely react with 1.5ml of methyl benzoate?you do not need to consider and excess and should calculate (and choose) the minimum amount as required by the reaction stoichiometry Enter your answer to one decimal place with the proper unit of measurement.The following evidence was obtained from an experiment to determine the solubility of calcium chloride at room temperature. A sample of saturated calcium chloride solution was evaporated to dryness, and the mass of solid residue was measured.EvidenceVolume of solution (mL) = 15.0Mass of empty beaker (g) = 90.54Mass of beaker and residue (g) = 101.36The solubility of calcium chloride is g/100 mLthe dimensionless Henry's law constant for trichloroethylene at 25 degrees Celcius is 0.4. A sealed glass vial is prepared that has an air volume of 4ml overlying an aqueous volume of 36ml. TCE is added to the aqueous phase so that initially it has an aqueous-phase concentration of 100 ppb. After the system equilibrates, what will be the concentration (in units of microgram per liter) of TCE in the aqueous phase