You are a lab assistant preparing a solution of known concentration of phosphorus. You have pure trisodium phosphate (Na3PO4) to work with, and you weigh out 0.328 g of the solid and add it to a 1.00 L volumetric flask which is mostly full of DI water; you then fill to the mark with DI water. The volumetric flask thus contains mg/L Na3PO4 solution. O 0.33 O 0.328
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- (a) A commercial 737 jet transporting 143 passengers and 5 crew members from Kansas City (MCI) to Baltimore (BWI) burned 11,800 lb (about 1700 gallons) of Jet A fuel en route. Jet A fuel is kerosine based, consisting primarily of CnH2n+2 hydrocarbons, with n =6 to 16, so the carbon:hydrogen ratio is close to 1:2. During this flight, how much CO2 was released into the atmosphere? Assume the combustion of the fuel was complete, so all the fuel was burned to form CO2 and H2O. Give both the mass of CO2 produced (in kg and in lbs) and the volume it would occupy at 298 K, 1 atm.(b) How much CO2 would be released into the atmosphere if those passengers and crew made the trip instead, in pairs, in hybrid cars at 40 miles per gallon. Assume the density of the gasoline is 0.75 kg L-1 and that carbon and hydrogen dominate the composition in a ratio of 1:2. The road trip is 1082 miles.Dissolve 0.25g NaClI, 0.20g NaHCO3. 0.35g KCI, and 1.5g of glucose in 100 ml distilled water using a 250 mL capacity beaker. Use the formula to create a 60 mL ORS. Based on the given procedure, calculate the total amount of glucose in the prepared solution. (MW: Na: 23, K: 39, CI: 35, H: 1, C: 12, 0: 16) O 83.33 mmol/L 66.91 mmol/L 90.40 mmol/L 71.11 mmol/L O 23.81 mmol/L O 47.30 mmol/Lb) A carbonate of metal X has the formular X,CO3. The carbonate reacts with hydrochloric acid according to the following equation: X,CO3 + 2HC! → 0.25g of X,CO3 was found to neutralize exactly 23.6cm³ of hydrochloric acid of concentration 0.15moldm? ( RAM for C=12;0=16) i) Calculate the number of moles of hydrochloric acid 2XCl + CO2 +H,0 ii) Calculate the number of moles of X,CO3 iii) Calculate the relative molecular mass of X,CO3 iv) Calculate the relative atomic mass of X and hence deduce its identity c) Propanoic acid is a weak acid with an acid dissociation constant of 1.22x 10°moldm i) Write an equation for the ionization of propanoic acid -3 ii) Calculate the pKa for propanoic acid Lo iii) Sodium propanoate is made by the titration using 0.1M sodium hydroxide with propanoic acid A: Write an equation for the reaction B: Name a suitable indicator for this titration iv) A mixture of sodium propanoate and propanoic acid acts as a buffer solution. What is a buffer solution?
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- Heat of Reaction, Mole Fraction 1. A group of students perform a series of experiments mixing HCI with an unknown base of the formula M(OH)n. For each trial the total volume of acid and base was 50.0 mL. The concentration of the acid and base solutions were 0.6000 M. The data is plotted in the graph provided. The density of the aqueous solution is assumed to be 1.00 g/mL and the specific heat of water is 4.18 J/g °C in joules 1600 1400 1200 1000 800 600 400 200 0 0.0000 0.6000 M HCI 0 2000 0.6000 M(OH)x 0 4000 0 6000 Mole Fraction of Acid 0 8000 10000 a) What is the limiting reagent at a mole fraction of 0.6 of acid? b) Write a balanced equation for the reaction of M(OH), with HCI. (You must determine "n") c) For one trial, the students measured a temperature change of + 2.9 °C. Calculate q. d) The students calculated a value of q of 1.5 x 10³ J for one of their trials. For this trial 0.015 mol of HCI and 0.015 mol of M(OH), were used. Calculate heat per mole for this reaction.A sample containing chlorophenol, C6H4ClOH, was analysed by gravimetric analysis. A 0.783-g of this sample goes through a chemical process allowing the chlorine in the chlorophenol to precipitate as silver chloride, weighing 0.271 g. Calculate the % (wt/wt) of the chlorophenol in the sample, assuming that chlorophenol is the only source of chlorine in the sample. Provide your answer to two decimal places and without units. Avoid using scientific notation.TRUE OR FALSE A student synthesizing an organic compound from 2 starting materials. it is determined that starting material X is in excess while starting material Y is the limiting reagent. It is imperative that the measurements of Y are precise in order to determine the correct number of significant figures in the calculation of the theoretical yield Distillation is used in organic chemistry to both purify a compound and determine its approximate boiling point.