Calculate the flux of oxygen between the ocean and the atmosphere, given that: Temp = 18°C Salinity = 35 ppt Density = 1025 kg/m3 Oxygen concentration measured in bulk water = 263.84 mmol/m3 Wind speed = 7.4 m/s Oxygen is observed to be about 10% initially supersaturated
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Calculate the flux of oxygen between the ocean and the atmosphere, given that:
- Temp = 18°C
- Salinity = 35 ppt
- Density = 1025 kg/m3
- Oxygen concentration measured in bulk water = 263.84 mmol/m3
- Wind speed = 7.4 m/s
- Oxygen is observed to be about 10% initially supersaturated
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- If 30.0 mL of water that is 0.0500 M in Q is to be extracted with four 10.0-mL portions of an immiscible organic solvent, what is the minimum distribution coefficient that allows transfer of all but the following percentages of the solute to the organic layer: (a) 1.00 X10-24 (b) 1.00 X10-22A salt solution (30% Na2CO3) weighing 1ton iscooled to 20C where the salt crystallizes asdecahydrate. What will be the crystal yield ifthe solubility is 21.5 kg anhydrous Na2CO3/100kg water? (assume that 3% of the totalsolution is lost by evaporation)The distribution ratio D for an analyte is defined as the ratio of its analytical concentration in two immiscible solvents (organic versus aqueous): D = Corg/Caq Show that the fraction of analyte remained in the aqueous phase after the extraction (from aqueous to organic) is given by the following: Fraction remained = Vaq/(VorgD + Vaq) where Vaq and Vorg are the volume of water and organic solvent used in the extraction, respectively.
- To each digestion flask 200 mL aliquots of 10 different drinking water samples were added. Silver was extracted by a co-precipitation procedure and collected by filtration. The precipitate was digested in 200 μl hot concentrated nitric acid and diluted to 5 mL in a dilute phosphate solution. Standards were prepared according to the following table. The samples were analyzed by graphite furnace AAS. Calculate the concentration of silver in each sample. Are there any problems? How will you address each of the identified problems?Hydroxyapatite, Ca₁0 (PO4) 6 (OH)2, has a solubility constant of Ksp = 2.34 x 10-59, and dissociates according to Ca10 (PO4)(OH)2(s) = 10 Ca²+(aq) + 6 PO¾-¯(aq) + 2 OH(aq) Solid hydroxyapatite is dissolved in water to form a saturated solution. What is the concentration of Ca²+ in this solution if [OH] is fixed at 3.60 × 10-4 M? [Ca2+] = MAllowable recovery from limiting salt calculations Determine the limiting sait and allowable recovery for a brackish water RO system containing the following solutes: calcium 74 mg/L. barium 0.008 mg/L. and sulfate 68 mg/L. Assume 100 percent rejection of all solutes and & polarization factor of 1.15 and ignore activity coeficients (i.e., activity = concentration).
- Ammonium iron(II) sulfate crystals have the following formula: (NH4)2SO4.FeSO4.nH2O . In an experiment to determine n 8.492g of the salt were dissolved and made up to 250cm^-3 of solution with distilled water and sulphuric acid. A 25.0cm^-3 portion of the solution was titrated against 0.0150 mol dm^-3 KMnO4. A volume of 22.5cm^-3 was required. Find the value of nDescribe the challenge of transporting oxygen and carbon dioxide in animals. In particular, discuss the polarity of oxygen and carbon dioxide gas, their consequence on solubility in the aqueous environment, and the inadequacy of passive diffusion in transporting these gases into cells and tissues.An impure sample of calcium carbonate with a mass of 7.95 g was reacted with 50.00 cm3 of 1.00 mol dm hydrochloric acid (an excess). The resulling solution was transferred to a volumetric flask and titrated with 11.10cm3 of 0.300 mol dm-3 sodium hydroxide solution. Determine the percentage purity by mass of the calcium carbonate sample.CaCO3 + HCl -> CaCl2 + H2O + CO2 HCl + NaOH -> NaCl +H2O a. Determine how many moles of hydrochloric acid were used.b. Determine how many moles of excess HCI was titratedc. Determine how much in moles calcium carbonate present in the sample.d. Calculate the mass of calcium carbonate presente. Determine the percentwge calcium carbonate is in the sample.
- The complete ionic composition of natural waters often is not known, aquatic chemists have developed equations to estimate ionic strength (/) from readily available information such as electrical conductivity (e.g., specific conductance (SC) in µS/cm) or total dissolved solids (TDS): /= 1.6 × 10-5 × SC (for 1 <0.06); / = 1.3 × 10-5 × SC (for 1 < 0.5) /= 2.5 x 10-5 × TDS; TDS ≈ b × SC (b= 0.55-0.70) Your field measurement of a stream sample gave a specific conductance of 100 µS/cm, and your analysis of the water gave concentrations of Na+, Ca²+, Cl-, and HCO3 of 9, 21, 6, and 45 mg/L, respectively. Are these measurements consistent?Using the Kf and Kb equations with electrolytesThe %purity of a powdered crude sample of Na2CO3 containing only inert impurities is to be determined by reacting 225.0 mg of the crude sample to 10.0 mL of 3.00 M HCl solution, and bubbling the resulting CO2(g) product in water that is at exactly 29 °C. After the reaction has completed, the level of the liquid inside the eudiometer rests 4.30 cm above the water level in the beaker. The graduation on the eudiometer indicates that the trapped gas is 44.37 mL. The experiment was done under a barometric pressure of 755.2 torr. a. How many moles of CO2 were collected? b. What is the percent purity of the sample? Round off to the nearest whole number