The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25°C. How many grams of DDT, C14H,Cls, a nonvolatile, nonelectrolyte (MW= 354.5 g/mol), must be added to 266.0 grams of diethyl ether to reduce the vapor pressure to 458.42 mm Hg ? diethyl ether = CH;CH,0CH,CH3 = 74.12 g/mol. g DDT
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- Mass of empty dish: 38.386 grams Volume of 0.0400 M stock solution: 5.00 mL Mass of Dish and 0.0400 M stock solution: 44.751 grams Mass of Dish and CuSO4 (after evaporation): 38.468 grams 1. Calculate the density of the solution a)Calculate the percent by mass, CuSO4, in stock solution (100 x g CuSO4/g solution) b)Calculate the molality of the stock solution (mole CuSO4 / kg solvent) c) Calculate the molarity of the stock solution (moles CuSO4 / L solution)The Safe Drinking Water Act (SDWA) sets a limit for mercury-a toxin to the central nervous system-at 0.002 ppmppm by mass. Water suppliers must periodically test their water to ensure that mercury levels do not exceed this limit. Suppose water becomes contaminated with mercury at twice the legal limit (0.004 ppmppm). How much of this water would have to be consumed for someone to ingest 43 mgmg of mercury?The presence of the radioactive gas radon (Rn) in well waterpresents a possible health hazard in parts of the UnitedStates. (a) Assuming that the solubility of radon in waterwith 1 atm pressure of the gas over the water at 30 °C is7.27 x 10-3 M, what is the Henry’s law constant for radon in water at this temperature? (b) A sample consisting ofvarious gases contains 3.5 x 10-6 mole fraction of radon.This gas at a total pressure of 32 atm is shaken with waterat 30 °C. Calculate the molar concentration of radon in thewater.
- Ascorbic acid 1vitamin C, C6H8O62 is a water-soluble vitamin.A solution containing 80.5 g of ascorbic acid dissolvedin 210 g of water has a density of 1.22 g>mL at 55 °C. Calculate(a) the mass percentage, (b) the mole fraction, (c) themolality, (d) the molarity of ascorbic acid in this solution.The vapor pressure of diethyl ether (ether) is 463.6 mm Hg at 25 °C. How many grams of chlorophyll , C55H72MgN4O5, a nonvolatile, nonelectrolyte (MW = 893.5 g/mol), must be added to 268.0 grams of diethyl ether to reduce the vapor pressure to 457.6 mm Hg ?diethyl ether = CH3CH2OCH2CH3 = 74.12 g/mol.Answer: _____ g chlorophyllEstimate the molality (mol/kg) of oxygen in water at 25 °C and given that the partial pressure of O2 is 21 kPa near sea level (1 atm). (b) What would the solubility of oxygen be in water [O2] in (mmol/L)? (c) What is the solubility of [O2] in (mg/L) at that temperature? Henry’s constant for oxygen gas KO2 = 7.9 x 104 kPa kg mol-1.
- Two organic solvents (A and B) form an ideal solution when they mixed at 25 °C. The vaporpressures of A and B solvents at 25 °C are 500 and 180 mmHg, respectively. By mixing 30 mLof A (d=0.64 g/mL) with 48 mL B (d=0.67 g/mL), an ideal solution is prepared.(a) What is the vapor pressure of resulting ideal solution?(b) What is the composition by mole fraction of A in the vapor that is in equilibrium withthis solution? (Mw of A= 72.15 g/mol; Mw of B= 86.17 g/mol)What mass (in kg) of ethylene glycol would be needed to add to 5.0 kg of water to raise the boiling point of water by 2.0 oC? Assuming, Kbp H2O = +0.5121 oC/m and Kfp H2O = -1.86 oC/m.You are handed a 15.85% by mass aqueous KCl (m.m. = 74.5513 g mol–1) solution (at 25 °C). Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the following: Boiling Point in degrees Celcius
- In 100 g of pure benzene whose freezing and boiling temperatures are 5.5 100C and 80.1 C respectively, 24.4 g biphenyl (C12H10) is dissolved. Since the cryoscopy and ebulioscopy constants of benzene are 5.12 K.kg/mol and 2.63 K.kg/mol respectively; Find the vapor pressure of the solution at 80.1ᴼC, the freezing and boiling temperatures of benzene in the solution. (MAbenzene = 78 g / mol; MAbiphenyl = 154 g / mol; 1atm = 760 mmHg)Seawater contains about 3.5% by mass dis- solved solids. As a rough approximation, assume that the dissolved solids are predominantly NaCl(aq) [that is, 3.5 grams of NaCl(aq) in 96.5 grams of H2O(l )] and estimate the normal boiling point of seawater.You are handed a 15.85% by mass aqueous KCl (m.m. = 74.5513 g mol–1) solution (at 25 °C). Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the following: Vapor pressure of the solution in atm