ofh too mees us faranos 240+ 200+ 160+ 120- KND CuSO, SH,0 10 20 30 40 50 60 70 80 90 100 Temperature in "C Figure 1: Solubility as a function of temperature for KNO3 and CuSO4'5 H₂O
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- If 124.4 mL of water is shaken with oxygen gas at 0.81atm, it will dissolve 0.0036 g O2. Estimate the Henry's law constant for the oxygen gas in water in units of g mL ^-1atm^-1.Some water dissolves in liquid methane at -161°C to givea solution in which the mole fraction of water is 6.0 × 10-5. Determine the mass of water dissolved in 1.00 L ofthis solution if the density of the solution is 0.78 g cm-3.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
- The table below shows temperature/composition data collected for a mixture of methylbenzene (M) and octane (O) at 1 atm. Recall that x stands for the mole fraction in the liquid and y stands for the mole fraction in the vapor in equilibrium. The boiling points for methylbenzene (M) and octane (O) are 110.60C and 125.60C, respectively. Construct the phase diagram with Temperature vs. xM. What is the composition of the vapor in equilibrium with the liquid of composition (a) xM = 0.250 and (b) xO = 0.250. T (0C) 110.9 112.0 114.0 115.8 117.3 119.0 121.1 123.0 xM 0.908 0.795 0.615 0.527 0.408 0.300 0.203 0.097 yM 0.923 0.836 0.698 0.624 0.527 0.410 0.297 0.164In benzene, dimerization occurs with benzene due to hydrogen bonding. In 110 g of benzene, 1.70g of acetic acid is dissolved that increases the boiling point by 0.40 oC. What is the expected degree of association of acetic acid? (Use Kb=2.57 Kg mol-1 )?Example: Calculation the weight of barium iodate Ba(IO3)2 if it dissolved in 500mL of distilled water (D.W) at 25 °C if M.wt of ppt = 487 g/mole and %3D Ksp= 1.57x10.
- Asample of 2.05 g of polystyrene of uniform polymer chain length was dissolved in enough toluene to form 0.100 Lofsolution. The osmotic pressure of this solution was found to be 1.21 kPa at 25°C. Calculate the molar mass of thepolystyrene.a) 2.35 x 104 g/molb) 4.20x 105 g/molc) 3.05 105 g/mold) 4.20x 103 g/mole) 4.20 x 104 g/molYou 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 of solution (in °C to one decimal place) Freezing point of solution (in °C to two decimal places) Vapor pressure of the solution (in atm to three decimal places) Osmotic pressure (in atm to three decimal places)Osmotic pressures are often reported in units of atmospheres or mm Hg. The latter impliesthat the height of a column of liquid can be used as a measure of pressure. This is, in fact, thebasis of the torricellian barometer from which the units of “torr” come. The pressure, P, isrelated to the height of the column by:P = ρghwhere ρ is the density of the liquid, g is the acceleration due to gravity and h is the height. Whatwill be the height (in mm) of a column of aqueous solution with a density of 0.9987 g/mL, if theosmotic pressure of the solution at 25 °C is 1.4 mm Hg? The density of mercury at thistemperature is 13.8 g/mL
- Suppose that a solution made from an unknown solute dissolved in solvent X. Its molality is 0.0125 and it boils 0.047oC higher than solvent X's boiling point. With the use of valid approximations, calculate the osmotic pressure of the said solution at 60oC? The following are useful thermodynamic data for solvent X to solve the problem: ΔSvap=87.92 J*K-1mol-1 Tb=61.15oC density at 60oC=1.394 g/cm3If 102.6 mL of water is shaken with oxygen gas at 1.8 atm, it will dissolve 0.0034 g O2. Estimate the Henry's law constant for the oxygen gas in water in units of g mL-1atm-1.Consider the following two white solids below and their physical properties based on information gathered from the Merck Index: Camphor: melting point=179C; boiling point = 209C; sublimes (under vacuum); the solubility of camphor at 25C is listed as follows: to dissolve 1g of camphor: 800mL of ethanol; 1mL of ether. (Note: ethanol is miscible with water and with ether; ether is mot miscible with water). Cinnamic acid: melting point= 134C; heating above 146C causes the molecule to chemically change; the solubility of cinnamic acid at 25C is listed as follows: to dissolve 1g of cinnamic acid: 2,000mL of water; 6mLof ethanol; fully soluble in ether. based on the information above, would either of the following two methods be suitable to seperate camphor from cinnamic acid? explain your answer. a. Sublimination b. Distillation c. Treating a 2g mixture with 30mL of ethanol to selectively dissolve camphor and leaving cinamic acid behind.