Arrange the following compounds in order of increasing solubility in water: O2, LiCl, Br2, CH3OH (methanol).

The Henry's Law constant of methyl bromide, CH3Br, is k = 0.159 mol/(L atm) at 25°C. What is the solubility of this compound in water at 25°C and at a partial pressure of 406 mmHg?

5.152g of Na2CO3(s) is added to 75.0mL of water at 21.20°C. When the dissolution is complete, the final temperature of the solution is measured at 25.00°C. The final volume of the solution is 75.8mL, and the density of water at 21.20°C is 0.99798g/mL. Identify the strongest intermolecular force present in Na2CO3(s): and in water:

The Henry's law constant (kH) for O2 in water at 20 °C is 1.28 × 10^-3 mol Be sure each of your answer entries has the correct number of significant figures. How many grams of O, will dissolve in 5.75 L of H2O that is in contact with pure O2 at 1.40 atm? How many grams of O2 will dissolve in 5.75 L of HO that is in contact with air where the partial pressure of 02 is 0.299 atm?

A sample of 3.929 g of polystyrene was dissolved in toluene and diluted to a total volume of 100.8 mL. The osmotic pressure of this solution at 25.0°C was 44.56 torr. What is the molar mass?

Calculate the freezing point of a solution containing 74.0 g of eucalyptol (C10H8O) solute dissolved in 0.600 kg of CHCl3.  The freezing point of pure CHCl3 is -63.5 oC.  CHCl3 has a Kf of 4.68 oC/molality. -64.9 oC -67.5 oC -48.3 oC -58.0 oC -69.0 oC -62.1 oC -59.5 oC -78.7 oC

(a) Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide. CaCl₂(s) Cal₂(s) Lattice Energy -2247 kJ/mol -2059 kJ/mol * Explain. ΔΗ soln -46 kJ/mol -104 kJ/mol *Lattice energy is defined as the energy change for the process M*(g) + X¯(g) → MX(s). calcium chloride 2201 calcium iodide 1955 XkJ/mol X kJ/mol (b) Based on your answers to part (a), which ion, CI or I, is more strongly attracted to water? chloride iodide The enthalpy of hydration for CaCl₂ is more exothermic than for Cal2. Any differences must be due to differences in hydrations between CI and I¯.

At a certain temperature the vapor pressure of pure chloroform (CHC13) is measured to be 0.20 atm. Suppose a solution is prepared by mixing 92.3 g of chloroform and 96.5 g of acetyl bromide (CH₂COBr). Calculate the partial pressure of chloroform vapor above this solution. Be sure your answer has the correct number of significant digits. Note for advanced students: you may assume the solution is ideal. atm x10

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You must mix 168 g of carbon disulfide (CS2, 76.13 g/mol) with acetonitrile (CH3CN, 41.06 g/mol) to create a solution that has a total vapor pressure of 292 torr at 25°C. Calculate the number of grams of CH3CN required. Substance Vapor Pressure at 25°C (torr) Carbon disulfide 357 Acetonitrile 89.5