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- One of the possible consequences of climate change is anincrease in the temperature of ocean water. The oceansserve as a “sink” for CO2 by dissolving large amounts of it.(a) The figure below shows the solubility of CO2 in water as a function of temperature. Does CO2 behave more or lesssimilarly to other gases in this respect?(b) What are the implications of this figure for the problemof climate change?A 0.100-L solution is made by dissolving 0.441 g of CaCl21s2 in water. (a) Calculate the osmotic pressure of this solution at 27 °C, assuming that it is completely dissociated into its component ions.When 14.3 g of a certain molecular compound X are dissolved in 85.0 g of benzene C6H6, the freezing point of the solution is measured to be 0.5 °C. Calculate the molar mass of X. molal freezing point depression constant (Kf)°C·kg·mol−1 of benzen is 5.07 If you need any additional information on benzene, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to 2 significant digits.
- 14. Consider two ionic solids, both composed of singly-charged ions, that have different lattice energies. Which solid will be more soluble in water, the one with the larger lattice energy or the one with the smaller lattice energy? Assume that solute- solvent interactions are the same for both solids. (A) The solid with the larger lattice energy, if entropy increases as a result of mixing, and the solid with the smaller lattice energy, if entropy decreases as a result of mixing. (B) The solid with the smaller lattice energy, if entropy increases as a result of mixing, and the solid with the larger lattice energy, if entropy decreases as a result of mixing. (C) The solid with the smaller lattice energy. (D) The solid with the larger lattice energy. (E) They will have the same or very similar solubilities.What are the factors that contributes to the stability of a colloidal system? Why are they important in maintaining the stability of a colloidal system?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.
- 28. (a) Calculate the theoretical lattice energy for the salt CaF2. (b) The hydration enthalpy of Ca²+ is –1592 kJ mol-; the hydration enthalpy of F is -497 kJ mol-. Calculate the enthalpy of precipitation of CaF2. (c) Ignoring entropy effects, use the results of your calculations to predict whether CaF, is soluble or insoluble. Can entropy effects generally safely be ignored in questions like this?The vapor pressure of benzene, C6H6, is 94.6 Torr at 25 °C. A nonvolatile compound was added to 0.300 mol C6H6(l) at 25 °C and the vapor pressure of the benzene in solution decreased to 75.0 Torr. What amount of (in moles) of solute molecules was added to the benzene?The vapor pressure of pure THF at 20 °C is 0.1651 atm. When 10 g of an unknown non-volatile non-dissociating solute A is dissolved in 100 g THF, the vapor pressure of solution at 20 °C is 0.1562 atm. Calculate the mole fraction of solute A in the solution. 0.395 а. 0.946 Ob. 0.824 Oc. 0.054 Od. 0.176 е.
- Calculate the molar solubility in water at 20 °C and the respective partial pressure for:a) Oxygen at 50.0 kPa,b) Carbon dioxide at 500.0 TorrThe mean activity coefficient in an 0.050 molKg-1 LaCl3 (aq) solutions is 0.303 at 25 o C. What is the percentage error in the value predicted by the debye – Huckel limiting law?When 2.60 g of a substance that contains only indium andchlorine is dissolved in 50.0 g of tin(IV) chloride, the normal boiling point of the tin(IV) chloride is raised from 114.1°C to 116.3°C. If Kb = 9.43 K kg mol-1for SnCl4, what are the approximate molar mass and the probablemolecular formula of the solute?