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The solubility of N2 in water at 25°C and an
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- The following table lists the concentrations of the principal ions in seawater: (a) Calculate the freezing point of seawater. (b) Calculate the osmotic pressure of seawater at 25 C. What is the minimum pressure needed to purify seawater by reverse osmosis?arrow_forwardA sample of water contains 0.010 ppm lead ions, Pb2+. (a) Calculate the mass of lead ions per liter in this solution.(Assume the density of the water solution is 1.0 g/mL.) (b) Calculate the mass fraction of lead in ppb.arrow_forwardRefer to Figure 13.10 ( Sec. 13-4b) to determine whether these situations would result in an unsaturated, saturated, or supersaturated solution. 120. g RbCl is added to 100. g H2O at 50 °C. 30. g KCl is dissolved in 100. g H2O at 70 °C. 20. g NaCl is dissolved in 50. g H2O at 60 °C. Figure 13.10 Solubility of ionic compounds versus temperature.arrow_forward
- Sodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride (CaCl2) is sometimes used for this purpose too. Let us compare the effectiveness of equal masses of these two compounds in lowering the freezing point of water, by calculating the freezing point depression of solutions containing 200. g of each salt in 1.00 kg of water. (An advantage of CaCl2 is that it acts more quickly because it is hygroscopic, that is. it absorbs moisture from the air to give a solution and begin the process. A disadvantage is that this compound is more costly.)arrow_forwardIn Exercise 96 in Chapter 8, the pressure of CO2 in a bottle of sparkling wine was calculated assuming that the CO2 was insoluble in water. This was a bad assumption. Redo this problem by assuming that CO2 obeys Henry s law. Use the data given in that problem to calculate the partial pressure of CO2 in the gas phase and the solubility of CO2 in the wine at 25C. The Henrys law constant for CO2 is 3.1 w2 mol/L atm at 25C with Henrys law in the form C = kP, where C is the concentration of the gas in mol/L.arrow_forwardList the following aqueous solutions in order of increasing melting point. (The last three are all assumed to dissociate completely into ions in water.) (a) 0.1 m sugar (b) 0.1 m NaCl (c) 0.08 m CaCl2 (d) 0.04 m Na2SO4arrow_forward
- The dispersed phase of a certain colloidal dispersion consists of spheres of diameter 1.0 102 nm. (a) What are the volume (V=43r2) and surface area (A = r2) of each sphere? (b) How many spheres are required to give a total volume of 1.0 cm3? What is the total surface area of these spheres in square meters?arrow_forwardThe Henry's law constant for the solubility of argon gas in water is 1.0103M/atm at 30C. (a) Express the constant in M/mm Hg. (b) If the partial pressure of argon gas at 30C is 693 mm Hg, what is the concentration (in M) of the dissolved argon gas at 30C? (c) How many grams of argon gas can be dissolved in 29 L of water at 693 mm Hg and 30C? (Ignore the partial pressure of water.)arrow_forwardTable sugar (C12H22O11) or urea [(NH2)2CO] can be used by road crews to melt ice on roads, but solutions of CaCl2 are generally used instead. Assuming equal costs per pound of substance, why is CaCl2 used instead of table sugar or urea?arrow_forward
- A carbonated beverage is made by saturating water with carbon dioxide at 0C and a pressure of 3.0 atm. The bottle is then opened at room temperature (25C), and comes to equilibrium with air in the room containing CO2(PCO2=1.0103M/atm). The Henry's law constant for the solubility of CO2 in water is 0.0769 M/atm at 0C and 0.0313 M/atm at 25C. (a) What is the concentration of carbon dioxide in the bottle before it is opened? (b) What is the concentration of carbon dioxide in the bottle after it has been opened and come to equilibrium with the air?arrow_forwardConsider three test tubes. Tube A has pure water. Tube B has an aqueous 1.0 m solution of ethanol, C2H5OH. Tube C has an aqueous 1.0 m solution of NaCl. Which of the following statements are true? (Assume that for these solutions 1.0m=1.0M.) (a) The vapor pressure of the solvent over tube A is greater than the solvent pressure over tube B. (b) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube A. (c) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube C. (d) The boiling point of the solution in tube B is higher than the boiling point of the solution in tube C. (e) The osmotic pressure of the solution in tube B is greater than the osmotic pressure of the solution in tube C.arrow_forwardDimethylglyoxime [DMG, (CH3CNOH)2] is used as a reagent to precipitate nickel ion. Assume that 53.0 g of DMC has been dissolved in 525 g of ethanol (C2H5OH). s The red, insoluble compound formed between nickel(II)ion and dimethylglyoxime (DMG) is precipitated when DMG is added to a bask solution of Ni2+ (aq). (a) What is the mole fraction of DMG? (b) What is the molality of the solution? (c) What is the vapor pressure of the ethanol over the solution at ethanols normal boiling point of 78.4 C? (d) What is the boiling point of the solution? (DMG does not produce ions in solution.) (Kbp for ethanol = +1.22 C/m)arrow_forward
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