CHEM:ATOM FOC 2E CL (TEXT)
2nd Edition
ISBN: 9780393284218
Author: Stacey Lowery Bretz, Natalie Foster, Thomas R. Gilbert, Rein V. Kirss
Publisher: WW Norton & Co
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CHEM:ATOM FOC 2E CL (TEXT)
Ch. 11 - Prob. 11.1VPCh. 11 - Prob. 11.2VPCh. 11 - Prob. 11.3VPCh. 11 - Prob. 11.4VPCh. 11 - Prob. 11.5VPCh. 11 - Prob. 11.6VPCh. 11 - Prob. 11.7VPCh. 11 - Prob. 11.8VPCh. 11 - Prob. 11.9VPCh. 11 - Prob. 11.10VP
Ch. 11 - Prob. 11.11QACh. 11 - Prob. 11.12QACh. 11 - Prob. 11.13QACh. 11 - Prob. 11.14QACh. 11 - Prob. 11.15QACh. 11 - Prob. 11.16QACh. 11 - Prob. 11.17QACh. 11 - Prob. 11.18QACh. 11 - Prob. 11.19QACh. 11 - Prob. 11.20QACh. 11 - Prob. 11.21QACh. 11 - Prob. 11.22QACh. 11 - Prob. 11.23QACh. 11 - Prob. 11.24QACh. 11 - Prob. 11.25QACh. 11 - Prob. 11.26QACh. 11 - Prob. 11.27QACh. 11 - Prob. 11.28QACh. 11 - Prob. 11.29QACh. 11 - Prob. 11.30QACh. 11 - Prob. 11.31QACh. 11 - Prob. 11.32QACh. 11 - Prob. 11.33QACh. 11 - Prob. 11.34QACh. 11 - Prob. 11.35QACh. 11 - Prob. 11.36QACh. 11 - Prob. 11.37QACh. 11 - Prob. 11.38QACh. 11 - Prob. 11.39QACh. 11 - Prob. 11.40QACh. 11 - Prob. 11.41QACh. 11 - Prob. 11.42QACh. 11 - Prob. 11.43QACh. 11 - Prob. 11.44QACh. 11 - Prob. 11.45QACh. 11 - Prob. 11.46QACh. 11 - Prob. 11.47QACh. 11 - Prob. 11.48QACh. 11 - Prob. 11.49QACh. 11 - Prob. 11.50QACh. 11 - Prob. 11.51QACh. 11 - Prob. 11.52QACh. 11 - Prob. 11.53QACh. 11 - Prob. 11.54QACh. 11 - Prob. 11.55QACh. 11 - Prob. 11.56QACh. 11 - Prob. 11.57QACh. 11 - Prob. 11.58QACh. 11 - Prob. 11.59QACh. 11 - Prob. 11.60QACh. 11 - Prob. 11.61QACh. 11 - Prob. 11.62QACh. 11 - Prob. 11.63QACh. 11 - Prob. 11.64QACh. 11 - Prob. 11.65QACh. 11 - Prob. 11.66QACh. 11 - Prob. 11.67QACh. 11 - Prob. 11.68QACh. 11 - Prob. 11.69QACh. 11 - Prob. 11.70QACh. 11 - Prob. 11.71QACh. 11 - Prob. 11.72QACh. 11 - Prob. 11.73QACh. 11 - Prob. 11.74QACh. 11 - Prob. 11.75QACh. 11 - Prob. 11.76QACh. 11 - Prob. 11.77QACh. 11 - Prob. 11.78QACh. 11 - Prob. 11.79QACh. 11 - Prob. 11.80QACh. 11 - Prob. 11.81QACh. 11 - Prob. 11.82QACh. 11 - Prob. 11.83QACh. 11 - Prob. 11.84QACh. 11 - Prob. 11.85QACh. 11 - Prob. 11.86QACh. 11 - Prob. 11.87QACh. 11 - Prob. 11.88QACh. 11 - Prob. 11.89QACh. 11 - Prob. 11.90QACh. 11 - Prob. 11.91QACh. 11 - Prob. 11.92QACh. 11 - Prob. 11.93QACh. 11 - Prob. 11.94QACh. 11 - Prob. 11.95QACh. 11 - Prob. 11.96QA
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- The freezing point of a 0.21 m aqueous solution of H2SO4 is -0.796C. (a) What is i? (b) Is the solution made up primarily of (i) H2SO4 molecules only? (ii) H+ and HSO4- ions? (iii) 2H+ and 1SO42- ions?arrow_forward6-111 As noted in Section 6-8C, the amount of external pressure that must be applied to a more concentrated solution to stop the passage of solvent molecules across a semipermeable membrane is known as the osmotic pressure The osmotic pressure obeys a law similar in form to the ideal gas law (discussed in Section 5-4), where Substituting for pressure and solving for osmotic pressures gives the following equation: RT MRT, where M is the concentration or molarity of the solution. (a) Determine the osmotic pressure at 25°C of a 0.0020 M sucrose (C12H22O11) solution. (b) Seawater contains 3.4 g of salts for every liter of solution. Assuming the solute consists entirely of NaCl (and complete dissociation of the NaCI salt), calculate the osmotic pressure of seawater at 25°C. (c) The average osmotic pressure of blood is 7.7 atm at 25°C. What concentration of glucose (C6H12O6) will be isotonic with blood? (d) Lysozyme is an enzyme that breaks bacterial cell walls. A solution containing 0.150 g of this enzyme in 210. mL of solution has an osmotic pressure of 0.953 torr at 25°C. What is the molar mass of lysozyme? (e) The osmotic pressure of an aqueous solution of a certain protein was measured in order to determine the protein's molar mass. The solution contained 3.50 mg of protein dissolved in sufficient water to form 5.00 mL of solution. The osmotic pressure of the solution at 25°C was found to be 1.54 torr. Calculate the molar mass of the protein.arrow_forward6-20 Give a familiar example of solutions of each of these types: (a) Liquid in liquid (b) Solid in liquid (c) Gas in liquid (d) Gas in gasarrow_forward
- For each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Ammonia gas in water with P = 1 atm and T = 50C Ammonia gas in water with P = 1 atm and T = 90C b. Carbon dioxide gas in water with P = 2 atm and T = 50C Carbon dioxide gas in water with P = 1 atm and T = 50C c. Table salt in water with P = 1 atm and T = 60C Table salt in water with P = 1 atm and T = 50C d. Table sugar in water with P = 2 atm and T = 40C Table sugar in water with P = 1 atm and T = 70Carrow_forwardWhat is the freezing point and normal boiling point of a solution made by adding 39 mL of acetone, C3H6O, to 225 mL of water? The densities of acetone and water are 0.790 g/cm3 and 1.00 g/cm3, respectively.arrow_forwardCalculate the molality of a solution made by dissolving 115.0 g ethylene glycol, HOCH2CH2OH, in 500. mL water. The density of water at this temperature is 0.978 g/mL. Calculate the molarity of the solution.arrow_forward
- For each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Oxygen gas in water with P = 1 atm and T = 10C Oxygen gas in water with P = 1 atm and T = 20C b. Nitrogen gas in water with P = 2 atm and T = 50C Nitrogen gas in water with P = 1 atm and T = 70C c. Table salt in water with P = 1 atm and T = 40C Table salt in water with P = 1 atm and T = 70C d. Table sugar in water with P = 3 atm and T = 30C Table sugar in water with P = 1 atm and T = 80Carrow_forwardWhat would be the freezing point of a solution formed by adding 1.0 mole of glucose (a molecular compound) to the following amounts of water? a. 250 g (0.25 kg) b. 500 g (0.500 kg) c. 1000 g (1.000 kg) d. 2000 g (2.000 kg)arrow_forwardWhat is the freezing point of a solution of dibromobenzene, C6H4Br2, in 0.250 kg of benzene, if the solution boils at 83.5 C?arrow_forward
- A 1.00 mol/kg aqueous sulfuric acid solution, H2SO4,freezes at 4.04 C. Calculate i, the vant Hoff factor,for sulfuric acid in this solution.arrow_forward6-67 Calculate the freezing points of solutions made by dissolving 1.00 mole of each of the following ionic solutes in 1000. g of H2O. (a) NaCI (b) MgCI2 (c) (NH4)2CO3 (d) AI(HCO3)3arrow_forward6-113 List the following aqueous solutions in order of decreasing freezing point: 0.040 M glycerin (C3H8O3) 0.025 M NaBr, and 0.015 M AI(NO3)3 Assume complete dissociation of any salts.arrow_forward
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Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY