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PS5.1. Describe all the energy changes which must be considered in the solution process. Indicate the types of interactions which are important in the solution process and discuss what conditions favor and do not favor formation of a solution. PS5.2. Which substance of each of the following pairs is likely to be more soluble in water? Explain each choice and, for the substance of each pair that is less soluble in water, suggest a better solvent. Include Lewis structures for each of the substances. (NOTE: If you have vitamins as an option you do not have to draw the structure of vitamin E.) a) nitrogen(g) and ammonia(g) b) methylamine(g) and carbon disulfide(l) c) vitamin B6(s) or vitamin E(s) NOTE: See page 565 in your textbook. d) phenol(s) or toluene(l) PS5.3. Describe the attractive forces present when NaCl(s), NH3(g) and methanol(l) dissolve in water. Use the space below to sketch diagrams depicting at the atomic level how each of the three substances interact with water molecules. Drawing: Drawing:Drawing: Explanation: Explanation: Explanation: PS5.5. A concentrated solution of sucrose, C12H22O11, contains 185.6 g dissolved in 316.02 g water. The density of the solution is 1.1507 g mL-1 Calculate; a) the weight percent C12H22O11 in the solution; b) the mol fraction of C12H22O11 in the solution; c) molality of C12H22O11 in the solution; d) the molarity of C12H22O11 in the solution PS5.6. Describe how you would prepare the following aqueous solutions; a) 100 mL of a 0.399 M Mg(NO3)2 solution b) 527 g of a 36.93 % (by weight) solution of NaOH. c) 410.6 g (grams of solution) of a 2.26 molal NaCl solution PS5.7. An aqueous solution of sulfuric acid is 1.26 molal and has a density of 1.6864 g mL-1. Calculate the a) weight percent sulfuric acid; b) mol fraction of sulfuric acid; c) the molarity of sulfuric acid. PS5.8. A solution of glycerol, C3H8O3, in water is prepared by mixing 345.1 g C3H8O3 with 1749 g of water. The molarity was found to be 1.846 M. Calculate a) the molality of the glycerol solution b) the density of the glycerol solution PS5.9. A solution of a compound called potassium acid phthlate, is prepared by dissolving 2.43 g in 250 mLs of water. This solution is then reacted with exactly 14.39 mLs of a 0.827 M NaOH solution. Assume KHP reacts in a one-to-one ratio with NaOH, calculate the molar mass of KHP (potassium acid phthlate).
The initial volume of the balloon is 5.00 , and the pressure is 760. The balloon ascends to an altitude of 20, where the pressure is 76.0 and the temperature is 50. What is the new volume, of the balloon in liters, assuming it doesn't break or leak
Calculate the atom economy for each method for preparing 2,3-dibromo-3-phenylpropanioc acid.
Calculate the total volume of gas (at 133 degrees C and 758 mmHg) produced by the complete decomposition of 1.56 kg of ammonium nitrate.
What is the work done in terms of the system?
what is the molar mass of a gaseous element that Effuses through an opening of a box 1.12 times as fast as argon at the same temperature.
1.9 kJ f heat is added to a slug of rhodium and a separate 1.9 kJ of heat is added toa slug of zinc. The heat capacity of the rhodium slug is 318 J/ degree C while the heat capacity of the zinc slug is 996 J/ degree C.
Develop an argument based on bond enthalpies for the importance of SiO bonds in substances common in the Earth's crust in preference to SiSi or SiH bonds
The dissolution of ammonium nitrate occurs spontaneosly in water 25 degrees celcius. As NH4NO3 dissolves, the temperature of the water decreases. What are the signs of Delta H, Delta S, and Delta G for this process
A volume of 40.0 mL of iron (II) sulfate is oxidized to iron (III) by 20.0 mL of 0.100 M potassium dichromate solution. What is the concentration of the iron (II) sulfate solution
A) aqueous naoh and ch3ch2co2h B) aqeous naoh and c6h5so3h c) ch3ch2Li in hexane and ethyne d) ch3ch2Li in hexane and ethyl alcohol
For the H2PO4- -HPO4-2 bufer system, pka=7.21. If the pH of a urine sample is 5.6 and its total phosphate concentration is 46.6mmol/L, calculate the concentration of each phosphate species in the sample.
Which of the changes listed will shift the equilibrium to the right for the following reversible reaction. CO(g) +H2O(g) (arrow points to the left and right) CO2(g) + H2(g) + heat
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