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1. Colligative properties of solutions are physical properties which depend on the total number, but not the identity, of solute particles, in the solution. The presence of different solute particles results in vapor pressure lowering, boiling 12. Calculate the molality of benzoic acid in each solution. point clevation, freezing point depression, and osmotic pressure of a solvent. 2. The freezing point depression (T))is the difference in Tf berween pure solvent and solution (solvent + solute): 1379molalmolalmolalmolalmolal2468molalmolalmolalmolal Tf=Tf FUxesocvent Tf socimon Show the work for solution 6 . 3. Tf depends on the solute particle molality where Kr is the freezing point depression constant of a solvent, and the dissociation factor i is the relative number of particles each solute unit dissociates into in a particular solution: Tf=iKf molality soume 4. For lauric acid Kf=3.9C/m, and for lauric acid and benzoic acid i=1. 13. Clean the thermometer probe thoroughly with a paper towel 5. Molality is a measure of concentration that is independent of wet with acetone. Use the same thermometer for all trials. temperature, commonly written as moles solute / kg solvent: 14. Prepare a hot water bath with 300mL of tap water in a 600 molality soume =n soturn /m socvmr (in mol kg 1 units) mL beaker heated on a hot plate to 95C100C. Solutions 7 - 10 require heating in an oven set at 120C. 6. The solute molar mass is the ratio of its mass to its amount: 15. Measure the melting/freezing temperature of each solution Msocuts= mass soturt / n soute (repeating steps 16 - 19). 7. Combining the molality and molar mass equations gives: 16. Remove the rubber stopper and place the test tube in the hot Msocute= mass souvt / (molality socute mass socvest ) water bath. Handle the test tubes with a clamp. When the 8. solution is fully melted insert the clean thermometer probe 8. The accepted melting points and molar masses are: into the solution. Remove the test tube from the hot water lauric acid (LA): TM=43.2CM=200.32gmot1 bath. Make sure that only liquid, and no solids, are present. benzoic acid (BA): TM=122.4CM=122.12gmol1 17. Cool the liquid in air while stirring with the thernometer. 9. The objectives of the experiment are: Hold the test tube near the top lip so that you can see all the Measurethefreezingpointsofpurelauricacidandofsolutionsofbenzoicacidandlauricacid.sourcetobestobservethefreezingpoint.Stirfastenoughmaintainthesametemperaturethroughouttheliquidasit liquid as it cools. Look through the liquid in front of a light Calculate the freezing point depression and molalities of the cools but not so fast that liquid splashes up on the sides of solutions, and the molar mass of benzoic acid. the tube above the liquid. 10. In addition to standard laboratory equipment and glassware, 18. Observe the liquid carefully and record the temperature When crystallization just begins. This temperature is the the materials and equipment needed are: freezing point of the solution. The temperature of the pure digital thermometer acetone for cleaning hot plate lauric acid remains constant until the liquid is fully solutions of benzoic acid and lauric acid oven crystalized. The temperature of the solutionis decreases as the CAUTION: Wear safety glasses at all times. The molien solutions are hot enough to burn skin. 19. Remove the themometer before the solution fully freezes. 11. Obtain or make the following solutions in test mbes. Clean the thermometer probe thoroughly with a paper towel wet with acetone between each measurement. 21. Calcalane the % errox of 7 for pore lauric acid (solution 1) from the accepted value (from step 8). \$s error 26. Ilentify the benwis acid matsst that gives the minimum frccaing tempennice and briefly explain wity. 22. Using equation 3 and the Tf of solution 2 , calculate the experimentai molafity of the benzoic acid in solution 2 . molality of benzoic acid 27. Explain why the temperature of the pare lauric acid remains constase as the liquif crymal ines but the temperiture of the benwis acidlairis acid miture continues to decrease as the solution crytultines. 23. Using the molality of rolution 2 (s4cp 22) and equation 7, calculate the experimental molar mas of benzoic acid. molar mais of benzoic acid 25. The fireries point degeettion of a 1.0045 by mass aqueous tolutiae of acetic acid (CH,COOH) is 0.310OC. For water Kr -1.36-Cir Calculate be fcrmala mas of acetic acid 24. Calculate the percent emor of the molar mass of benmoic acid of solution 2 (compare the values in steps 8 and 23). 29. The freaine point depression of a 1.00S by mass solution persent error of acceic acid (CH,COOH) in benzene is 0.441C. For: bentene Kj5.124C/m, Calculate the formula mass of acetic acid froe this datn 25. Graph the freczing temperature versus the mass pereent of benzoic acid in the solutions. The horizcatal avis ranges from 0.6 (solution 1) to 100 s bennoic acid. 30. How asd aly are these calculated molar masses of acetic acid (from 28 and 29 ) different? 1. Colligative properties of solutions are physical properties which depend on the total number, but not the identity, of solute particles, in the solution. The presence of different solute particles results in vapor pressure lowering, boiling 12. Calculate the molality of benzoic acid in each solution. point clevation, freezing point depression, and osmotic pressure of a solvent. 2. The freezing point depression (T))is the difference in Tf berween pure solvent and solution (solvent + solute): 1379molalmolalmolalmolalmolal2468molalmolalmolalmolal Tf=Tf FUxesocvent Tf socimon Show the work for solution 6 . 3. Tf depends on the solute particle molality where Kr is the freezing point depression constant of a solvent, and the dissociation factor i is the relative number of particles each solute unit dissociates into in a particular solution: Tf=iKf molality soume 4. For lauric acid Kf=3.9C/m, and for lauric acid and benzoic acid i=1. 13. Clean the thermometer probe thoroughly with a paper towel 5. Molality is a measure of concentration that is independent of wet with acetone. Use the same thermometer for all trials. temperature, commonly written as moles solute / kg solvent: 14. Prepare a hot water bath with 300mL of tap water in a 600 molality soume =n soturn /m socvmr (in mol kg 1 units) mL beaker heated on a hot plate to 95C100C. Solutions 7 - 10 require heating in an oven set at 120C. 6. The solute molar mass is the ratio of its mass to its amount: 15. Measure the melting/freezing temperature of each solution Msocuts= mass soturt / n soute (repeating steps 16 - 19). 7. Combining the molality and molar mass equations gives: 16. Remove the rubber stopper and place the test tube in the hot Msocute= mass souvt / (molality socute mass socvest ) water bath. Handle the test tubes with a clamp. When the 8. solution is fully melted insert the clean thermometer probe 8. The accepted melting points and molar masses are: into the solution. Remove the test tube from the hot water lauric acid (LA): TM=43.2CM=200.32gmot1 bath. Make sure that only liquid, and no solids, are present. benzoic acid (BA): TM=122.4CM=122.12gmol1 17. Cool the liquid in air while stirring with the thernometer. 9. The objectives of the experiment are: Hold the test tube near the top lip so that you can see all the Measurethefreezingpointsofpurelauricacidandofsolutionsofbenzoicacidandlauricacid.sourcetobestobservethefreezingpoint.Stirfastenoughmaintainthesametemperaturethroughouttheliquidasit liquid as it cools. Look through the liquid in front of a light Calculate the freezing point depression and molalities of the cools but not so fast that liquid splashes up on the sides of solutions, and the molar mass of benzoic acid. the tube above the liquid. 10. In addition to standard laboratory equipment and glassware, 18. Observe the liquid carefully and record the temperature When crystallization just begins. This temperature is the the materials and equipment needed are: freezing point of the solution. The temperature of the pure digital thermometer acetone for cleaning hot plate lauric acid remains constant until the liquid is fully solutions of benzoic acid and lauric acid oven crystalized. The temperature of the solutionis decreases as the CAUTION: Wear safety glasses at all times. The molien solutions are hot enough to burn skin. 19. Remove the themometer before the solution fully freezes. 11. Obtain or make the following solutions in test mbes. Clean the thermometer probe thoroughly with a paper towel wet with acetone between each measurement. 21. Calcalane the % errox of 7 for pore lauric acid (solution 1) from the accepted value (from step 8). \$s error 26. Ilentify the benwis acid matsst that gives the minimum frccaing tempennice and briefly explain wity. 22. Using equation 3 and the Tf of solution 2 , calculate the experimentai molafity of the benzoic acid in solution 2 . molality of benzoic acid 27. Explain why the temperature of the pare lauric acid remains constase as the liquif crymal ines but the temperiture of the benwis acidlairis acid miture continues to decrease as the solution crytultines. 23. Using the molality of rolution 2 (s4cp 22) and equation 7, calculate the experimental molar mas of benzoic acid. molar mais of benzoic acid 25. The fireries point degeettion of a 1.0045 by mass aqueous tolutiae of acetic acid (CH,COOH) is 0.310OC. For water Kr -1.36-Cir Calculate be fcrmala mas of acetic acid 24. Calculate the percent emor of the molar mass of benmoic acid of solution 2 (compare the values in steps 8 and 23). 29. The freaine point depression of a 1.00S by mass solution persent error of acceic acid (CH,COOH) in benzene is 0.441C. For: bentene Kj5.124C/m, Calculate the formula mass of acetic acid froe this datn 25. Graph the freczing temperature versus the mass pereent of benzoic acid in the solutions. The horizcatal avis ranges from 0.6 (solution 1) to 100 s bennoic acid. 30. How asd aly are these calculated molar masses of acetic acid (from 28 and 29 ) different