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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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State how to prepare the following solutions. Identify the solute and the solvent for each preparation
and the corresponding volume of each.
(Example: 1.a. solute: ethyl alcohol = 68.0 mL solvent: water = 32.0 mL)
- 120 mL of 10 % v/v solution of Povidone iodine (betadine), C6H9I2NO, in water
- 100 mL of 40 % v/v solution of Isopropyl alcohol, C3H8O, in water
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- Indicate the volume of each solute and solvent needed to make the following solutions: a. 280. mL of a 39% v/v solution of ethanol, C2HO, in water mL of C2 H6O mL of water b. 435 mL of a 1.8% v/v solution of ethyl acetate, C4H3 O2, in water mL of C4Hg O2 mL of waterarrow_forwardWhat mass of oxalic acid (H2C2O4) is required to prepare a 1.00L solution(d = 1.05 g/mL) with a vapor pressure of 21.97 mm Hg at 24°C (vapor pressure of water at 24°C = 22.38 mm Hg)? Assume oxalic acid nonvolatile, nonelectrolyte solute.arrow_forwardFill in the values for the table. The molar mass of NaCl is 58.443 g/mol Mass of NaCl (g) Mass of solution (g) Volume of solution (mL) Boiling point (C) Mass of water (g) % NaCl (%) Density of Solution (g/mL) Moles of NaCl (mol) Molarity (mol/L) Molality (mol/kg) 0.0000 9.9451 10.00 99.8 c 1.0090 100.3998 100.00 100.4 2.4904 101.4023 100.00 100.8 5.0063 103.2222 100.00 101.5 5.1559 103.0978 100.00 102.1 6.0024 103.4004 100.00 101.1 6.3477 104.9210 100.00 102.7 7.4815 104.5044 100.00 101.8 10.0041 106.2007 100.00 102.1 10.2103 106.6904 100.00 102.8arrow_forward
- Calculate the: %m/v, %v/v, %m/m and M of a solution that contains 28.0 grams of KNO3 in 300.0 mL ofwater. The density of KNO3=2.11g/mL and the density of H2O=1.0g/mL.arrow_forwardnheducation.com Saved Be sure to answer all parts. Ethylene glycol CH,(OH)CH,(OH) is a common automobile antifreeze. Calculate the freezing point and boiling point of a solution containing 223 g of ethylene glycol and 1055 g of water. (K, and K for water are 0.52°C/m and 1.86°C/m, respectively.) freezing point PC boiling point °C Prey 9 of 10 Nearrow_forwardWhat volume of a 1.2 M sulfuric acid solution should be used to prepare 2.0 L of a 1.00 Msulfuric acid solution? Equations- M = mol of solute /L of solution for molarity M 1 (V 1 ) = M 2 (V 2 ) for dilutionarrow_forward
- Calculate the percent mass per volume, % (m/v), of a dextrose solution containing 8.00 g8.00 g of dextrose in 2.00×102 mL2.00×102 mL of solution. Note that mass is not technically the same as weight, but the abbreviation % (w/v) is often used interchangeably with % (m/v).arrow_forwardHow much KNO3 does a student need to make a SATURATED KNO3 aqueous solution in 500 g of H₂O at 50°C? a) At least 200 g b) At least 400 g c) At least 500 g d) At least 750 g Solubility (grams per 100 grams of water) 260 240 220 200 180 160 140 120 100 80 60 40 20 0 20 NACIO 40 KNO, KBr NaCl 60 60 100 Temperature (°C)arrow_forwardGiven the following mixture of two compounds 45.00 mL of X (MW =53.00 g/mol)(density 1.186 g/mL) and 830.00 mL of Y (71.00 g/mol)(density 1.041 g/mL). The freezing point of pure Y is 71.00 degrees C. The molal freezing constant is 4.609 degrees C/m. What is the freezing point of the solution.arrow_forward
- What is the boiling point of a solution prepared by dissolving 37.5 g of glucose (C6H12O6, MW=180.16g/mol) in 750 g of ethanol (CH3CH2OH, MW=46.07g/mol)? Kb 1.22°C/m, boiling point of pure ethanol=78.24°C? ATb=ikbm 78.56°C 70.57°C 77.91°C 85.91°Carrow_forward[References] Indicate how much of each solute and solvent is needed to make the following solutions (assume that density is 1 g/mL) a. 500.0 mL of a 5.00% w/w H2S solution in water g of H2S g of water b. 342.0 mL of a 0.400% w/w benzene solution in toluene g of benzene g of toluenearrow_forward
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