c# barcode reader from image + (300 mL)(050 mol H /1000 mL) + + (700 mL)(100 mol H /1000 mL) + = 0085 mol H in C#.NET Reader Data Matrix 2d barcode in C#.NET + (300 mL)(050 mol H /1000 mL) + + (700 mL)(100 mol H /1000 mL) + = 0085 mol H

+ (300 mL)(050 mol H /1000 mL) + + (700 mL)(100 mol H /1000 mL) + = 0085 mol H
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(0085 mol H )(1000 mL) = 085 M H+ (1000 mL)(1L)
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Solutions and Colligative Properties 193
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13 D This is a dilution problem Vbefore = (Mafter) (Vafter)/(Mbefore) (60 M HNO3)(0500 L)(1000 mL/1 L)/ (160 M HNO3) = 190 mL 14 D To calculate the molar mass, the mass of the solute and the moles of the solute are needed The molality of the solution may be determined from the freezing-point depression, and the freezingpoint depression constant (I and II) If the mass of the solvent is known, the moles of the solute may be calculated from the molality These moles, along with the mass of the solute, can be used to determine the molar mass 15 A If the mole fraction of chloroform is 020 then the solution has a 080 mol fraction of carbon tetrachloride The moles of chloroform and the kilograms of carbon tetrachloride are needed If 020 mol of chloroform are present, the number of kilograms of carbon tetrachloride is: (080 mol CCl4)(1538 g CCl4 /l mol CCl4) (1 kg/1000 g) = 012 kg m CHCl3 = (020 mol CHCl3)/(012 kg) = 17 m 16 A To calculate the molarity, the moles of urea and the volume of the solution are needed Density is an intensive property, so any arbitrary volume of solution may be used One liter is a convenient volume Using this volume and the density of the solution, you can calculate the mass of the solution Ten percent of this is the mass of urea The mass of urea and the molecular weight of urea give the moles of urea 17 A Freezing-point depression is a colligative property, which depends on the number of particles present The solution with the greatest concentration of particles will have the greatest depression The concentration of particles in E (a nonelectrolyte) is 010 m All other answers are strong electrolytes, and the concentration of particles in these may be calculated by multiplying the concentration by the van t Hoff factor A: 3 010 = 030 B, C, and D: 2 010 = 020
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18 E The strong electrolyte with the greatest concentration of ions is the best conductor D is a weak electrolyte, not a strong electrolyte The number of ions for the strong electrolytes may be found by simply counting the ions: A 2, B 2, C 2, E 4 The best conductor has the greatest value when the molarity is multiplied by the number of ions 19 D Cooling the solution will change the temperature and the volume of the solution Volume is important in the calculation of molarity and density A volume change eliminates answers A and C The mass and the number of moles are not affected by the temperature change Mole fraction and molality will not change This eliminates B and E 20 E This is a dilution problem Vafter = (Mbefore Vbefore)/(Mafter) (100 M HNO3 500 mL)/(40 M HNO3) = 125 mL The final volume is 125 mL Since the original volume was 500 mL, an additional 750 mL must be added 21 E The two most similar substances will be most likely to be ideal 22 A Solutions cannot be separated by titrations or filtering Electrolysis of the solution would produce hydrogen and oxygen gas Chromatography might achieve a minimal separation 23 C The solubility of a gas is increased by increasing the partial pressure of the gas, and by lowering the temperature
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194 U Step 4 Review the Knowledge You Need to Score High
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U Free-Response Questions
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You have 20 minutes to answer the following questions You may not use a calculator You may use the tables at the back of the book Five beakers each containing 1000 mL of an aqueous solution are placed on a lab bench The solutions are all at 25 C Solution 1 contains 020 M KNO3 Solution 2 contains 010 M BaCl2 Solution 3 contains 015 M C2H4(OH)2 Solution 4 contains 020 M (NH4)2SO4 Solution 5 contains 025 M KMnO4 a One of the solutions could oxidize two of the other solutions Which solution is it Which solutions could it oxidize b Which solution has the lowest pH Explain c Which pair of solutions would give a precipitate if they are mixed What is the formula for this precipitate d Which solution would be the poorest conductor of electricity Explain e Rank the solutions in order of increasing boiling point Explain
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