Exam 12: Solutions

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What is the freezing point of a solution of 7.15 g MgCl2 in 100 g of water? Kf for water is What is the freezing point of a solution of 7.15 g MgCl<sub>2</sub> in 100 g of water? K<sub>f</sub> for water is

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Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molarity of the HCl if the solution has a density of 1.20 g mL-1.

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Calculate the freezing point of a solution containing 5.0 grams of KCl and 550.0 grams of water. The molal freezing point depression constant ( Calculate the freezing point of a solution containing 5.0 grams of KCl and 550.0 grams of water. The molal freezing point depression constant (   ) for water is  ) for water is Calculate the freezing point of a solution containing 5.0 grams of KCl and 550.0 grams of water. The molal freezing point depression constant (   ) for water is

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A 1.00 L sample of water contains 0.0036 g of Cl⁻ ions. Determine the concentration of chloride ions in ppm if the density of the solution is 1.00 g mL-1.

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Pentane (C5H12) is mixed with 75.8 g hexane (C6H14). Calculate the vapour pressure of the resulting solution. The vapour pressures of pure pentane and hexane are 425 Torr and 151 Torr, respectively. The total solution mass is 206.6 g. Assume ideal behaviour.

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A solid can be purified through which technique?

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Match the following. -0.020 mol kg-1 NH4Cl

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A solution is 2.25% by weight NaHCO3. How many grams of NaHCO3 are in 150.0 g of solution?

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Determine the solubility of CO2 in soda water at 25 °C if the pressure of CO2 is 5.2 bar. The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10-2 mol L-1 bar-1.

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A solution is prepared by dissolving 21.0 g of glycerin ( A solution is prepared by dissolving 21.0 g of glycerin (       ) in 201 g of ethanol   The freezing point of the solution is ________°C. The freezing point of pure ethanol is   . The molal freezing point depression constant (   ) for ethanol is   The molar masses of glycerin and of ethanol are 92.1 g mol<sup>-1</sup> and 46.1 g mol<sup>-</sup><sup>1</sup>, respectively. A solution is prepared by dissolving 21.0 g of glycerin (       ) in 201 g of ethanol   The freezing point of the solution is ________°C. The freezing point of pure ethanol is   . The molal freezing point depression constant (   ) for ethanol is   The molar masses of glycerin and of ethanol are 92.1 g mol<sup>-1</sup> and 46.1 g mol<sup>-</sup><sup>1</sup>, respectively. A solution is prepared by dissolving 21.0 g of glycerin (       ) in 201 g of ethanol   The freezing point of the solution is ________°C. The freezing point of pure ethanol is   . The molal freezing point depression constant (   ) for ethanol is   The molar masses of glycerin and of ethanol are 92.1 g mol<sup>-1</sup> and 46.1 g mol<sup>-</sup><sup>1</sup>, respectively. ) in 201 g of ethanol A solution is prepared by dissolving 21.0 g of glycerin (       ) in 201 g of ethanol   The freezing point of the solution is ________°C. The freezing point of pure ethanol is   . The molal freezing point depression constant (   ) for ethanol is   The molar masses of glycerin and of ethanol are 92.1 g mol<sup>-1</sup> and 46.1 g mol<sup>-</sup><sup>1</sup>, respectively. The freezing point of the solution is ________°C. The freezing point of pure ethanol is A solution is prepared by dissolving 21.0 g of glycerin (       ) in 201 g of ethanol   The freezing point of the solution is ________°C. The freezing point of pure ethanol is   . The molal freezing point depression constant (   ) for ethanol is   The molar masses of glycerin and of ethanol are 92.1 g mol<sup>-1</sup> and 46.1 g mol<sup>-</sup><sup>1</sup>, respectively. . The molal freezing point depression constant ( A solution is prepared by dissolving 21.0 g of glycerin (       ) in 201 g of ethanol   The freezing point of the solution is ________°C. The freezing point of pure ethanol is   . The molal freezing point depression constant (   ) for ethanol is   The molar masses of glycerin and of ethanol are 92.1 g mol<sup>-1</sup> and 46.1 g mol<sup>-</sup><sup>1</sup>, respectively. ) for ethanol is A solution is prepared by dissolving 21.0 g of glycerin (       ) in 201 g of ethanol   The freezing point of the solution is ________°C. The freezing point of pure ethanol is   . The molal freezing point depression constant (   ) for ethanol is   The molar masses of glycerin and of ethanol are 92.1 g mol<sup>-1</sup> and 46.1 g mol<sup>-</sup><sup>1</sup>, respectively. The molar masses of glycerin and of ethanol are 92.1 g mol-1 and 46.1 g mol-1, respectively.

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Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 bar of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 mol L-1 bar-1.

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Choose the aqueous solution that has the highest boiling point. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

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What mass of CuCl2 is contained in 75.85 g of a 22.4% by mass solution of CuCl2 in water?

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Calculate the vapour pressure of pure water at 65 °C if a 465 mL solution containing 123.0 g of ribose, C5H10O5, has a vapour pressure of 247.54 mbar. Assume no change in volume occurs upon dissolution.

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Determine the freezing point depression of a solution that contains 30.7 g glycerin (C3H8O3, molar mass = 92.09 g mol-1) in 376 mL of water. Some possibly useful constants for water are Kf = 1.86 °C m-1 and Kb = 0.512 °C m-1.

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Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C2H6O2) dissolved in 500.0 g of water. Kf = 1.86 °C m-1 and Kb = 0.512 °C m-1.

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Determine the molality of a solution prepared by dissolving 0.500 moles of CaF2 in 11.5 moles H2O.

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What is the expected van't Hoff factor for FeCl3? (Assume dilute conditions)

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At 20 °C, a 0.389 mol L-1 aqueous solution of ammonium chloride has a density of 1.0064 At 20 °C, a 0.389 mol L<sup>-1</sup> aqueous solution of ammonium chloride has a density of 1.0064   What is the mass % of ammonium chloride in the solution? The formula weight of   Cl is  What is the mass % of ammonium chloride in the solution? The formula weight of At 20 °C, a 0.389 mol L<sup>-1</sup> aqueous solution of ammonium chloride has a density of 1.0064   What is the mass % of ammonium chloride in the solution? The formula weight of   Cl is  Cl is At 20 °C, a 0.389 mol L<sup>-1</sup> aqueous solution of ammonium chloride has a density of 1.0064   What is the mass % of ammonium chloride in the solution? The formula weight of   Cl is

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A nonelectrolyte compound with a molar mass of 648 g mol-1 was dissolved in enough water to make 250 mL of solution at 25 °C and produced an osmotic pressure of 27.4 mbar. Calculate the mass of the compound, in g, used to make this solution.

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