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Problem 33
Which of the following in each pair is likely to be more soluble in hexane, C6H14: (a) CCl4 or CaCl2, (b) benzene (C6H6) or glycerol, CH2(OH)CH(OH)CH2OH, (c) octanoic acid, CH3CH2CH2CH2CH2CH2CH2COOH, or acetic acid, CH3COOH? Explain your answer in each case.
Problem 34a
Which of the following in each pair is likely to be more soluble in water: (a) cyclohexane (C6H12) or glucose (C6H12O6),
Problem 34b
Which of the following in each pair is likely to be more soluble in water: (b) propionic acid (CH3CH2COOH) or sodium propionate (CH3CH2COONa)
Problem 34c
Which of the following in each pair is likely to be more soluble in water: (c) HCl or ethyl chloride (CH3CH2Cl)? Explain in each case.
Problem 35c
Indicate whether each statement is true or false: (c) As you cool a saturated solution from high temperature to low temperature, solids start to crystallize out of solution if you achieve a supersaturated solution.
Problem 35d
Indicate whether each statement is true or false: (d) If you take a saturated solution and raise its temperature, you can (usually) add more solute and make the solution even more concentrated.
- The Henry’s law constant for helium gas in water at 30 °C is 3.7 * 10^-4 M/atm and the constant for N2 at 30 °C is 6.0 * 10^-4 M/atm. If the two gases are each present at 1.5 atm pressure, calculate the solubility of each gas.
Problem 37
Problem 39a
(a) Calculate the mass percentage of Na2SO4 in a solution containing 10.6 g of Na2SO4 in 483 g of water.
Problem 39b
(b) An ore contains 2.86 g of silver per ton of ore. What is the concentration of silver in ppm?
- A solution is made containing 14.6 g of CH3OH in 184 g of H2O. Calculate (a) the mole fraction of CH3OH.
Problem 41
Problem 42a
A solution is made containing 20.8 g of phenol (C6H5OH) in 425 g of ethanol (CH3CH2OH). Calculate (a) the mole fraction of phenol,
Problem 42c
A solution is made containing 20.8 g of phenol (C6H5OH) in 425 g of ethanol (CH3CH2OH). Calculate (c) the molality of phenol.
Problem 43c
Calculate the molarity of the following aqueous solutions: (c) 25.0 mL of 3.50 M HNO3 diluted to 0.250 L.
Problem 44b
What is the molarity of each of the following solutions: (b) 5.25 g of Mn(NO3)2⋅2H2O in 175 mL of solution,
- How many grams of sulfur (S) must be dissolved in 100.0 g of naphthalene (C10H8) to make a 0.12 m solution?
Problem 46
- A sulfuric acid solution containing 571.6 g of H2SO4 per liter of solution has a density of 1.329 g/cm³. Calculate (d) the molarity of H2SO4 in this solution.
Problem 47
Problem 48a
Ascorbic acid (vitamin C, C6H8O6) is a water-soluble vitamin. A solution containing 80.5 g of ascorbic acid dissolved in 210 g of water has a density of 1.22 g/mL at 55 °C. Calculate (a) the mass percentage,
Problem 48c
Ascorbic acid (vitamin C, C6H8O6) is a water-soluble vitamin. A solution containing 80.5 g of ascorbic acid dissolved in 210 g of water has a density of 1.22 g/mL at 55 °C. Calculate (c) the molality,
Problem 49a
The density of acetonitrile (CH3CN) is 0.786 g/mL and the density of methanol (CH3OH) is 0.791 g/mL. A solution is made by dissolving 22.5 mL of CH3OH in 98.7 mL of CH3CN. (a) What is the mole fraction of methanol in the solution?
Problem 49b
The density of acetonitrile (CH3CN) is 0.786 g/mL and the density of methanol (CH3OH) is 0.791 g/mL. A solution is made by dissolving 22.5 mL of CH3OH in 98.7 mL of CH3CN. (b) What is the molality of the solution?
Problem 49c
The density of acetonitrile (CH3CN) is 0.786 g/mL and the density of methanol (CH3OH) is 0.791 g/mL. A solution is made by dissolving 22.5 mL of CH3OH in 98.7 mL of CH3CN. (c) Assuming that the volumes are additive, what is the molarity of CH3OH in the solution?
Problem 50a
The density of toluene (C7H8) is 0.867 g/mL, and the density of thiophene (C4H4S) is 1.065 g/mL. A solution is made by dissolving 8.10 g of thiophene in 250.0 mL of toluene. (a) Calculate the mole fraction of thiophene in the solution.
Problem 50b
The density of toluene (C7H8) is 0.867 g/mL, and the density of thiophene (C4H4S) is 1.065 g/mL. A solution is made by dissolving 8.10 g of thiophene in 250.0 mL of toluene. (b) Calculate the molality of thiophene in the solution.
Problem 51b
Calculate the number of moles of solute present in each of the following aqueous solutions: (b) 86.4 g of 0.180 m KCl,
Problem 51c
Calculate the number of moles of solute present in each of the following aqueous solutions: (c) 124.0 g of a solution that is 6.45% glucose (C6H12O6) by mass.
Problem 52a
Calculate the number of moles of solute present in each of the following solutions: (a) 255 mL of 1.50 M HNO3(aq),
Problem 52b,c
Calculate the number of moles of solute present in each of the following solutions: (b) 50.0 mg of an aqueous solution that is 1.50 m NaCl, (c) 75.0 g of an aqueous solution that is 1.50% sucrose (C12H22O11) by mass.
Problem 53b
Describe how you would prepare each of the following aqueous solutions from water and solid KBr: b. 125 g of 0.180 m KBr.
Problem 54a
Describe how you would prepare each of the following aqueous solutions from water and the solid solute: a. 1.50 L of 0.110 M (NH4)2SO4 solution;
Problem 55
Commercial aqueous nitric acid has a density of 1.42 g/mL and is 16 M. Calculate the percent HNO3 by mass in the solution.