Concept explainers
Ethylene glycol [CH2(OH)CH2(OH)] is a common automobile antifreeze. It is water soluble and fairly nonvolatile (b.p. 197°C). Calculate (a) the freezing point and (b) the boiling point of a solution containing 685 g of ethylene glycol in 2075 g of water.
(a)
Interpretation:
Freezing point and boiling point of the solution containing 685g of ethylene glycol has to determine.
Concept introduction:
Freezing point is the temperature at which liquid turns into solid.
Freezing point depression
Where,
m- Molality of the solution
Boiling point is the temperature at which liquid turns into a gas. Example: boiling point of water is
Where,
Boiling point elevation
Where,
m- Molality of the solution
Answer to Problem 13.6WE
Freezing point of the solution =
Explanation of Solution
Given
Amount of Ethylene glycol in water =
Amount of water in which Ethylene glycol dissolved=
Boiling point of Ethylene glycol =
Conversion of grams of ethylene glycol to moles
By plugging in the value of mass and molar mass of ethylene glycol, the number of moles of ethylene glycol has calculated.
Calculation of molality of the solution
By plugging in the value of moles of ethylene glycol and amount of water, the molality of the solution has calculated.
Calculation of molality of glucose solution
By plugging in the value of moles of the glucose and kilogram of water, the molality solution has calculated.
Calculation of freezing point of the solution
The freezing point of the solution is (0-
By plugging in the value of freezing point and molal freezing point depression constant for ethylene glycol, freezing point of the solution has calculated.
Freezing point of the solution has calculated as
(b)
Interpretation:
Freezing point and boiling point of the solution containing 685g of ethylene glycol has to determine.
Concept introduction:
Freezing point is the temperature at which liquid turns into solid.
Freezing point depression
Where,
m- Molality of the solution
Boiling point is the temperature at which liquid turns into a gas. Example: boiling point of water is
Where,
Boiling point elevation
Where,
m- Molality of the solution
Answer to Problem 13.6WE
Boiling point of the solution =
Explanation of Solution
Given
Amount of Ethylene glycol in water =
Amount of water in which Ethylene glycol dissolved=
Boiling point of Ethylene glycol =
Conversion of grams of ethylene glycol to moles
By plugging in the value of mass and molar mass of ethylene glycol, the number of moles of ethylene glycol has calculated.
Calculation of molality of the solution
By plugging in the value of moles of ethylene glycol and amount of water, the molality of the solution has calculated.
Calculation of molality of glucose solution
By plugging in the value of moles of the glucose and kilogram of water, the molality solution has calculated.
Calculation of boiling point of the solution
The boiling point of the solution is (100+
By plugging in the value of freezing point and molal freezing point depression constant for ethylene glycol, freezing point of the solution has calculated.
Boiling point of the solution has calculated as
Want to see more full solutions like this?
Chapter 13 Solutions
Chemistry: Atoms First
- A 1.00 mol/kg aqueous sulfuric acid solution, H2SO4,freezes at 4.04 C. Calculate i, the vant Hoff factor,for sulfuric acid in this solution.arrow_forwardWhat would be the freezing point of a solution formed by adding 1.0 mole of glucose (a molecular compound) to the following amounts of water? a. 250 g (0.25 kg) b. 500 g (0.500 kg) c. 1000 g (1.000 kg) d. 2000 g (2.000 kg)arrow_forward6-111 As noted in Section 6-8C, the amount of external pressure that must be applied to a more concentrated solution to stop the passage of solvent molecules across a semipermeable membrane is known as the osmotic pressure The osmotic pressure obeys a law similar in form to the ideal gas law (discussed in Section 5-4), where Substituting for pressure and solving for osmotic pressures gives the following equation: RT MRT, where M is the concentration or molarity of the solution. (a) Determine the osmotic pressure at 25°C of a 0.0020 M sucrose (C12H22O11) solution. (b) Seawater contains 3.4 g of salts for every liter of solution. Assuming the solute consists entirely of NaCl (and complete dissociation of the NaCI salt), calculate the osmotic pressure of seawater at 25°C. (c) The average osmotic pressure of blood is 7.7 atm at 25°C. What concentration of glucose (C6H12O6) will be isotonic with blood? (d) Lysozyme is an enzyme that breaks bacterial cell walls. A solution containing 0.150 g of this enzyme in 210. mL of solution has an osmotic pressure of 0.953 torr at 25°C. What is the molar mass of lysozyme? (e) The osmotic pressure of an aqueous solution of a certain protein was measured in order to determine the protein's molar mass. The solution contained 3.50 mg of protein dissolved in sufficient water to form 5.00 mL of solution. The osmotic pressure of the solution at 25°C was found to be 1.54 torr. Calculate the molar mass of the protein.arrow_forward
- 6-68 If we add 175 g of ethylene glycol, C2H6O2, per 1000. g of water to a car radiator, what will be the freezing point of the solution?arrow_forwardWhich solute has the greatest effect on the boiling pointof 1.00 kg of water: 50.0 g of strontium chloride (SrCl2) or 150.0 g of carbon tetrachloride (CCl4) ? Justify youranswer.arrow_forwardWater at 25 C has a density of 0.997 g/cm3. Calculate the molality and molarity of pure water at this temperature.arrow_forward
- What is the freezing point and normal boiling point of a solution made by adding 39 mL of acetone, C3H6O, to 225 mL of water? The densities of acetone and water are 0.790 g/cm3 and 1.00 g/cm3, respectively.arrow_forwardSome ethylene glycol, HOCH2CH2OH, is added to your cars cooling system along with 5.0 kg of water. If the freezing point of the water-glycol solution is 15.0 C, what mass of HOCH2CH2OH must have been added?arrow_forwardSodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride (CaCl2) is sometimes used for this purpose too. Let us compare the effectiveness of equal masses of these two compounds in lowering the freezing point of water, by calculating the freezing point depression of solutions containing 200. g of each salt in 1.00 kg of water. (An advantage of CaCl2 is that it acts more quickly because it is hygroscopic, that is. it absorbs moisture from the air to give a solution and begin the process. A disadvantage is that this compound is more costly.)arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningGeneral, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage Learning