Concept explainers
(a)
Interpretation:
Approximate molar mass of the compound has to be calculated.
Concept introduction:
Freezing point depression:
The lowering of the vapor pressure of a solvent by a solute leads to a lowering of the freezing point of the solution relative to that of the pure solvent. This effect is called as the freezing point depression. The mathematical relationship is given below.
Where,
(b)
Interpretation:
When the empirical formula of the compound is
(c)
Interpretation:
More accurate molar mass of the compound has to be calculated
Want to see the full answer?
Check out a sample textbook solutionChapter 5 Solutions
Chemical Principles: The Quest for Insight
- Simple acids such as formic acid, HCOOH, and acetic acid, CH3COOH, are very soluble in water; however, fatty acids such as stearic acid, CH3(CH2)16COOH, and palmitic acid, CH3(CH2)14COOH, are water-insoluble. Based on what you know about the solubility of alcohols, explain the solubility of these organic acids.arrow_forwardFor each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Ammonia gas in water with P = 1 atm and T = 50C Ammonia gas in water with P = 1 atm and T = 90C b. Carbon dioxide gas in water with P = 2 atm and T = 50C Carbon dioxide gas in water with P = 1 atm and T = 50C c. Table salt in water with P = 1 atm and T = 60C Table salt in water with P = 1 atm and T = 50C d. Table sugar in water with P = 2 atm and T = 40C Table sugar in water with P = 1 atm and T = 70Carrow_forwardFor each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Oxygen gas in water with P = 1 atm and T = 10C Oxygen gas in water with P = 1 atm and T = 20C b. Nitrogen gas in water with P = 2 atm and T = 50C Nitrogen gas in water with P = 1 atm and T = 70C c. Table salt in water with P = 1 atm and T = 40C Table salt in water with P = 1 atm and T = 70C d. Table sugar in water with P = 3 atm and T = 30C Table sugar in water with P = 1 atm and T = 80Carrow_forward
- A certain liquid X has a normal freezing point of 7.00°C and a freezing point depression constant =Kf 7.41·°C·kgmol−1. A solution is prepared by dissolving some iron(III) chloride (FeCl3) in 700.g of X. This solution freezes at 3.5°C. Calculate the mass of FeCl3 that was dissolved. Be sure your answer is rounded to the correct number of significiant digits.arrow_forward3) Camphor (CoH160) melts at 179.8 °C, and it has a particularly large freezing point depression constant of 40.0 "C/m. When 0.186 g of an organic substance of unknown molar mass is dissolved in 22.10 g of liquid camphor, the freezing point of the mixture is found to be 176.7 C. What is the molar mass of the organic substance?arrow_forwardWhen 14.3 g of a certain molecular compound X are dissolved in 85.0 g of benzene C6H6, the freezing point of the solution is measured to be 0.5 °C. Calculate the molar mass of X. molal freezing point depression constant (Kf)°C·kg·mol−1 of benzen is 5.07 If you need any additional information on benzene, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to 2 significant digits.arrow_forward
- If you compare the solubilities of the noble gases in water,you find that solubility increases from smallest atomicweight to largest, Ar < Kr < Xe. Which of the followingstatements is the best explanation? (a) The heavier the gas, the more it sinks to the bottom ofthe water and leaves room for more gas molecules at thetop of the water.(b) The heavier the gas, the more dispersion forces it has,and therefore the more attractive interactions it haswith water molecules.(c) The heavier the gas, the more likely it is to hydrogenbondwith water.(d) The heavier the gas, the more likely it is to make a saturatedsolution in water.arrow_forwardDistinguish between water quality and hydrochemistry.arrow_forwardA 0.100-L solution is made by dissolving 0.441 g of CaCl21s2 in water. (a) Calculate the osmotic pressure of this solution at 27 °C, assuming that it is completely dissociated into its component ions.arrow_forward
- What is the solubility of carbon dioxide (in units of grams per liter) in water at 25 °C, when the CO2 gas over the solution has a partial pressure of 208 mm Hg? kH for CO2 at 25 °C is 3.36×10-2 mol/L·atm.arrow_forwardTo obtain a precipitate which is useful for gravimetric analysis, the analyst tries to obtain conditions to encourage crystal growth, as opposed to the formation of a colloid. Which of the following statements aids in the formation of a crystalline precipitate and the formation of a colloidal precipitate? Drag your answers to the appropriate markers. (a) The solutions are made as dilute as practical to allow crystals to form slowly. (b) The addition of strong electrolytes (e.g. NaCl or HCl) in the analyte solution, prior to the precipitation reaction. (c) After the digestion of the precipitate, the hot solution is cooled down to room temperature gradually and kept undisturbed overnight. (d) The analyst selects the precipitate of the analyte with the Ksp less than 1 x 10 -15 (e) The Relative Supersaturation value of the analyte solution should be greater than 1 million upon the addition of the precipitating reagent. formation of colloidal precipitate favored formation of crystalline…arrow_forward4. (a) The boiling point of a methanolic solution of the non-electrolyte, acetamide (CH;CONH2) is 66.9 °C. Calculate the percentage by mass of acetamide in this solution. Methanol: K, = 1.13 °C kg mol"arrow_forward
- General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning