(a)
Interpretation:
The vapor pressure of the solvent in an aqueous solution of
Concept Introduction:
The equilibrium between a liquid and its vapor produces a characteristic vapor pressure for each substance that depends on the temperature. The lowering of the vapor pressure is caused by a lesser ability of the solvent to evaporate, so equilibrium is reached with a smaller concentration of the solvent in the gas phase. The vapor pressure of a solution is expressed using Raoult’s law:
The vapor pressure of the solvent
Mole fraction: Mole fraction of a substance in a solution is the number of moles of that substance divided by the total number of moles of all substances present. The formula is,
(b)
Interpretation:
The vapor pressure of the solvent in an aqueous solution of
Concept Introduction:
Refer to part (a).
Want to see the full answer?
Check out a sample textbook solutionChapter 5 Solutions
ACHIEVE/CHEMICAL PRINCIPLES ACCESS 2TERM
- For 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_forwardSimple 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_forwardFluoridation of city water supplies has been practiced in the United States for several decades. It is done by continuously adding sodium fluoride to water as it comes from a reservoir. Assume you live in a medium-sized city of 150,000 people and that 660 L (170 gal) of water is used per person per day. What mass of sodium fluoride (in kilograms) must be added to the water supply each year (365 days) to have the required fluoride concentration of 1 ppm (part per million)that is, 1 kilogram of fluoride per 1 million kilograms of water? (Sodium fluoride is 45.0% fluoride, and water has a density of 1.00 g/cm3.)arrow_forward
- Use the following data to calculate the enthalpy of solution of sodium perchlorate, NaClO4: fH(s)=382.9kJ/mol and fH(aq,1m)=369.5kJ/molarrow_forwardWhat 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_forwardWrite the equilibrium constant for the reaction CH4(g) + 3 Cl2(g) ⇋ CHCl3(l) + 3 HCl(g), with the gases treated as perfect.arrow_forward
- Calculate the vapor pressure of ethanol, CH₃CH₂OH, in a water solution containing 72.5% ethanol by volume at 19.0 °C. The vapor pressure of pure ethanol at 19.0 °C is 40.0 Torr. The density of ethanol is 0.789 g·mL⁻¹ and the density of water is 1.000 g·mL⁻¹.arrow_forwardAt 20 °C, the concentration of dissolved oxygen in water exposed to gaseous oxygen at a partial pressure of 101.3 kPa is 1.38 × 10–3 mol L–1. Use Henry’s law to determine the solubility of oxygen when its partial pressure is 20.7 kPa, the approximate pressure of oxygen in earth’s atmosphere. The vapor pressure of pure hexane and pentane at 25°C are 149.1 mmHg and 508.5 mmHg, respectively. If a hexane pentane solution has a mole fraction of hexane of 0.750, what are the vapor pressures of hexane and pentane above the solution? What is the total vapor pressure?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_forward
- Calculate the molality of chloride ions in an aqueous solution of magnesium chloride in which the mole fraction of magnesium chloride is 0.0600. b= Calculate the molality of 6.80 g of sodium hydroxide dissolved in 315 g of water. b= Calculate the molality for 1 L of a 2.00 M HCl aqueous solution that has a density of 1.0745 g·cm^−3. b=arrow_forwardWrite the equilibrium constant for the reaction P4(s) + 6 H2(g) ⇋ 4 PH3(g), with the gases treated as perfect.arrow_forwardIf 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_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 & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning