Your know-it-all classmate just explained to the class that NaCl is a gas because the line on the graph is basicallyflat. Is your classmate correct? Explain your reasoning.100NaNO,80067060CaCl50Pb(NO)240NaCIKCI3020KCIO,10Ce,(SO0.10 20 3040 50 60 70 80 90 100Temperature (°C)Solubility (g of salt in 100 g H,O)CONS

The solubility of a solute in a particular solvent is the concentration of its saturated solution at…

Your know-it-all classmate just explained to the class that NaCl is a gas because the line on the graph is basically flat. Is your classmate correct? Explain your reasoning. 100 06 80 NaNO 70 60 CaCl 50 Pb(NO3)2 40 KCI NaCI 30 20 KCIO, 10 Ce (SO 10 20 30 40 50 60 70 80 90 100 Temperature (°C) Solubility (g of salt in 100 g H,O) ON

Your know-it-all classmate just explained to the class that NaCl is a gas because the line on the graph is basically flat. Is your classmate correct? Explain your reasoning. 100 06 80 NaNO 70 60 CaCl 50 Pb(NO3)2 40 KCI NaCI 30 20 KCIO, 10 Ce (SO 10 20 30 40 50 60 70 80 90 100 Temperature (°C) Solubility (g of salt in 100 g H,O) ON

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter8: Solutions

Section: Chapter Questions

Problem 8.35EP

See similar textbooks

Similar questions

In some regions of the southwest United States, the water is very hard. For example, in Las Cruces, New Mexico, the tap water contains about 560 g of dissolved solids per milliliter. Reverse osmosis units are marketed in this area to soften water. A typical unit exerts a pressure of 8.0 atm and can produce 45 L water per day. a. Assuming all of the dissolved solids are MgCO3 and assuming a temperature of 27C, what total volume of water must be processed to produce 45 L pure water? b. Would the same system work for purifying seawater? (Assume seawater is 0.60 M NaCl.)
Caffeine is made up of 49.5% C, 5.2% H, 16.5% O, and 28.9% N. A solution made up of 8.25 g of caffeine and 100.0 mL of benzene (d=0.877g/mL) freezes at 3.03C. Pure benzene (k f =5.10C/m) freezes at 5.500C. What are the simplest and molecular formulas for caffeine?
Concentrated hydrochloric acid contains 1.00 mol HCl dissolved in 3.31 mol H2O. What is the mole fraction of HCl in concentrated hydrochloric acid? What is the molal concentration of HCl?
Anthraquinone contains only carbon, hydrogen, and oxygen. When 4.80 mg anthraquinone is burned, 14.2 mg CO2 and 1.65 mg H2O are produced. The freezing point of camphor is lowered by 22.3C when 1.32 g anthraquinone is dissolved in 11.4 g camphor. Determine the empirical and molecular formulas of anthraquinone.
Indicate the most important type of intermolecular attraction responsible for solvation in each of the following solutions: (a) the solutions in Figure 11.8 (b) methanol, CH3OH, dissolved in ethanol, C2H5OH (c) methane, CH4, dissolved in benzene, C6H6 (d) the polar halocarbon CF2CI2 dissolved in the polar halocarbon CF2CICFCI2 (e) O2(I) in N2(l)
Calculate the mole fraction of each solute and solvent: (a) 583 g of H2SO4 in 1.50 kg of water—the acid solution used in an automobile battery (b) 0.86 g of NaCl in 1.00102 g of water—a solution of sodium chloride for intravenous injection (c) 46.85 g of codeine, C18H21NO3, in 125.5 g of ethanol, C2H5OH (d) 25 g of I2 in 125 g of ethanol, C2H5OH
Indicate the most important types of intermolecular attractions in each of the following solutions: (a) The solution in Figure 11.2. (b) NO(I) in CO(I) (c) CI2(g) in Br2(l) (d) HCl(g) in benzene C6H6(l) (e) Methanol CH3OH(I) in H2O(I)
Calculate the freezing point and normal boiling points of each of the following aqueous solutions. (a) 2.63 m acetic acid (b) 33.0 % by mass lactose, C12H22O11 (c) 32.15 mL of ethylene glycol, C2H6O2(d=1.113g/mL) in 624 mL of water (d=1.00g/mL)
Calculate the solubility of O2 in water at a partial pressure of O2 of 120 torr at 25C. The Henrys law constant for O2 is 1.3 103 mol/L atm for Henrys law in the form C = kP, where C is the gas concentration (mol/L).