The boiling point of water is 100.0°C at 1 atmosphere.How many grams of potassium hydroxide (56.11 g/mol), must bedissolved in 221.0 grams of water to raise the boiling point by 0.450 °C?Refer to the table for the necessary boiling or freezing point constant.SolventFormulaKы(°C/m) K(°C/m)WaterH₂O0.5121.86EthanolCH3CH2OH1.221.99Chloroform CHC133.67BenzeneC6H62.535.12Diethyl ether CH3 CH2OCH2CH3 2.02Mass =g potassium hydroxide

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Answered: The boiling point of water is 100.0°C…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section: Chapter Questions

Problem 75QRT

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Consider two hypothetical pure substances, AB(s) and XY(s). When equal molar amounts of these substances are placed in separate 500-mL samples of water, they undergo the following reactions: AB(s)A+(aq)+B(aq)XY(s)XY(aq) a Which solution would you expect to have the lower boiling point? Why? b Would you expect the vapor pressures of the two solutions to be equal? If not, which one would you expect to have the higher vapor pressure? c Describe a procedure that would make the two solutions have the same boiling point. d If you took 250 mL of the AB(aq) solution prepared above, would it have the same boiling point as the original solution? Be sure to explain your answer. e The container of XY(aq) is left out on the bench top for several days, which allows some of the water to evaporate from the solution. How would the melting point of this solution compare to the melting point of the original solution?
The solubility of NaCl in water at 100 C is 39.1 g/100. g of water Calculate the boiling point of this solution. (Assume i = 1.85 for NaCl.)
In a mountainous location, the boiling point of pure water is found to be 95C. How many grams of sodium chloride must be added to 1 kg of water to bring the boiling point back to 100C? Assume that i = 2.
Carbon tetrachloride (CCl4) boils at 76.8C and has a density of 1.59 g/mL. (a) A solution prepared by dissolving 0.287 mol of a nonelectrolyte in 255 mL of CCl4 boils at 80.3C. What is the boiling point constant (kb) for CCl4? (b) Another solution is prepared by dissolving 37.1 g of an electrolyte (MM=167g/mol) in 244 mL of CCl4. The resulting solution boils at 85.2C. What is i for the electrolyte?
A forensic chemist is given a white solid that is suspected of being pure cocaine (C17H21NO4, molar mass = 303.35 g/mol). She dissolves 1.22 0.01 g of the solid in 15.60 0.01 g benzene. The freezing point is lowered by 1.32 0.04C. a. What is the molar mass of the substance? Assuming that the percent uncertainty in the calculated molar mass is the same as the percent uncertainty in the temperature change, calculate the uncertainty in the molar mass. b. Could the chemist unequivocally state that the substance is cocaine? For example, is the uncertainty small enough to distinguish cocaine from codeine (C18H21NO3, molar mass = 299.36 g/mol)? c. Assuming that the absolute uncertainties in the measurements of temperature and mass remain unchanged, how could the chemist improve the precision of her results?
A 12.0-g sample of a nonelectrolyte is dissolved in 80.0 g of water. The solution freezes at -1.94 C. Calculate the molar mass of the substance.
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?
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)
Sodium 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.)
a. Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide. Lattice Energy Hsoln CaCl2(s) 2247kj/mol 46kj/mol Cal2(s) 2059kj/mol 104kj/mol b. Based on your answers to part a, which ion, Cl or I, is more strongly attracted to water?
Two samples of sodium chloride solutions are brought to a boil on a stove. One of the solutions boils at 100.10C and the other at 100.15C. a Which of the solutions is more concentrated? b Which of the solutions would have a lower freezing point? c If you split the solution that boils at 100.1C into two portions, how would the boiling points of the samples compare? Which of the following statements do you agree with regarding the determination of your answer for part c? I. The question cannot be answered with certainty without knowing the volumes of each portion. II. Making the necessary assumption that the two samples have equal volumes, I was able to correctly answer the question. III. The volumes that the sample was split into are irrelevant when determining the correct answer.
Water at 25 C has a density of 0.997 g/cm3. Calculate the molality and molarity of pure water at this temperature.

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