A solution is prepared by mixing 1.00 g ethanol (C2H5OH) with 100.0 g water to give a final volume of 101 mL. Calculate the molarity, mass percent, mole fraction, and molality of ethanol in this solution.A certain soft drink is bottled so that a bottle at 25OC contains CO2 gas at a pressure of 5.0 atm over the liquid. Assuming that the partial pressure of CO2 in the atmosphere is 4.0 x 10-4 atm, calculate the equilibrium concentrations of CO2 in the soda both before and after the bottle is opened. The Henry’s law constant for CO2 in aqueous solution is 3.1 x 10-2 mol/L atm at 25oC.Calculate the freezing point and the boiling point of each of the following solutions. (Assume complete dissociation.)5.0 g NaCl in 25 g H2O2.0 g Al(NO3)3 in 15 g H2OKf = 1.86, Kb = 0.51

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A solution is prepared by mixing 1.00 g ethanol (C₂H₅OH) with 100.0 g water to give a final volume of 101 mL. Calculate the molarity, mass percent, mole fraction, and molality of ethanol in this solution.
A certain soft drink is bottled so that a bottle at 25^OC contains CO₂ gas at a pressure of 5.0 atm over the liquid. Assuming that the partial pressure of CO₂ in the atmosphere is 4.0 x 10^-4 atm, calculate the equilibrium concentrations of CO₂ in the soda both before and after the bottle is opened. The Henry’s law constant for CO₂ in aqueous solution is 3.1 x 10^-2 mol/L atm at 25^oC.
Calculate the freezing point and the boiling point of each of the following solutions. (Assume complete dissociation.)
5.0 g NaCl in 25 g H₂O
2.0 g Al(NO₃)₃ in 15 g H₂O

K_f = 1.86, K_b = 0.51

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