(13) A 9.50 % by mass solution of acetone (C3H,0) in water has a density of 0.9849g/mL at 20C. What is the molarity of this solution?(14) The mole fraction of NaCl in an aqueous solution of NaCl is 0.23. What is themolality of the solution?(15) Draw and explain a Phase Diagram of water as pure solvent, and saline solution assolvent with non-volatile solute. Determine the following points: Triple point, Boiling andFreezing points at sea level, Delta Tb, and Delta Tf,

Answered: Image /qna-images/answer/1ae26b82-d423-4ee5-8ef1-ec0d755dac12.jpg

(13) A 9.50 % by mass solution of acetone (C3H&O) in water has a density of 0.9849 g/mL at 20C. What is the molarity of this solution? 114) T he mole freetion oE NeCl in on eguee ue oelution of NeC Lie O 22 Wbet ie t he

(13) A 9.50 % by mass solution of acetone (C3H&O) in water has a density of 0.9849 g/mL at 20C. What is the molarity of this solution? 114) T he mole freetion oE NeCl in on eguee ue oelution of NeC Lie O 22 Wbet ie t he

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter10: Properties Of Solutions

Section: Chapter Questions

Problem 9ALQ

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Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

(13) A 9.50 % by mass solution of acetone (C3H,0) in water has a density of 0.9849
g/mL at 20C. What is the molarity of this solution?
(14) The mole fraction of NaCl in an aqueous solution of NaCl is 0.23. What is the
molality of the solution?
(15) Draw and explain a Phase Diagram of water as pure solvent, and saline solution as
solvent with non-volatile solute. Determine the following points: Triple point, Boiling and
Freezing points at sea level, Delta Tb, and Delta Tf,

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(a) If you dissolve 10.0 g (about one heaping teaspoonful) of sugar (sucrose, C12H22O11) in a cup of water (250. g), what are the mole fraction, molality, and weight percent of sugar? (b) Seawater has a sodium ion concentration of 1.08 104 ppm. If the sodium is present in the form of dissolved sodium chloride, what mass of NaCl is in each liter of seawater? Seawater is denser than pure water because of dissolved salts. Its density is 1.05 g/mL
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?
What would be the freezing point of a solution formed by adding 1.0 mole of glucose (a molecular compound) to the following amounts of water? a. 250 g (0.25 kg) b. 500 g (0.500 kg) c. 1000 g (1.000 kg) d. 2000 g (2.000 kg)
What is the freezing point and normal boiling point of a solution made by adding 39 mL of acetone, C3H6O, to 225 mL of water? The densities of acetone and water are 0.790 g/cm3 and 1.00 g/cm3, respectively.
A 1.00 mol/kg aqueous sulfuric acid solution, H2SO4,freezes at 4.04 C. Calculate i, the vant Hoff factor,for sulfuric acid in this solution.
What is the freezing point of a solution of dibromobenzene, C6H4Br2, in 0.250 kg of benzene, if the solution boils at 83.5 C?
The vapor pressures of several solutions of water-propanol (CH3CH2CH2OH) were determined at various compositions, with the following data collected at 45C: H2O Vapor pressure(torr) 0 74.0 0.15 77.3 0.37 80.2 0.54 81.6 0.69 80.6 0.83 78.2 1.00 71.9 a. Are solutions of water and propanol ideal? Explain. b. Predict the sign of Hsoln for water-propanol solutions. c. Are the interactive forces between propanol and water molecules weaker than, stronger than, or equal to the interactive forces between the pure substances? Explain. d. Which of the solutions in the data would have the lowest normal boiling point?
Distinguish between a strong electrolyte, a weak electrolyte, and a nonelectrolyte. How can colligative properties be used to distinguish between them? What is the vant Hoff factor? Why is the observed freezing-point depression for electrolyte solutions sometimes less than the calculated value? Is the discrepancy greater for concentrated or dilute solutions?

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