Activitv 1.1.1. How does rise in temperature affect solubility of solids, liquidsand gases?2. How do colligative properties of solutions vary according toconcentration?Activity 1.2.1. Calculate the vapor pressure of a solution made by dissolving82.4 g of urea (molar mass = 60.06 g/mol) in 212 mL of water at35 °C. What is the vapor-pressure lowering?2. A solution of 0.85 gof an organic compound in 100.0 g of benzenehas a freezing point of 5.16 °C. What are the molality of thesolution and the molar mass of the solute?AssessmentChoose the letter of the correct answer. Write your answer on youranswer sheet.1. Which factor would NOT affect the solubility of sugar in water?A. add salt to the waterB. stir the water and sugar13C. heat the water and sugarD. grind the sugar to make it finer2. Which is NOT a property of solution?A. it consists of a single phaseB. it is a homogeneous mixtureC. it has a definite compositionD. components readily separate if left undisturbed for 24 hours3. Which is TRUE about colligative properties of solution?A. they have different originB. they depend on the nature of solutesC. solutes may be atoms, molecules, or ionsD. they depend on the number of solvent particles4. Which term refers to the temperature at which a solution's vapor pressureequals the external atmospheric pressure?A. melting pointB. boiling point5. A solution is prepared by dissolving 35.0 g of hemoglobin (Hb) in enough waterto make up 1 L in volume. If the osmotic pressure of the solution is found tobe 10.0 mmHg at 25 °C, what is the molar mass of hemoglobin?A. 5.38 X 104B. 8.21 X 10C. freezing pointD. sublimation pointC. 3.50 X 10D. 6.51 X 10

Activity- 1.1 - (1) On increasing the temperature of the Solution containing solid or liquid…

Activity 1.1. 1. How does rise in temperature affect solubility of solids, liquids and gases? 2. How do colligative properties of solutions vary according to concentration? Activity 1.2. 1. Calculate the vapor pressure of a solution made by dissolving 82.4 g of urea (molar mass = 60.06 g/mol) in 212 mL of water at 35 "C. What is the vapor-pressure lowering?

Activity 1.1. 1. How does rise in temperature affect solubility of solids, liquids and gases? 2. How do colligative properties of solutions vary according to concentration? Activity 1.2. 1. Calculate the vapor pressure of a solution made by dissolving 82.4 g of urea (molar mass = 60.06 g/mol) in 212 mL of water at 35 "C. What is the vapor-pressure lowering?

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter11: Properties Of Solutions

Section: Chapter Questions

Problem 6RQ: In terms of Raoults law, distinguish between an ideal liquid-liquid solution and a nonideal...

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In terms of Raoults law, distinguish between an ideal liquid-liquid solution and a nonideal liquid-liquid solution. lf a solution is ideal, what is true about Hsoln, T for the solution formation, and the interactive forces within the pure solute and pure solvent as compared to the interactive forces within the solution? Give an example of an ideal solution. Answer the previous two questions for solutions that exhibit either negative or positive deviations from Raoults law.
(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
You dissolve 1.0 mol of urea (H2NCONH2) in 270 g of water. The mole fraction of urea is (a) 3710 3 (b) 0.063 (c) 16 (d) 1.0 and its molality is (a) 1.0 (b) 3.7 (c) 0.063 (d) 0.27
The Henry's law constant for the solubility of radon in water at is 9.57106 M/mm Hg. Radon is present with other gases in a sample taken from an aquifer at 30C. Radon has a mole fraction of 2.7106 in the gaseous mixture. The gaseous mixture is shaken with water at a total pressure of 28 atm. Calculate the concentration of radon in the water. Express your answers using the following concentration units. (a) molarity (b) ppm (Assume that the water sample has a density of 1.00 g/mL.)
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You make 20.0 g of a sucrose (C12H22O11) and NaCl mixture and dissolve it in 1.00 kg water. The freezing point of this solution is found to be 0.426C. Assuming ideal behavior, calculate the mass percent composition of the original mixture, and the mole fraction of sucrose in the original mixture.
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