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Basic Chemistry Practice Test: Properties of Solutions
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Here are some properties of solutions: Homogeneous mixture: A solution is a homogeneous mixture of two or more substances. The particles of a solution are smaller than 10-9 meters in diameter and are too small to be seen by the naked eye. All components of a solution appear as a single phase. Colligative properties: These are the physical changes that occur when a solute is added to a solvent. Colligative properties are determined by the number of solute particles present, as well as the amount of solvent present. Solubility: This is the ability of a compound to dissolve in water. The... Show more
Basic Chemistry Practice Test: Properties of Solutions
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25 Questions

1. Which of the following cannot be a colloid?
2. If the partial pressure of oxygen in the air a diver breathes is too great, __________.
3. A solution containing 10.0 g of an unknown liquid and 90.0 g water has a freezing point of -3.33 °C. Given Kf = 1.86°C/m for water, the molar mass of the unknown liquid is ________ g/mol.
4. At 20°C, an aqueous solution that is 24.00% by mass in ammonium chloride has a density of 1.0674 g/mL. What is the molarity of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol.
5. When solutions of strong electrolytes in water are formed, the ions are surrounded by water molecules. These interactions are best described as a case of __________.
6. Which component of air is the primary problem in a condition known as 'the bends?'
7. Molality is defined as the __________.
8. The dissolution of water in octane (C8H18 ) is prevented by __________.
9. The process of solute particles being surrounded by solvent particles is known as __________.
10. Hydrophobic colloids __________.
11. The concentration (M) of HCl in a solution prepared by dissolving 5.5 g of HCl in 200 g of C2H6O is__________ M. The density of the solution is 0.79 g/mL.
12. A solution is prepared by dissolving 15.0 g of NH3 in 250 g of water. The density of the resulting solution is 0.974 g/mL. The molarity of NH3 in the solution is __________.
13. Which of the following choices has the compounds correctly arranged in order of increasing solubility in water? (least soluble to most soluble)
14. Hydration is a specific example of the phenomenon known generally as __________.
15. A sample of potassium nitrate (49.0 g) is dissolved in 101 g of water at 100 °C with precautions taken to avoid evaporation of any water. The solution is cooled to 30.0 °C and a small amount of precipitate is observed. Thissolution is __________.
16. The mole fraction of He in a gaseous solution prepared from 4.0 g of He, 6.5 g of Ar, and 10.0 g of Ne is __________.
17. A solution is prepared by dissolving 16.2 g of benzene (C6H6 ) in 282 g of carbon tetrachloride (CCl4 ) The concentration of benzene in this solution is __________ molal. The molar masses of C6H6 and CCl4 are 78.1 g/mol and 154 g/mol, respectively.
18. A solution contains 15 ppm of benzene. The density of the solution is 1.00 g/mL. This means that __________.
19. Calculate the freezing point of a solution containing 40.0 grams of KCl and 4400.0 grams of water. The molalfreezing-point-depression constant (Kf ) for water is 1.86 °C/m.
20. Formation of solutions where the process is endothermic can be spontaneous provided that __________.
21. Which one of the following is most soluble in hexane (C6H14 ) ?
22. The concentration of KBr in a solution prepared by dissolving 2.21 g of KBr in 897 g of water is __________ molal.
23. Which of the following substances is more likely to dissolve in CH3OH ?
24. A solution contains 11% by mass of sodium chloride. This means that __________.
25. Pressure has an appreciable effect on the solubility of __________ in liquids.

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