Chemistry Solutions: Types, Concentration & Colligative Properties: 31 flashcards
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1. What is a solution?
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A homogeneous mixture of two or more substances, with particles dispersed at the molecular or ionic level.
2. Define solute.
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The substance that dissolves in a solvent.
3. Define solvent.
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The substance that does the dissolving; usually present in greater amount.
4. What does 'like dissolves like' mean?
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Polar solvents dissolve polar and ionic solutes; nonpolar solvents dissolve nonpolar solutes.
5. Why does water dissolve salt?
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Water is polar; its molecules surround and stabilize the ions (hydration).
6. What is hydration?
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The process where water molecules surround and interact with solute particles (ions or molecules).
7. What is a saturated solution?
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A solution that contains the maximum amount of solute that can dissolve at a given temperature.
8. What is an unsaturated solution?
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A solution that can still dissolve more solute at a given temperature.
9. What is a supersaturated solution?
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A solution containing more dissolved solute than normally possible at that temperature; it is unstable.
10. How does temperature affect solubility of most solids?
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Solubility generally increases with temperature.
11. How does temperature affect solubility of gases?
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Solubility decreases as temperature increases.
12. What is concentration?
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The amount of solute in a given amount of solution or solvent.
13. Give the formula for mass percent.
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Mass percent = (mass of solute / mass of solution) × 100%
14. Give the formula for molarity (M).
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Molarity = moles of solute / liters of solution
15. Give the formula for molality (m).
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Molality = moles of solute / kilograms of solvent
16. Give the formula for parts per million (ppm).
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ppm = (mass of solute / mass of solution) × 10⁶
17. What is a dilute solution?
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A solution with a small amount of solute relative to the solvent.
18. What is a concentrated solution?
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A solution with a large amount of solute relative to the solvent.
19. Give an example of a gaseous solution.
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Air (a mixture of gases, mainly nitrogen and oxygen).
20. Give an example of a solid solution.
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Brass (a solid solution of zinc in copper).
21. Why do oil and water not mix?
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Oil is nonpolar and water is polar; they cannot form favorable interactions, so oil separates.
22. What is the difference between dissolving and melting?
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Dissolving is dispersal of solute particles in a solvent; melting is a change of state from solid to liquid due to heat.
23. Why are solutions transparent?
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Particles are too small (typically <1 nm) to scatter light significantly.
24. Why do solutions not settle on standing?
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Particles are dispersed at molecular/ionic level and are too small to settle under gravity.
25. What is the solvent in a solution of 10 mL ethanol and 90 mL water?
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Water, because it is present in the greater amount.
26. Why do reactions often proceed faster in solution?
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Dissolved particles move freely and collide more frequently.
27. What is an example of a solution in medicine?
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Intravenous (IV) fluids are carefully prepared solutions with precise concentrations.
28. What is an example of a solution in the environment?
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Seawater is a solution of various salts in water.
29. What is an example of a solution in biology?
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Blood plasma is a complex aqueous solution containing many solutes.
30. What is the general rule for predicting solubility?
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'Like dissolves like' — polar with polar/ionic, nonpolar with nonpolar.
31. What is a homogeneous mixture?
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A mixture with uniform composition throughout; components cannot be distinguished.
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