Name: ______Pretest: ______/33
Posttest: ______/33
Solubility and Concentration Pretest
1. ______a measure of how well one A. concentration
substance dissolves in anotherB. hydrogen bond
2. ______something that has partially chargedC. nonpolar compound
molecules; will dissolve in waterD. polar compound
3. ______a liquid into which things are dissolvedE. saturated
F. solubility
4. ______the exact amount of solute dissolved G. solute
in a given solventH. solvent
5. ______a solution that holds more solute thanI. supersaturated
it usually can at a given temperatureJ. unsaturated
6. ______a solution that is holding all it can at
that temperature
7. ______forms between the hydrogen of one water molecule and the oxygen of another because of their partial charges
8. ______a solution that can hold more solute at that temperature
9. ______substance dissolved in a liquid to make a solution
10. ______has no partial charges; will not dissolve in water
11. – 12. I mix up a solution of some Kool Aid by using the mix, sugar and water.
Whatis the solute and what is the solvent?
13. I add some more sugar to the Kool Aidfrom 11. – 12. and it dissolves. Was the
original liquid saturated, unsaturatedor supersaturated? Explain.
14. – 15. Describe what would’ve happened for the other two terms above.
Use the graph at the right for #16 – 20.
16. ______How many grams of
NH3 are needed to make a saturated
solution in 100 g of water at 20 °C?
17. ______In terms of
saturation, how would you classify a NaNO3 solution with a concentration of
90 g / 100 g of water at 50 °C?
18. ______If we lowered the
temperature to 10 °C, what would its saturation be?
19. ______At what
temperature is the solubility of NaCl the same as that of KClO3?
20. ______Which is more
soluble in water, NaCl or NaNO3? How can you tell?
21. – 22. As you raise the temperature of a solvent, how does the solubility of a
solute change if it is a
Solid? Explain why.
Gas? Explain why.
23. Are any of the substances gases? Explain.
How do the following affect the process of dissolving, at a molecular level?
24. Stirring/shaking?
25. Breaking it into smaller pieces?
26. Heating the solvent?
27. – 28. Draw a water molecule. Explain why water is a polar molecule using your
drawing.
29. Draw the hydrogen bond that occurs with water molecules.
30. Describe how/why “like dissolves like.”
Concentration = mass of solute / volume of solvent
31. ______What is the concentration of 42.1 grams of silver nitrate that
dissolves in 1750 mL of water?
32. ______How many grams of salt will dissolve in 350 mL of water if
the solubility of salt is 359 g / 100. mL of H2O? (try
using a proportion)
33. ______If the solubility of KNO3 is 180 g / 100. mL of H2O, will 560 g
dissolve in 400 mL of H2O?(try using a proportion)