Section 6.1 – 6.4, 6.7 Study Guide
Section 6.1 – Solutions & Electrolytes
1. The process of water molecules pulling away the ions from an ionic compound is called
_________, and it is what occurs when an ionic compound dissolves in water.
2. T or F: When a substance dissolves in water it disappears.
3. The process of breaking up an ionic compound into the separate ions is called
__________ or ____________.
4. Why does pure water not conduct electricity?
5. A ______________ solution has more solute particles dissolved in it than it ordinarily
would have been able to hold.
6. A _________ solution has dissolved all the solute that it can hold.
7. If a solution is holding less than the maximum amount of solute that can be dissolved in
it, it is ___________.
8. Break down the following strong electrolytes into ions.
a.
Al(NO3)3
b.
FeSO4
Section 6.2 – Concentrations of Solutions
9. Find the %(W/V) of a sample that has 5 g solute in 200 mL of solution.
10. Find the molarity of a solution that has 15 g NaOH dissolved in 225 mL of solution.
11. A 250 mL sample is .5 M CaCl2. Find the %(W/V).
Section 6.3 – Acidity & pH
12. A strong base is one in which all the molecules of the base produce _________ ions.
13. If the concentration of hydronium is greater than the concentration of hydroxide, the
sample will be ______.
14. Find the hydroxide concentration of a solution with a pH of 11.6.
Section 6.4 – Solubility & Precipitation
15. Ions that bond with other ions in a solution, form an insoluble compound called a
___________.
16. Finish the following equation: CaCl2 + AgNO3 
Be sure to balance the equation and state the state of matter for each product and reactant.
Section 6.7 – Properties of Solutions
17. The process of a liquid changing to a gas is called ___________.
18. The vapor pressure of a solution is always _____ than the vapor pressure of the pure
solvent.
19. Solutions always boil at ______ temperatures than pure solvents.
20. When a substance’s solid phase and liquid phase are in equilibrium, that substance is at
its ________ _____.
21. The freezing point of a solution will always be _____ than for the pure liquid.
22. Calculate the freezing point of a solution of 5 g of C12H10 and 7.5 g of C10H8 dissolved in
200 g of benzene, (has a freezing point of 5.5 °C).