Chapter 4 – Types of Reactions and Solution Stoichiometry Name: ______
1) What does it mean that water is polar?
2) How does water’s polarity affect the process of “hydration”?
3) There are two parts to every solution, called the solute and solvent. Describe the difference between them.
4) There are three ways to describe “electrolytes”. Describe the difference between them.
5) When an acid or base is considered “strong” what does that term imply?
6) List some examples of strong acids.
7) What “ion” must be present to classify something as a base?
8) List some examples of strong bases.
9) When an acid or base are considered “weak” what does that term imply?
10) List some examples of weak acids.
11) List some examples weak bases.
12) What is the term used to describe the concentration of a solution?
13) What is the mathematical way to express the above term?
14) What is happening to a solution when it is being diluted?
15) How does the number of moles of the solute change during dilution?
16) What is the equation used when calculating molarity and volume during a dilution? (pg 139)
17) Describe a precipitation reaction.
Take note of the solubility rules in table 4.1 on page 144. You will not need to memorize these, but you do need to be familiar with how to determine if something is soluble or not.
18) How does the complete ionic equation different from the formula equation?
19) In general, how would you identify/classify something as a “spectator ion”?
20) What is included in the “net ionic equation”?
21) What are the 6 steps involved when solving stoichiometry problems for reactions in solution?
STOP READING THE CHAPTER AFTER YOU FINISH THIS QUESTION! We will cover the rest in class at later points in the year. Skip to the end of the chapter and start with the selected questions from the textbook on page 171.