Module 7 Study Guide
Module 7 Exam Review ANSWER KEY
1. Define acid. (7.01)
An acid is a substance that produces hydrogen ions, H+ or hydrodium ionsH3O+ in solution.
2. Compare the three theories of acids. (7.01)
An Arrhenius acid is a substance the increases the concentration of hydrogen ion, H+ or hydronium ions H3O+when dissolved in water. You must have water. A BrØnsted-Lowry acid is any substance that donates a hydrogen ion, H+ to another substance. A Lewis acid is any substance that accepts a lone pair of electrons. Yes, this is the same Lewis that wrote the Lewis Dot Structures in module 3.
3. What makes an acid to be classified as a ‘strong’ acid? (2.01)
A strong acid is one that breaks apart close to 100% when in solution. HCl is an example. When HCl is dissolved in water, it breaks apart into H+ and Cl- ions. Not all acids break apart. Those chemicals that do not break apart well are considered ‘weak’ acids.
4. List three general properties of acids. (7.01)
Acids have a sour taste, they are corrosive, acids are electrolytes, acids react with active metals (group 1 or 2) to produce hydrogen gas, H2 and acids react with bases to produce salt and water.
5. Compare the three theories of bases. (7.01)
An Arrhenius base is any substance that increases the concentration of hydroxide ions (OH-) when dissolved in water. A BrØnsted-Lowry base is one that accepts a hydrogen ion, H+. A Lewis base is any substance that donates a lone pair of electrons.
6. List 2 weak acids. (7.01)
Ammonia, NH3 and pyridine, C5H5N
7. List three general properties of bases. (7.01)
Bases have a bitter taste, bases react with acids to produce salt and water (also called a neutralization reaction), and solutions that are basic feel slippery.
8. Identify the BrØnsted-Lowry acid and base in the forward reaction below. (7.01)
HCl + NaHCO3 H2CO3 + NaCl
HCl is the BrØnsted-Lowry acid; NaHCO3 is the BrØnsted-Lowry base.
9. Write the neutralization reaction of
1. Define acid. (7.01)
An acid is a substance that produces hydrogen ions, H+ or hydrodium ionsH3O+ in solution.
2. Compare the three theories of acids. (7.01)
An Arrhenius acid is a substance the increases the concentration of hydrogen ion, H+ or hydronium ions H3O+when dissolved in water. You must have water. A BrØnsted-Lowry acid is any substance that donates a hydrogen ion, H+ to another substance. A Lewis acid is any substance that accepts a lone pair of electrons. Yes, this is the same Lewis that wrote the Lewis Dot Structures in module 3.
3. What makes an acid to be classified as a ‘strong’ acid? (2.01)
A strong acid is one that breaks apart close to 100% when in solution. HCl is an example. When HCl is dissolved in water, it breaks apart into H+ and Cl- ions. Not all acids break apart. Those chemicals that do not break apart well are considered ‘weak’ acids.
4. List three general properties of acids. (7.01)
Acids have a sour taste, they are corrosive, acids are electrolytes, acids react with active metals (group 1 or 2) to produce hydrogen gas, H2 and acids react with bases to produce salt and water.
5. Compare the three theories of bases. (7.01)
An Arrhenius base is any substance that increases the concentration of hydroxide ions (OH-) when dissolved in water. A BrØnsted-Lowry base is one that accepts a hydrogen ion, H+. A Lewis base is any substance that donates a lone pair of electrons.
6. List 2 weak acids. (7.01)
Ammonia, NH3 and pyridine, C5H5N
7. List three general properties of bases. (7.01)
Bases have a bitter taste, bases react with acids to produce salt and water (also called a neutralization reaction), and solutions that are basic feel slippery.
8. Identify the BrØnsted-Lowry acid and base in the forward reaction below. (7.01)
HCl + NaHCO3 H2CO3 + NaCl
HCl is the BrØnsted-Lowry acid; NaHCO3 is the BrØnsted-Lowry base.
9. Write the neutralization reaction of