Acids and Bases: Arrhenius vs Bronsted-Lowey

Today we learned the difference between acids and bases; everything from the physical characteristics to their chemical makeup. We also learned the difference between Arrhenius and Bronsted-Lowery bases and acids. Below is a quick overview of what we learned:

Physical Properties

• Acids- taste sour, feel sticky, show red or pink on litmus paper
• Bases- taste bitter, feel slippery, show blue on litmus paper

Arrhenius Acids and Bases

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• Acids- produce hydrogen ions in solution (H+) [HCL--> H+ + Cl-]
• Bases- produce hydroxide ions in solution (OH-) [NaOH--> Na+ + OH-]
• Amphitheater substance- can be an acid or a base  [water]

Bronsted-Lowery Acids and Bases

• Acids- donate a proton (H+)
• Bases- accept a proton (H+)
• Conjugate acid- substance formed when a proton is added to a base
• Conjugate base- remaining substance when a proton is lost from an acid

******* Acids produce conjugate bases, Bases produce conjugate acids********
Acid Strength

• List of Strong Acids
• Perchloric acid (HClO4)
• Chloric acid (HClO3)
• Hydrochloric acid (HCl)
• Hydrobromic acid (HBr)
• Hydroiodic acid (HI)
• Nitric acid (HNO3)
• Sulfuric acid (H2SO4) 

If the oxygen outnumbers the hydrogen by two or more, it is considered a strong acid.

For more information or practice use the links below:
Detailed Explanation with Examples
Video explanation
Shorter video
Quiz Yourself