Acids and Bases

Theories:

Arrhenious- Definition: Acids are substances that increase the concentration of hydrogen ions (H+) in aqueous solution, while bases increase the concentration of hydroxide ions (OH-) in solution.

Bronsted-Lowry - Definition: Acids are proton donors, while bases are proton acceptors, broadening the understanding of acid-base reactions beyond just aqueous solutions.

Binary Acid Names:

Hydroflouric Acid - HF

Hydrochloric Acid - HCl

Hydrobromich Acid - HBr

Hydroiodic Acid - HI

Hydrosulfaric Acid - H2S

Weak Acids

HF, H2CO3, H3PO4, H3AsO4, HClO3, HClO2, HClO

6 Most Important Strong Acids

HCl, HBr, HI, HClO4, HNO3, H2SO4

Strong Acids- Acids that ionize completely when dissolved in water

  • strong acids have very weak bonds, weak acids have stronger bonds

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Strong Bases- All metal hydroxides are strong bases

Weak Bases- All bases related to ammonia are weak acids

Anhydrides- means “without water”

  • Acid anhydrides are often the oxides of nonmetals

  • Basic anhydrides are the oxides of metal

Neutralization Reactions- The reactions between acids and bases are called neutralization reactions