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Acids & Bases

This guide explores the strength of acids and bases, distinguishing between strong and weak types. Strong acids like HCl and H2SO4 completely ionize in solutions, while weak acids do not fully dissociate. Similarly, strong bases dissociate entirely into metal ions and hydroxide ions, while weak bases like ammonia only partially react with water. We also discuss indicators such as litmus paper and phenol red, which reveal pH levels. Furthermore, we examine neutralization reactions, the process of titration, and the role of buffers in maintaining pH stability.

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Acids & Bases

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  1. Acids & Bases Strength & Neutralization

  2. Acid Strength • Strong Acids -completely ionize in an aqueous solution • Ex. HCl, H2SO4 • Weak Acids - only slightly ionize in an aqueous solution

  3. Base Strength • Strong Bases – completely dissociate into metal ions & hydroxide ions in aqueous solution • NaOH • Weak Bases – react w/ water to form hydroxide ions & the conjugate acid • Ammonia

  4. Types of Indicators • Litmus paper • Acids – Blue turns to Red • Bases – Red turns Blue • Phenol Red • Acids turn YELLOW • Bases turn PINK • pH paper • Tests all 14 pH levels, each having a different color

  5. Neutralization Rxns • Acid + Base = Salt + Water • Remember “Salts” are compounds made of an anion from an acid & a cation from a base!

  6. Titrations • A way to find the concentration of one solution, when you know the concentration of the other solution….

  7. Buffers • A solution of a weak acid & a weak base • A buffer keeps the pH relatively constant if a small amt of acid or base is added

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