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Hydrogen Ions and acidity

Hydrogen Ions and acidity. Unit 13 Chapter 19-2. 1 more definition of acids and bases. Lewis acids and bases Acid: accepts a pair of electrons Base: donates a pair of electrons. Self-ionization. A rxn where water molecules produce ions. Neutral Solutions.

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Hydrogen Ions and acidity

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  1. Hydrogen Ions and acidity Unit 13 Chapter 19-2

  2. 1 more definition of acids and bases • Lewis acids and bases • Acid: accepts a pair of electrons • Base: donates a pair of electrons

  3. Self-ionization • A rxn where water molecules produce ions

  4. Neutral Solutions • In water the [OH-] and the [H+] is 1X10-7M….so they are equal in concentration • Neutral solutions contain equal amounts of OH- ions and H+ ions

  5. Ion product • Naturally as you inc the [H+] the [OH-] dec • The [OH-] and [H+] has to equal 1.0 X10-14 • Kw = ion-product constant for water Kw = [H+] X [OH-] = 1.0 X10-14

  6. Acidic solutions • Solution where the [H+] ions are larger than the [OH-] ions

  7. Basic/ alkaline solutions • Solution where the [H+] ions are less than the [OH-] ions.

  8. The pH concept • Soren Sorensen created the pH scale • pH scale ranges from 0-14 • 7= neutral • 0 = strongly acidic • 14 = strongly basic

  9. The pH concept • pH is the negative logarithm of [H+]. • pH = -log[H+] • pOH = -log[OH-] • for water solutions, pH + pOH = 14

  10. Acid-base indicator • An indicator is a dye that changes a particular color depending on the acidity of the solution • Fig 19-12, P602 • pH meters

  11. Indicators important to lab

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