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Chemistry 102 OUTLINE FOR ACID-BASE

Chemistry 102 OUTLINE FOR ACID-BASE. I. WATER. A. Nature and Composition B. Importance in Acid-Base Chemistry 1. Acid : Proton Donor 2. Base : Proton Acceptor 3. Autoionization 4. K w = 1 x 10 -14. II. pH SCALE.

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Chemistry 102 OUTLINE FOR ACID-BASE

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  1. Chemistry 102OUTLINE FOR ACID-BASE

  2. I. WATER A. Nature and Composition B. Importance in Acid-Base Chemistry 1. Acid : Proton Donor 2. Base : Proton Acceptor 3. Autoionization 4. Kw = 1 x 10-14

  3. II. pH SCALE A. Technical Definition : Acidic = 0 – 7.0 Practical Definition : Acidic = 0 - 6.5 B. Technical Definition : Basic = 7.0 - 14 Practical Definition : Basic = 7.5 – 14 C. Technical Definition : Neutral = 7.0 Practical Definition : Neutral = 6.5 - 7.5

  4. III. ACIDS A. Know These Five Strong Acids : HCl, HBr, HNO3, HClO4 and H2SO4 B. Weak Acids : Ka (partial dissociation) and pKa : HC2H3O2(acetic acid) C. Polyprotics : H2CO3(carbonic acid) and H3PO4 (phosphoric acid)

  5. IV. BASES A. Know These Five Strong Bases : LiOH, NaOH, KOH, Mg(OH)2 and Ca(OH)2 B. Weak Bases : Kb (partial dissociation) and pKb : NH3(ammonia)

  6. V. CONJUGATE ACID-BASE PAIRS A. Weak Acid plus the conjugate base of that same weak acid. B. Weak Base plus the conjugate acid of that same weak base. C. Ka x Kb = Kw D. pKa + pKb = 14

  7. VI. SALTS A. Salts Of Weak Acids : "ARE BASIC“ B. Salts Of Weak Bases : "ARE ACIDIC“ C. Neutral Salts : "CATION FROM STRONG BASE AND ANION FROM STRONG ACID"

  8. VII. USING ICE DIAGRAMS FOR ACID-BASE PROBLEMS : You may ignore the "-x" value in the Equilibrium Concentration [E] VIII. PRACTICE PROBLEM SET PLUS KEY IX. PRACTICE QUIZ PLUS KEY X. QUIZ PLUS KEY

  9. XI. HINTS FOR USE OF SIGNIFICANT FIGURES IN ACID-BASE PROBLEM SOLVING SITUATIONS : A. In calculating a pH of a solution with a pH between 0 – 1 : Use the same number of significant figures as in the hydrogen ion concentration! Example: for a 0.11 M solution of acid the pH would be 0.96 (2 sig figs). B. In calculating a pH of a solution with a pH between 1 – 10 : Use one more significant figure as in the hydrogen ion concentration! Example: for a 0.011 M solution of acid the pH would be 1.96 (3 sig figs). C. In calculating a pH of a solution with a pH between 10 – 14 : Use two more significant figures as in the hydrogen ion concentration! Example: for a 1.1 x 10-12 M solution of acid the pH would be 11.96 (4 sig figs). D. The same logic will apply for calculating pOHs, pKas and pKbs.

  10. XII. ACID-BASE WORKSHEET pH = -log [H+] pOH = -log [OH-] pH + pOH = 14 Kw = [H+] x [OH-] Kw = Ka x Kb = 1.0 x 10-14 pKa = -log Ka pKb = -log Kb pKa + pKb = 14 [conjugate base] pH = pKa + log____________________________________ [acid]

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