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I. Introduction to Acids & Bases

Acids & Bases. I. Introduction to Acids & Bases. electrolytes  electrolytes. A. Properties. ACIDS. BASES. bitter taste. sour taste. turn litmus red. turn litmus blue. react with metals to form H 2 gas. slippery feel. vinegar, milk, soda, apples, citrus fruits.

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I. Introduction to Acids & Bases

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  1. Acids & Bases I. Introduction toAcids & Bases

  2. electrolytes electrolytes A. Properties ACIDS BASES • bitter taste • sour taste • turn litmus red • turn litmus blue • react with metals to form H2 gas • slippery feel • vinegar, milk, soda, apples, citrus fruits • ammonia, lye, antacid, baking soda ChemASAP

  3. H H – + O O Cl Cl H H H H B. Definitions Acidsform hydronium ions (H3O+) HCl+ H2O  H3O+ + Cl– acid

  4. H H – + N O O N H H H H H H H H B. Definitions • Bases form hydroxide ions (OH-) NH3+ H2O  NH4+ + OH- base

  5. B. Definitions • Amphoteric - can be an acid or a base. • MonoproticAcid – can donate only one proton (H+) per molecule. • Examples: HCl, HNO3 • Polyprotic Acid – can donate more than one proton (H+) per molecule. • Example: H2SO4 (diprotic) • H3PO4 (triprotic)

  6. - + C. Strength • Strong Acid/Base • 100% ionized in water • strong electrolyte HCl HNO3 H2SO4 HBr HI HClO4 NaOH KOH Ca(OH)2 Ba(OH)2

  7. - + C. Strength • Weak Acid/Base • does not ionize completely • weak electrolyte HF CH3COOH H3PO4 H2CO3 HCN NH3

  8. E. Neutralization Reactions Strong acid + Strong base  Salt + Water Ex. HCl(aq) + NaOH(aq) NaCl(aq)+ H2O

  9. Acids & Bases II. Aqueous Solutions and the Concept of pH

  10. H2O + H2O H3O+ + OH- A. Self-Ionization of Water Water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton.

  11. B. Neutral, Acidic, and Basic Solutions • Any solution in which [H3O+] = [OH-] isneutral. • Any solution in which [H3O+] > [OH-] isacidic. • Any solution in which [H3O+] < [OH-] is basic.

  12. pouvoir hydrogène (Fr.) “hydrogen power” C. The pH Scale 14 0 7 INCREASING BASICITY INCREASING ACIDITY NEUTRAL pH = -log[H3O+]

  13. C. The pH Scale pH of Common Substances

  14. C. The pH Scale pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14

  15. pH • pH = -log [H+] • [H+] = 10-pH • pOH = -log [OH-] • pH + pOH = 14

  16. Calculations with pH Q: What is the pH if [H+]= 6.3 x 10–5? pH = –log [H+] ‘(-)’, ‘log’, ‘6.3’, ‘EE’, ‘(-)’, ‘5’, ‘)”, ‘ENTER’) Ans: 4.2 Q: What is the [H+] if pH = 7.4? [H+] = 10–pH mol/L (’10x’, ‘(-)’, ‘7.4’, “)” ‘ENTER‘) 3.98x10–8 M

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