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Neutralization & pH

Acids & Bases. Neutralization & pH. A. Neutralization Reactions. Acids react with bases to produce a salt and water NaOH ( aq ) + HCl ( aq ) → NaCl + H 2 O base acid salt water Ca (OH) 2 + 2 HCl → CaCl 2 + 2H 2 O base acid salt water.

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Neutralization & pH

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  1. Acids & Bases Neutralization & pH

  2. A. Neutralization Reactions • Acids react with bases to produce a salt and water NaOH (aq) + HCl(aq) →NaCl + H2O base acid salt water Ca(OH)2 + 2 HCl→ CaCl2 + 2H2O base acid salt water

  3. A. Neutralization • Acid + Base Salt + Water • HCl + NaOH  NaCl + HOH salt water

  4. H2O + H2O H3O+ + OH- B. Acid-Base Properties of Water Hydronium ion Hydroxide ion Conjugate acid Conjugate base acid base

  5. Kw = [H3O+][OH-] = 1.0  10-14 • [ ] = Concentration (Molarity) Solution Is [H+] = [OH-] neutral [H+] > [OH-] acidic [H+] < [OH-] basic

  6. B. Ionization of Water • Find the hydroxide ion concentration of 3.0  10-2 M HCl. Given: [H3O+][OH-] = 1.0  10-14 Do acids produce H3O+ ions or OH- ions? [3.0  10-2][OH-] = 1.0  10-14 [OH-] = 3.3  10-13 M Acidic or basic? Acidic

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

  8. C. pH Scale pH of Common Substances

  9. C. pH Scale [H3O+] comes from the acid and [OH-] comes from the base pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14 [H3O+]= 10(-pH) [OH -] = 10(-pOH) [ ] always mean concentration (Molarity) [H3O+] and [H+] are the same thing!!

  10. C. pH Scale • What is the pH of 0.050 M HNO3? • Since HNO3 has 1 H+, then 0.050 M HNO3 = 0.050 M H+ pH = -log[H+] pH = -log[0.050] pH = 1.3 Acidic or basic? Acidic

  11. C. pH Scale • What is the [H+] in an HBr solution that has a pOH of 9.6? 10(–pH) = [H+] [H+] = 4.0  10-5 M HBr pH + pOH = 14 pH + 9.6 = 14 pH = 4.4 Acidic

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