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Acids and Bases

Acids and Bases. 1) Properties and examples 2) Theories 3) pH scale 4) Indicators 5) Neutralization 6) Molarity. Acids Properties and Examples. 1) Have a sour taste 2) React with metals 3) Contain Hydrogen 4) Formed from non metals. Acids Properties and Examples.

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Acids and Bases

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  1. Acids and Bases 1) Properties and examples 2) Theories 3) pH scale 4) Indicators 5) Neutralization 6) Molarity

  2. AcidsProperties and Examples • 1) Have a sour taste • 2) React with metals • 3) Contain Hydrogen • 4) Formed from non metals

  3. AcidsProperties and Examples • 5) Form hydronium ions in water (H3O+) • 6) Poisonous and corrosive to the skin • 7) Conducts electricity in water (electrolytes)

  4. Acids (cont.) • 8) Forms ionic bonds • 9) Turns blue litmus paper red

  5. EXAMPLES • acetic acid - vinegar (from grapes and apples) • lactic acid - milk, butter milk, sour cream

  6. EXAMPLES • citric acid - citrus fruits • hydrochloric acid- muratic, cleaning, stomach acid

  7. Acids (cont.) • nitric acid - a dehydrator, turns skin yellow

  8. Acids (cont.) • sulfuric acid - battery acid, dehydrator • The number one chemical produced in the US. More sulfuric acid is produced than any other compound.

  9. BasesProperties and Examples • 1) Taste bitter • 2) Feel slippery • 3) Poisonous and corrosive to the skin

  10. BasesProperties and Examples • 4) Contains a metal, hydrogen and oxygen (except for ammonia NH3) • 5) Forms the OH- ion (hydroxide) in water • 6) conducts electricity (electrolyte) in water

  11. Bases (cont.) • 7) Dissolves oils and fats • 8) forms ionic bonds • 9) Turns red litmus paper blue

  12. EXAMPLES • sodium hydroxide - lye, drain cleaner, used to make soap, hair treatment • calcium hydroxide - tums antacid • aluminum hydroxide -antiperspirant, Rolaids antacid

  13. Acid-BaseTheories • Arrhenius • acid = releases H+ ions in water • base = releases OH- ions in water • Bronsted / Lowery • acid = proton donor H+ • base = proton acceptor • Lewis (organic acids and bases) • acid = electron pair acceptor • base = electron pair donor

  14. Conjugate Acids and bases • HCl + NaOH <=> NaCl + H+ (OH-) • acid base con. base con. acid • conjugate acids = product side, contains the proton from the acid and the (-) part of the base. • conjugate base = product side, contains the (+) part of the base and the (-) part of the acid.

  15. Neutralization • When an acid reacts with a base a salt and water is formed. The salt is the CB and the water is the CA. • HCl + KOH <=> H(OH) + KCl • A B water salt • salts are not always NaCl

  16. Anhydrides • Basic anhydrides = are formed when water is removed from a base • Acidic anhydrides = are formed when water is removed from an acid • The problem of acid rain is a result of acidic anhydrides being formed when high sulfur coal is burned. The anhydrides combine to form sulfuric acid.

  17. Indicators • Are weak acids that will turn different colors in acid and base solutions. • Examples • Litmus: red turns blue in a base • blue turns red in an acid • Phenolpthalein: clear in an acid / red in a base • Methyl Orange: turns red to yellow in a pH range of 3.1 to 4.4 • Red Cabbage: variety of colors from acids to bases

  18. pH scale pH is the measurement of the number of H3O+ ions in a solution. Distilled water has 1 x 10 -7 H3O+ ions. Using the -log the pH = 7 pH range 1………....…...…6.9…....7…...7.1……………......14 acid neutral base

  19. Common Substances • Stomach acid = 1.6 • vinegar = 2.8 • apples =3.0 • orange juice = 3.5 • carrots = 5.0 • urine = 6.0 • milk = 6.5 • blood = 7.35 • sea water = 8.4 • milk of magnesia antacid = 10.5

  20. Titration • In the reaction of an acid with a base an indicator is used to detect the pH change. • By carefully measuring the amount of acid or base used to cause the color change we can tell the number of moles used. • Then a mass:mass problem can be used to determine the amount of the unknown compound.

  21. Molarity • solute = what gets dissolved • solvent = what does the dissolving • moles of solute / 1 liter of solvent • grams / 1000 ml

  22. STRONG ACIDS H2(SO4)H(ClO4) H(NO3)HBr HI HCl WEAK ACIDS H3(PO4) H2(CO3) CH3COOH H2S STRONG BASES Ca(OH)2 Sr(OH)2 Ba(OH)2 Na(OH) K(OH) Rb(OH) Cs(OH) Mg(OH)2 WEAK BASES NH3 ACID BASE STRENGTH

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