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

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

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

EXAMPLES citric acid - citrus fruits hydrochloric acid- muratic, cleaning, stomach acid

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

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

Bases Properties and Examples 1) Taste bitter 2) Feel slippery 3) Poisonous and corrosive to the skin

Bases Properties 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

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

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

Acid-Base Theories 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

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.

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

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.

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

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

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

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.

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

ACID BASE STRENGTH 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