Ch 14: Acids and Bases

Lactic acid

Found in sour milk.

Citric acid

Found in lemons.

Acetic acid

Found in vinegar.

Phosphoric acid

Found in carbonated beverages.

Malic acid

Found in apples.

Tartaric acid

Found in grape juice.

Ammonia

Used for all types of cleaning.

Sodium hydroxide

Also known as lye

Magnesium hydroxide

Also known as milk of magnesia

Properties of acids

1. Have a sour taste 2. Change the color of acid-base indicators 3. React with active metals to release hydrogen gas 4. React with bases to produce salts and water 5. Conduct electrical currents.

Single replacement reaction

Example: Ba(s) + H2SO4(aq) → Ba SO4 (aq) + H₂ (g).

Binary acid

An acid that contains only 2 different elements: Hydrogen and a more electronegative element.

Oxyacid

An acid that is a compound of hydrogen

Sulfuric acid

Most commonly produced industrial chemical

Nitric Acid

Very volatile

Hydrochloric Acid

Produced by the stomach to aid in digestion

Properties of Bases

1. Taste bitter 2. Change color in an acid base indicator 3. Feel slippery 4. React with acids to produce salt and water 5. Conduct electric current.

Svante Arrhenius

Swedish chemist who theorized that acids and bases produce ions in solution.

Arrhenius acid

A chemical compound that increases the amount of hydrogen ions

Arrhenius base

a substance that increases the concentration of hydroxide ions

Aqueous acids

Water solutions of acids.

Strong acid

ionizes completely in aqueous solution and is a strong electrolyte.

Acid strength

depends on the polarity of the bond between hydrogen and the element it is bonded to and the ease with which that bond can be broken.

Weak acid

weak electrolyte

the amount of hydrogens on a molecule does not affect strength.

Example of weak acid

H3PO4

none of these ionize completely so it is a weak acid.

Organic acids

contain acidic carboxyl group (-COOH) and are weak.

Alkaline

when a base completely dissociates in water to yield aqueous (OH) ions.

Example of strong base

NaOH.

Sodium

an alkali metal

the group gets its name because when the elements combine with hydroxides they form alkaline solutions.

Strong bases

strong electrolytes.

Alkalinity

depends on the concentration of hydroxide ions in solution

Example of weak base

Ammonia (NH3) is highly soluble but a weak electrolyte.

Bronsted-Lowery acid

a molecule or ion that is a proton donor (H+).

Example of Bronsted-Lowery acid

Hydrochloric acid

Bronsted-Lowery base

a molecule or ion that is a proton acceptor.

Bronsted-Lowery reaction

proton transferred from one reactant (the acid) to another reactant (the base).

Monoprotic acid

an acid that can donate only one proton (hydrogen ion) per molecule.

Examples of monoprotic acids

HCl

Polyprotic acid

an acid that can donate more than one proton per molecule.

Example of diprotic acid

H2SO4 (sulfuric acid).

Example of triprotic acid

H3PO4 (phosphoric acid).

Conjugate base

the species that remains after a Bronsted-Lowery acid has given up a proton.

Conjugate acid

the species that is formed when a Bronsted-Lowery base gains a proton.

Strength of conjugate acids and bases

depends on the strength of the acids and bases involved. The stronger an acid is

the stronger a base is

the weaker its conjugate acid.

Amphoteric compounds

any species that can react as either an acid or a base.

Neutralization

the reaction of hydronium ions and hydroxide ions to form water molecules.

Salt

an ionic compound composed of a cation from a base and an anion from an acid.

Spectator ions

ions that do not participate in the overall reaction.

Net ionic equation

an equation that shows only the species that actually change during the reaction.

Acid rain

precipitation that occurs when gases such as NO

Calcium carbonate reaction with acid

CaCO3 (s) + 2H3O+ (aq) → Ca²+ (aq) + CO2 (g) + 3H₂O (l)

Hydriodic acid

HI

Iodide ion

I-

Perchloric acid

HClO4

Perchlorate ion

ClO4-

Hydrobromic acid

HBr

Bromide ion

Br-

Chloride ion

Cl-

Hydrogen sulfate ion

HSO4-

Nitrate ion

NO3-

Acetate ion

CH3COO-

Carbonic acid

H2CO3

Hydrogen carbonate ion

HCO3-

Hydrosulfuric acid

H2S

Hydrosulfide ion

HS-

Dihydrogen phosphate ion

H2PO4-

Hydrogen phosphate ion

HPO4^2-

Hypochlorous acid

HClO

Hypochlorite ion

ClO-

Ammonium ion

NH4+

Hydroxide ion

OH-

Amide ion

NH2-

Hydride ion

H-