Ch 14: Acids and Bases

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77 Terms

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Lactic acid

Found in sour milk.

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Citric acid

Found in lemons.

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Acetic acid

Found in vinegar.

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Phosphoric acid

Found in carbonated beverages.

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Malic acid

Found in apples.

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Tartaric acid

Found in grape juice.

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Ammonia

Used for all types of cleaning.

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Sodium hydroxide

Also known as lye

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Magnesium hydroxide

Also known as milk of magnesia

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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.
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Single replacement reaction

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

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Binary acid

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

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Oxyacid

An acid that is a compound of hydrogen

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Sulfuric acid

Most commonly produced industrial chemical

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Nitric Acid

Very volatile

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Hydrochloric Acid

Produced by the stomach to aid in digestion

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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.
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Svante Arrhenius

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

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Arrhenius acid

A chemical compound that increases the amount of hydrogen ions

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Arrhenius base

a substance that increases the concentration of hydroxide ions

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Aqueous acids

Water solutions of acids.

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Strong acid

ionizes completely in aqueous solution and is a strong electrolyte.

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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.

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Weak acid

weak electrolyte

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

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Example of weak acid

H3PO4

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

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Organic acids

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

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Alkaline

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

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Example of strong base

NaOH.

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Sodium

an alkali metal

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

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Strong bases

strong electrolytes.

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Alkalinity

depends on the concentration of hydroxide ions in solution

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Example of weak base

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

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Bronsted-Lowery acid

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

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Example of Bronsted-Lowery acid

Hydrochloric acid

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Bronsted-Lowery base

a molecule or ion that is a proton acceptor.

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Bronsted-Lowery reaction

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

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Monoprotic acid

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

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Examples of monoprotic acids

HCl

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Polyprotic acid

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

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Example of diprotic acid

H2SO4 (sulfuric acid).

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Example of triprotic acid

H3PO4 (phosphoric acid).

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Conjugate base

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

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Conjugate acid

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

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Strength of conjugate acids and bases

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

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the stronger a base is

the weaker its conjugate acid.

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Amphoteric compounds

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

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Neutralization

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

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Salt

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

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Spectator ions

ions that do not participate in the overall reaction.

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Net ionic equation

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

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Acid rain

precipitation that occurs when gases such as NO

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Calcium carbonate reaction with acid

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

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Hydriodic acid

HI

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Iodide ion

I-

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Perchloric acid

HClO4

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Perchlorate ion

ClO4-

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Hydrobromic acid

HBr

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Bromide ion

Br-

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Chloride ion

Cl-

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Hydrogen sulfate ion

HSO4-

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Nitrate ion

NO3-

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Acetate ion

CH3COO-

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Carbonic acid

H2CO3

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Hydrogen carbonate ion

HCO3-

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Hydrosulfuric acid

H2S

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Hydrosulfide ion

HS-

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Dihydrogen phosphate ion

H2PO4-

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Hydrogen phosphate ion

HPO4^2-

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Hypochlorous acid

HClO

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Hypochlorite ion

ClO-

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Ammonium ion

NH4+

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Hydroxide ion

OH-

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Amide ion

NH2-

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Hydride ion

H-