Section 14

Question 1

Acids were first recognized as a distinct class of compounds because their aqueous solutions have which five properties?

Answer 1

1. Aqueous solutions of acids have a sour taste. 2. Acids change color of acid-base indicators (red). 3. Some acids react with active metals and release hydrogen gas (H2). 4. Acids react with bases to produce salts and water (neutralization). 5. acids conduct electricity.

Question 2

Define a Binary Acid

Answer 2

Binary acid- an acid that contains only two different elements: hydrogen and one of the more electronegative elements.

Question 3

How do you name a binary acid?

Answer 3

The prefix is hyro-. The root of the name of the second element follow the prefix. The name then ends with -ic.

Question 4

Define oxyacid + 2 examples

Answer 4

Oxyacid- an acid that is a compound of hydrogen, oxygen, and a third element, usually a nonmetal. Examples, Nitric acid, HNO3 & Carbonic acid, H2CO3.

Question 5

List 5 Common Industrial Acids and briefly describe each.

Answer 5

(Most common) Sulfuric Acid- can be used to remove water from gases with which it does not react. (Also widely used) Nitric Acid- volatile, unstable liquid; suffocating odor, stain skin, and can cause serious burns. (Fertilizers) Phosphoric Acid- essential element used for plants and animals. (Digestion and Food) Hydrochloric Acid- stomach produced it to aid in digestion. (Food supplements) Acetic Acid- clear, colorless, and pungent-smelling liquid

Question 6

What are the five properties of bases?

Answer 6

1. Aqueous solutions of bases taste bitter (chalky). 2. Bases change the color og acid-base indicators (blue). 3. Dilute aqueous solutions of bases feel slippery. 4. Bases react with acids to produce salts and water. 5. Bases conduct electric current.

Question 7

How did Svente Arrhenius define acids?

Answer 7

An Arrhenius acid is a chemical compound that increases the concentration of hydrogen ions, H+, in aqueous solution.

Question 8

How did Svente Arrhenius define bases?

Answer 8

An Arrhenius base is a substance that increases the concentratoin of hydroxide ions, OH-, in aqueous solution.

Question 9

Define Strong Acid

Answer 9

Strong Acid- one that ionizes completely in aqueous solution. (highly ionize in solution)

Question 10

Define Weak Acid

Answer 10

Weak Acid- an acid that releases few hydrogen ions in aqueous solution. (do not ionize easily)

Question 11

How do strong and weak bases differ?

Answer 11

Strong bases are strong electrolytes, just as strong acids are strong electrolytes. Weak bases are weak electrolytes.

Question 12

What id the Bronsted-Lowry definition of an acid?

Answer 12

Bronsted-Lowry Acid - a molecule or ion that is a photon donor

Question 13

What is the Bronsted-Lowry definition of a base?

Answer 13

Bronsted-Lowry Base - a molecule or ion that is a photon acceptor.

Question 14

What occurs in a Bronsted-Lowry acid-base reaction?

Answer 14

Bronsted-Lowry acid-base reaction - photons are transferred from one reactant (the acid) to another (the base).

Question 15

Define Monoprotic Acid

Answer 15

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

Question 16

Define Polyprotic Acid

Answer 16

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

Question 17

What is the definition of a Lewis Acid?

Answer 17

Lewis Acid- an atom, ion, or molecule that accepts an electron pair to form a covalent bond

Question 18

What is the definition of a Lewis Base?

Answer 18

Lewis Base- an atom, ion or molecule that donates an electron pair to form a covalent bond.

Question 19

What occurs in a Lewis acid-base reaction?

Answer 19

Lewis acid-base reaction - the formation of one or more covalent bonds between an electron-pair donor and an electron-pair acceptor.

Question 20

What are the three types of Acid-Base Theories and what do their acid and base stand for?

Answer 20

Arrhenius: (acid) H+ or H3O+ producer. (base) OH- producer. Bronsted-Lowry: (acid) proton (H+) donor. (base) proton (H+) acceptor. Lewis: (acid) electron pair acceptor. (base) electron-pair donor.

Question 21

Define conjugate acid

Answer 21

conjugate acid- the species that is formed when Bronsted-Lowry gains a proton

Question 22

Define conjugate base

Answer 22

conjugate base- the species that remains after a Bronsted-Lowry acid has given up a proton.

Question 23

The stroner the acid is, the _____ is the conjugate base.

Answer 23

weaker

Question 24

The stronger the base is, the _____ is the conjugate acid.

Answer 24

weaker

Question 25

Proton transfer reactions favor the production of the ____ acid and the ____ base.

Answer 25

weaker; weaker

Question 26

What is an Amphoteric Compound?

Answer 26

Amphoteric Compound- any species that can react as either an acid or a base (water)

Question 27

Define Neutralization

Answer 27

Neautralization- the reaction of hydronium ions and hydroxide ions to form water molecules (when acids react with bases to form salts and water).

Question 28

What is a salt?

Answer 28

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

Question 29

What is acid rain and how is it formed?

Answer 29

Rainwater is normally slightly acidic but sometimes rain is very acidic and called acid rain. Acid rain results from chemical pollutants reacting with the water in the atmosphere.