Chapter 8

Physical Properties

A property of a substance that can be observed without a reaction.

Properties of Acids

Sour

pH less than 7

Generally clear solutions

A conductor of electricity

React with metals and metal carbonates

Turns litmus paper red

Properties of Bases

Bitter

pH greater than 7

Generally clear or foggy solutions

A conductor of electricity

Turns litmus paper blue

Chemical Properties

A property that can only be observed by a reaction

A base turns RED litmus paper

Blue

An Acid turns BLUE litmus paper

Red

Naming Binary Acids

Two Element solution

When name of anion (last element) ends in -ide

Begins with Hydro

Add -IC to the end

Add Acid

Example of Binary Acid

HC; (Hydrochloric acid)

Naming Tetra Acids

When name of anion (last element) ends in -ITE

Add -OUS to end

Add Acid

Ternary Acid

When the anion (last element) ends in -ATE

Add -IC

Does not Begin with Hydro

Add Acid

What are reactions with metals and acids classified as?

Single Replacement Equations

What is produced when a metal and acid react?

Hydrogen Gas

What are reactions with metal carbonates and acids classified as?

Double Replacement Equations

What is produced when a metal carbonate and acid reacts?

H20 and Co2 (Water and Carbon Dioxide)

All water solutions contain what?

Hydrogen Ions (H+) and Hydroxide ions (OH-)

What is an Acidic Solution?

A solution with a higher concentration of Hydrogen ions (H+)

What is a basic solution?

A solution with a higher concentration of Hydroxide ions (OH-)

Self-Ionization

When pure water produces even amounts of OH- and H+.

Strong Acids

Hydrochloric Acid (HCl)

Hydroionic Acid (HI)

Perchloric Acid (HCLO4)

Nitric Acid (HNO3)

Sulfuric Acid (H2SO4)

Strong Bases

Hydroxides from groups 1 or 2.

Ex. Sodium hydroxide (NaOH)

Potassium hydroxide (KOH)

Rubidium hydroxide (RbOH)

The more ions in a solution…

the easier an electrical current can be carried through the solution

Strong Acids ionize…

completely

Strong acids will produce how many ions in solutions?

The maximum amount

Weak Acids

An acid that ionizes only partly in dilute aqueous solutions

Strong Base

A base that dissociated completely into metal ions and hydroxide ions.

Salt

A compound made out of a metal ion and non-metal ion.

What is Arrhenius definitions for an acid and base?

Arrhenius states that Acids create H+ and Bases create OH-

Monoprotic Acids

Acids that produce one H+

Ex. HCl

Polyprotic Acids

Acids that produce more than one H+

\#x. H3PO4

Ion Product Constant for Water

Pure water contains equal concentration of H+ and OH- ions produced by the process called Self-ionization

Ex. H20→H+ + Oh-

Kw

Known as the ion product constant for water. It relates the concentration of the H+ and OH- ions in any aqueous solution\\

Kw=1.0x10^-14=H+ x OH-

what do \[\] mean? (The boxes around the H+ and OH-)

molarity

Hydrogen ion

When the H+ is greater than 1.0x10^-14, the solution is acidic

Hydroxide Ion

When the OH- is greater than 1.0x10^-14, the solution is basic

Bronsted-Lowry Model

A model of acids and bases in which an acid is a hydrogen-ion doner and a base is a hydrogen-ion receiver.

Conjugate Acid

The species produced when a base accepts a hydrogen ion from an acid.

Conjugate Base

The species produced when an acid donates a hydrogen ion to a base

conjugate acid-base pair

Consists of two substances related to each other by the donating and accepting of a single hydrogen ion.

Amphoteric

Describes water and other substances that can act as both an acid and base.

neutralization reaction

A reaction in which an acid and base react in aqueous solution to produce a salt and water.

Indicators

Indigo Carmine, Methyl Red, Methyl Orange, Litmus, Bromothymol blue, and Phenolphthalein.

Titrant

A solution of known concentration used to titrate a solution of unknown concentration, also called the standard solution.

Titration

The process in which an acid-base neutralization reaction is used to determine the concentration of a solution of unknown concentration.

Equivalence Point

The point in which the moles of H+ ions from the acid equals moles of OH- ions from the base.

End Point

The point in which the indicator used in titration changes color.

salt hydrolysis

The process in which anions of the dissociated salt accept hydrogen ions from water, or the cations from the dissociated salt donate hydrogen ions to water

Buffers

A solution that resists changes in pH when limited amounts of acid or base are involved

Buffer capacity

The amount of acid or base a buffer solution can absorb without a significant change in pH.