Chapter 10: Acids and Bases and Equilibrium

Arrhenius Acids

Substances that produce hydrogen ions when they dissolve in water.

Svante Arrhenius

A Swedish chemist to first describe acids and bases.

*–ic acid*

The most common form of an oxygen-containing acid has a name that ends with *____*.

*–ate*

The name of oxygen-containing acid polyatomic anion ends in *____*.

*–ous acid*

An acid that contains one less oxygen atom than the common form is named as an *____*.

*–ite*

The name of less oxygen atom polyatomic anion ends with *___*.

Arrhenius Bases

These are ionic compounds that dissociate into metal ions and hydroxide ions when they dissolve in water.

Group 1A and Group 2A

Most Arrhhenius bases are formed from ____ metals.

hydroxides

Typical Arrhenius bases are named as ____

J. N. Brønsted and T. M. Lowry

They expanded the definition of acids and bases in 1923.

Brønsted–Lowry acid

It can donate a hydrogen ion to another substance.

Brønsted–Lowry base

It can accept hydrogen ion.

Conjugate Acid–Base Pair

It consists of molecules or ions related by the loss of one H+ by an acid, and the gain of one H+ by a base.

Amphoteric

Substances that can act as acids and bases.

acid

The strength of an ____ is determined by the moles of H3O+ that are produced for each mole of acid that dissolves.

base

The strength of a ____ is determined by the moles of OH- that are produced for each mole of base that dissolves.

Strong acids

These are examples of strong electrolytes because they donate H+ so easily that their ionization in water is virtually complete.

Weak Acids

These are weak electrolytes because they ionize slightly in water, which produces only a few ions.

Diprotic Acid

Carbonic acid that has two H+, which ionize one at a time

Strong Bases

These are ionic compounds that dissociate in water to give an aqueous solution of metal ions and hydroxide ions.

Weak Bases

These are weak electrolytes that are poor acceptors of hydrogen ions and produce very few ions in solution.

Equilibrium

* The rates of the forward and reverse reactions become equal.
* The reactants form products at the same rate that the products form reactants.
* It has been reached when no further change takes place in the concentrations of the reactants and products.

Le Châtelier’s principle

It states that when equilibrium is disturbed, the rates of the forward and reverse reactions change to relieve that stress and reestablish equilibrium.

acidic solution

In this solution, the \[H3O+\] is greater than the \[OH-\].

basic solution

In this solution, the \[OH-\] is greater than the \[H3O+\].

pH Scale

A range of numbers typically from 0 to 14, which represents the \[H3O+\] of the solution.

7\.0

A neutral solution has a pH of ___.

acidic

In ____ solutions, the pH is below 7.0.

basic

In ____ solutions, the pH is above 7.0.

Salt

An ionic compound that does not have H+ as the cation or OH- as the anion.

Neutralization

A reaction between an acid and a base to produce water and salt.

Titration

A laboratory procedure n which we neutralize an acid sample with a known amount of base.

Antacids

These are substances used to neutralize excess stomach acid.

Buffer Solution

It maintains pH by neutralizing small amounts of added acid or base.

Acidosis

A condition that occurs when there’s an increase in the CO2 level that leads to a low blood pH concentration.

Alkalosis

A condition that occurs when there’s a decrease in the CO2 level that leads to a high blood pH concentration.

Ionization of Water Formula