Acids & Bases
Svante Arrhenius
A Swedish chemist, who proposed a commonality of all acids to explain their similar properties.
Hydrogen Ion
A hydrogen atom without its electron (consisting solely of a proton).
pH Scale
A logarithm scale that measures the acidity or alkalinity of a solution on a scale of 1 to 14.
Acidity
A measure of the hydrogen (hydronium) ion concentration of a solution.
Alkalinity
A measure of the hydroxide ion concentration of a solution.
Conjugate Acid-Base Pair
A pair of chemical formulas that differ only by the presence of a hydrogen ion.
Arrhenius Acid
A substance that produces hydronium ions (H3O+) as the only positive ions when dissolved in water.
Arrhenius Base
A substance that produces hydroxide ions (OH-) as the only negative ions when dissolved in water.
Indicator
A substance that undergoes a color change that can be used to determine when a reaction is complete.
Electrolyte
A substance whose water solution conducts an electric current.
Atom
A tiny particle theorized as the basic unit of matter.
Binary Acid
Acids composed of hydrogen and one other element. The names of binary acids begin with "hydro-" followed by the name of the other element modified to end with "-ic".
Strong Acid/Base
An acid or base that ionizes completely. Highly ionize acids and bases produce large numbers of ions. These strong acids and bases are strong electrolytes and are good conductors of electricity.
Weak Acid/Base
An acid or base that only ionizes slightly.
Ternary Acid
Another molecular substance that produces hydrogen ions when dissolved in water. They consist of a polyatomic ion containing oxygen such as nitrate (NO3-) or sulfate (SO4^2-).
Brønsted-Lowry Base
Any substance that accepts a proton (H+). Compared with the Arrhenius definition, however, the Brønsted-Lowry definition greatly expands the number of substances that are considered bases.
Brønsted-Lowry Acid
Any substance that donates a hydrogen ion (H+). All Brønsted-Lowry acids are also Arrhenius acids. Brønsted-Lowry theory expands on the Arrhenius concept.
Monoprotic Acid
The H+ molarity equals the molarity of the acid solution. Hydrochloric acid is an example. 2.5 M HCl = 2.5 M H+
Triprotic Acid
The H+ molarity is three times the molarity of the acid solution. Phosphoric acid is an example. 2.0 M H3PO4 = 6.0 M H+
Diprotic Acid
The H+ molarity is twice the molarity of the acid solution. Sulfuric acid is an example. 2.5 M H2SO4 = 5.0 M H+
Monohydroxy Base
The OH- molarity equals the molarity of the base solution. Sodium hydroxide is an example. 3.0 M NaOH = 3.0 M OH-
Dihydroxy Base
The OH- molarity is twice the molarity of the base solution. Barium hydroxide is an example. 0.5 M Ba(OH)2 = 1.0 M OH-
Naming a Base
The name of the positive ion is not modified, and the name of the base ends with hydroxide. For example, Ca(OH)2 is calcium hydroxide.
pH
The negative logarithm of a solution hydrogen ion concentration.
Hydronium Ion
The polyatomic anion produced by the ionization of a water molecule.
Titration
The process of determining the concentration of an unknown solution by a reaction with a solution of known concentration.
Salt
The product (other than water) of a neutralization reaction; an ionic substance consisting of a metallic cation and anion other than the hydroxide ion. Salts are named by using the named by using the name of the positive ion of the base and the negative ion of the acid.
Neutralization
The reaction between an acid and a base to produce water and a salt. In all neutralization reactions there must be a 1:1 ratio between the moles of hydrogen ions (H+) and the moles of hydroxide ions (OH-). Equation: MA x VA = MB x VB
Atomic Mass
The sum of the protons and neutrons in an atom of an element
Equation for Neutralization Reaction
acid + base --> water + salt
Characteristics of Properties of Bases
•Bases have a bitter taste. •Bases have a slippery or so be feeling. •Bases conduct an electric current. •Bases react with acids to produce water and a salt. •Bases cause acid-base indicators to change color.
Characteristic Properties of Acids
•Dilute solutions of acids have a sour taste. •Aqueous solutions of acids conduct an electric current. •Acids react with bases to form water and salt. •Acids react with certain metals to produce hydrogen gas. •Acids cause acid-base indicators to change color.
