Glossary
Acid - An acid donates [H+] protons and accepts electron pairs. Also, have a pH lower than 7.
Alkali - An alkali is a base that dissolves in water
Arrhenius Theory - The Arrhenius Theory states that acids produce H+ ions, while bases, when dissolved, produce OH- ions
Base - a substance that is a proton receiver, are electron pair donors and when dissolved in water they produce hydroxide ions (OH-).
Buffer - A buffer is a solution that can not change or resist the pH changing by the addition of acidic of basic solutions.
Bronsted Lowry Theory - acids are proton donors, bases are proton acceptors
Concentration - the amount of the acid per unit volume (liter)
Conjugate Acid - A conjugate acid is a substance formed when a base receives hydrogen ions.
Conjugate Base - A conjugate base is a substance created when an acid loses a proton
Indicator - An indicator is used to measure the pH of a solution
Lewis Theory - Acids are electron pair acceptors while bases are electron pair donors
[H+] - hydrogen protons
Neutralization - Neutralization is a reaction when you neutralize either a base or an acid.
Neutral - For a solution to be neutral, the pH has to be exactly 7
[OH-] - hydroxide ions
pH - The pH is the hydrogen ion concentration in the solution
pOH - The pOH is the hydroxide ion concentration in the solution
Strength of an acid - The strength of an acid is the dissociation of the hydrogen ions in the water
Strength of a base - The strength of a base if the dissociation of the hydroxide ions in the water
Titration - process of neutralization that can determine the molarity of an unknown concentration
Weak Acid - an acid that only partially dissociates or not at all to form hydrogen ions in water
Weak Base - a base that only partially dissociates or not at all to form hydroxide ions in water
Alkali - An alkali is a base that dissolves in water
Arrhenius Theory - The Arrhenius Theory states that acids produce H+ ions, while bases, when dissolved, produce OH- ions
Base - a substance that is a proton receiver, are electron pair donors and when dissolved in water they produce hydroxide ions (OH-).
Buffer - A buffer is a solution that can not change or resist the pH changing by the addition of acidic of basic solutions.
Bronsted Lowry Theory - acids are proton donors, bases are proton acceptors
Concentration - the amount of the acid per unit volume (liter)
Conjugate Acid - A conjugate acid is a substance formed when a base receives hydrogen ions.
Conjugate Base - A conjugate base is a substance created when an acid loses a proton
Indicator - An indicator is used to measure the pH of a solution
Lewis Theory - Acids are electron pair acceptors while bases are electron pair donors
[H+] - hydrogen protons
Neutralization - Neutralization is a reaction when you neutralize either a base or an acid.
Neutral - For a solution to be neutral, the pH has to be exactly 7
[OH-] - hydroxide ions
pH - The pH is the hydrogen ion concentration in the solution
pOH - The pOH is the hydroxide ion concentration in the solution
Strength of an acid - The strength of an acid is the dissociation of the hydrogen ions in the water
Strength of a base - The strength of a base if the dissociation of the hydroxide ions in the water
Titration - process of neutralization that can determine the molarity of an unknown concentration
Weak Acid - an acid that only partially dissociates or not at all to form hydrogen ions in water
Weak Base - a base that only partially dissociates or not at all to form hydroxide ions in water