Chemistry

Conjugate Base

A conjugate acid, within the Brønsted-Lowry acid-base theory, is a species formed by the reception of a proton (H+), by a base—in other words, the base with a hydrogen ion added to it. On the other hand, a conjugate base is merely what is left after an acid has donated a proton in a chemical reaction

Conjugate Acid

A conjugate acid, within the Brønsted-Lowry acid-base theory, is a species formed by the reception of a proton (H+), by a base—in other words, the base with a hydrogen ion added to it. On the other hand, a conjugate base is merely what is left after an acid has donated a proton in a chemical reaction.

Neutral Solution

A neutral solution is a solution that has a pH of 7. It is neither acidic (pH<7) or basic (pH>7), but right in the middle, or 'neutral.'

neutralization reaction

A neutralization reaction is when an acid and a base react to form water and a salt and involves the combination of H+ ions and OH- ions to generate water. The neutralization of a strong acid and strong base has a pH equal to 7.

Ph Scale

A pH scale is a measure of how acidic or basic a substance is. While the pH scale formally measures the activity of hydrogen ions in a substance or solution, it is typically approximated as the concentration of hydrogen ions

Strong Acid

A strong acid is one that completely ionizes (dissociates) in a solution.

strong base

A strong base is something like sodium hydroxide or potassium hydroxide which is fully ionic. You can think of the compound as being 100% split up into metal ions and hydroxide ions in solution. Each mole of sodium hydroxide dissolves to give a mole of hydroxide ions in solution.

weak acid

A weak acid is an acid that dissociates incompletely, releasing only some of its hydrogen atoms into the solution. Thus, it is less capable than a strong acid of donating protons. These acids have higher pKa than strong acids, which release all of their hydrogen atoms when dissolved in water.

Amphoteric

Able to react both as a base and as an acid. (of a compound, especially a metal oxide or hydroxide)

Acidic Solution

Any solution that has a higher concentration of hydrogen ions than water; solutions that have a lower concentration of hydrogen ions than water are called basic or alkaline solutions.

hydroxide ion

Hydroxide is a diatomic anion with chemical formula OH−. It consists of an oxygen and a hydrogen atom held together by a covalent bond, and carries a negative electric charge. It is an important but usually minor constituent of water

weak base

In chemistry, a weak base is a chemical base that does not ionize fully in an aqueous solution. As Brønsted-Lowry bases are proton acceptors, a weak base may also be defined as a chemical base in which protonation is incomplete.

Basic Solution

One is the Arrhenius definition, which revolves around the idea that acids are substances that ionize (break off) in an aqueous solution to produce hydrogen (H+) ions while bases produce hydroxide (OH-) ions in solution.

Ion-produced constant- Kw

The equilibrium constant for the reaction in which water undergoes an acid-base reaction with itself. That is, water is behaving simultaneously as both an acid and a base.

Hydronium ion

The ion H3O+, consisting of a protonated water molecule and present in all aqueous acids.