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Acids
Classes of compounds recognized by easily observed properties like conducting electricity in aqueous solutions, turning blue litmus red, and having a pH less than 7.
Bases
Classes of compounds recognized by properties such as conducting electricity in aqueous solutions, turning red litmus blue, and having a pH greater than 7.
Arrhenius Acid
Defined as a substance that has hydrogen (H) and releases H+ ions in solution, like HCl and HBr.
Arrhenius Base
Defined as a substance that has hydroxide (OH) and releases OH- ions in solution, like NaOH and KOH.
Neutralization Reaction
A reaction between an acid and a base to produce water and a salt, following the equation Acid + Base → Water + Salt.
Bronsted-Lowry Theory
Defines acids as proton donors and bases as proton acceptors, expanding upon the Arrhenius concept.
Conjugate Acid-Base Pairs
Two substances related by donating and accepting a single proton, where a conjugate base is what remains after an acid donates a proton.
pH Scale
A logarithmic scale indicating acidity, with pH less than 7 being acidic, pH more than 7 being basic, and pH of 7 being neutral.
Titration
Process of adding measured volumes of known molarity acid/base to an unknown molarity solution until neutralization, used to calculate the concentration of the unknown solution.
Acidity
The level of acid present in a solution, typically measured by the concentration of hydrogen ions.
Electrolyte
A substance that conducts electricity when dissolved in water, typically dissociating into ions.
Alkalinity
The level of alkaline (basic) substances present in a solution, often measured by the concentration of hydroxide ions.
Arrhenius
A Swedish scientist known for his theory of electrolytic dissociation, which explains the behavior of acids and bases in aqueous solutions.
Acid
A substance that donates protons (hydrogen ions) or accepts electron pairs in chemical reactions.
Hydrogen ion
A positively charged ion (H+) formed when an acid dissolves in water.
Hydronium ion
The hydrated form of the hydrogen ion (H3O+), present when acids dissolve in water.
Arrhenius base
A substance that dissociates in water to produce hydroxide ions (OH-) in solution.
Indicator
A substance that changes color in response to changes in pH, used to determine the endpoint of a titration.
Neutralization
The chemical reaction between an acid and a base to form water and a salt.
pH scale
A scale used to specify the acidity or alkalinity of a solution, ranging from 0 to 14, with 7 considered neutral, values below 7 acidic, and values above 7 basic.
Salt
A compound formed from the reaction between an acid and a base, consisting of positive and negative ions other than hydrogen and hydroxide ions.
Titration
A laboratory technique used to determine the concentration of a substance in solution by reacting it with a known volume and concentration of another substance.
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