"An acid is a molecule or ion capable of either donating a proton (i.e. hydrogen ion, H+), known as a Brønsted–Lowry acid."
This topic covers the physical and chemical properties of acids.
pH scale: The pH scale measures the concentration of hydrogen ions in a solution and ranges from 0 to 14.
Acid-base reactions: Acid-base reactions are chemical reactions that involve the transfer of protons from an acid to a base.
Bronsted-Lowry theory: The Bronsted-Lowry theory defines an acid as a proton donor and a base as a proton acceptor.
Lewis theory: The Lewis theory defines an acid as an electron-pair acceptor and a base as an electron-pair donor.
Strong acids and bases: Strong acids and bases completely dissociate in water and have a high concentration of hydrogen ions or hydroxide ions, respectively.
Weak acids and bases: Weak acids and bases only partially dissociate in water and have a low concentration of hydrogen ions or hydroxide ions, respectively.
Conjugate acid-base pairs: Conjugate acid-base pairs are two molecules or ions that differ by one proton.
Acid-base titration: Acid-base titration is a technique used to determine the concentration of an acid or base by adding a solution with a known concentration of the opposite type.
Buffer solutions: Buffer solutions resist changes in pH when small amounts of acid or base are added.
Acid rain: Acid rain is the deposition of acidic substances in the form of rain, snow, or fog, which results from the reaction of sulfur dioxide and nitrogen oxides with water in the atmosphere.
Sour taste: Acids have a sour taste due to the presence of hydrogen ions (H+) which stimulates the taste buds.
Corrosive: Acids are corrosive in nature and can eat away at metals and other materials. They also cause burns on human skin, clothing, and other objects.
Conductivity: Acids in aqueous solution are good conductors of electricity due to the presence of ions, particularly hydrogen ions.
pH less than 7: The pH scale ranges from 0-14, with 7 being neutral. Acids have a pH less than 7, indicating the presence of excess hydrogen ions in a solution.
Neutralizing bases: When acids react with bases, they undergo neutralization reactions and produce salt and water.
Weak or strong: Acids can be weak, meaning they only ionize slightly, or strong, meaning they ionize completely in water.
Reactivity: Acids are chemically reactive and can react with metals to produce hydrogen gas, with carbonates to produce carbon dioxide gas, and with many other compounds.
Acid-base indicators: Acids can be detected by acid-base indicators, which change color in response to changes in pH.
Bitter taste: Bases have a bitter taste due to the presence of hydroxide ions (OH-) which stimulate taste buds.
Slippery feel: Bases have a slippery or soapy feel due to their ability to react with fatty acids and produce soap.
Corrosive: Bases are also corrosive in nature and can eat away at metals and other materials like acids.
Conductivity: Like acids, bases in aqueous solution are good conductors of electricity due to the presence of ions, specifically hydroxide ions.
pH greater than 7: Bases have a pH greater than 7, indicating an excess of hydroxide ions in a solution.
Neutralizing acids: When bases react with acids, they undergo neutralization reactions and produce salt and water.
Weak or strong: Bases can be weak or strong, meaning they only ionize slightly (weak) or ionize completely in water (strong).
Reactivity: Bases are also chemically reactive and can react with acids to produce salt and water, and with many other compounds.
Acid-base indicators: Bases can also be detected by acid-base indicators, which change color in response to changes in pH.
"Proton donors form the hydronium ion H3O+ and are known as Arrhenius acids."
"Acids form aqueous solutions with a sour taste, can turn blue litmus red."
"Common aqueous acids include hydrochloric acid, acetic acid, sulfuric acid, and citric acid."
"A lower pH means a higher acidity, and thus a higher concentration of positive hydrogen ions in the solution."
"Strong acids and some concentrated weak acids are corrosive."
"Lewis acids form a covalent bond with an electron pair."
"An example is boron trifluoride (BF3), whose boron atom has a vacant orbital that can form a covalent bond by sharing a lone pair of electrons on an atom in a base."
"Hydrogen chloride, acetic acid, and most other Brønsted–Lowry acids cannot form a covalent bond with an electron pair."
"Conversely, many Lewis acids are not Arrhenius or Brønsted–Lowry acids."
"The word acid is derived from the Latin acidus, meaning 'sour'."
"Acids (in the colloquial sense) can be solutions or pure substances, and can be derived from acids (in the strict sense) that are solids, liquids, or gases."
"A Brønsted or Arrhenius acid usually contains a hydrogen atom bonded to a chemical structure that is still energetically favorable after loss of H+."
"Hydrochloric acid (a solution of hydrogen chloride that is found in gastric acid in the stomach) activates digestive enzymes."
"Acetic acid (vinegar) is a dilute aqueous solution of this liquid."
"Acids form aqueous solutions with a sour taste, can turn blue litmus red, and react with bases and certain metals to form salts."
"A lower pH means a higher acidity, and thus a higher concentration of positive hydrogen ions in the solution."
"Strong acids and some concentrated weak acids are corrosive, but there are exceptions such as carboranes and boric acid."
"In modern terminology, an acid is implicitly a Brønsted acid and not a Lewis acid."
"An acid is a chemical species that accepts electron pairs either directly or by releasing protons (H+) into the solution, which then accept electron pairs."