An acid-base reaction is a chemical reaction between an acid and a base. ...more on Wikipedia about "Acid-base reaction theories"
Alkalinity or AT is a measure of the acid neutralizing capacity (ANC) of a solution. ...more on Wikipedia about "Alkalinity"
In chemistry, a substance is described as amphiprotic, if it can both donate or accept a proton, thus acting either like an acid or a base. Water, amino acids, hydrogen carbonate ions and hydrogen sulfate ions are common examples of amphiprotic species. Since they can donate a proton, all amphiprotic substances contain a hydrogen atom. Also, since they can act like an acid or a base, they are amphoteric. Amphoteric substances, however, are not necessarily amphiprotic. ...more on Wikipedia about "Amphiprotic"
A Brønsted-Lowry acid (sometimes shortened to Brønsted acid) is an acid that donates a hydrogen ion to another compound, called a Brønsted-Lowry base. ...more on Wikipedia about "Brønsted acid"
In chemistry, the Brønsted-Lowry system defines acids and bases. This acid-base theory was independently proposed by Johannes Nicolaus Brønsted and Thomas Lowry in 1923. In this system, a Brønsted-Lowry acid is defined as any substance which donates a proton (a Hydrogen Ion, H+) in a reaction; and a base as a substance which receives a proton in a reaction. ...more on Wikipedia about "Brønsted-Lowry"
Buffer solutions are solutions which resist change in pH upon addition of small amounts of acid or base. As a consequence of this definition, the theory of buffer solutions presented in this article uses the Arrhenius and Brønsted-Lowry notion of acids and bases, as opposed to the Lewis acid-base theory. See Acid-base reaction theories for further details on this subtle point. The scope of this article also does not consider buffer solutions prepared with solvents other than water. ...more on Wikipedia about "Buffer solution"
A buffering agent adjusts the pH of a solution. The function of a buffering agent is to drive an acidic or alkaline solution to a certain pH state and prevent a change in this pH. Buffering agents have variable properties -- some are more soluble than others; some are acidic while others are basic. As pH managers, they are important in many chemical applications, including agriculture, food processing, medicine and photography. ...more on Wikipedia about "Buffering agent"
My shortopedia is mine.
Carbonate Alkalinity is a measure of the amount of carbonate and bicarbonate anions in solution. Carbonate and bicarbonate anions contibute to alkalinty due to their basic nature, hence their ability of neutralize acid. Mathmatically, the carbonate anion concentration is counted twice due to its abiliity to neutralize two protons, while bicarbonate is counted once as it can neutralize one proton. Carbonate alkalinity is often the major component of a natural solution's total alkalinity. It is an important factor in understanding large scale environmental interactions based on simple pH and carbon dioxide measurements. ...more on Wikipedia about "Carbonate alkalinity"
A chemical indicator is any substance used to assist in the classification of another substance. Indicators or [In] are weak acids or bases that undergo dissociation in a known pH range. It is in this range that the acid (or base) is a different colour from its conjugate base (or acid). ...more on Wikipedia about "Chemical indicator"
Deprotonation is a chemistry term that refers to the removal of a proton ( hydrogen ion H+) from a molecule, forming the conjugate base. The relative ability for a molecule to give up a proton is measured by a pK value. A low pK value indicates that the compound is acidic and will easilly give up its proton to a base. The pK of a compound is determined by many things, but most significantly impacted by the conjugate base's ability (or inability) to stabilize the negative charge through resonance. ...more on Wikipedia about "Deprotonation"
The Henderson-Hasselbalch (frequently misspelled Henderson-Hasselbach) equation in chemistry describes the derivation of pH as a measure of acidity (using pKa, the acid dissociation constant) in biological and chemical systems. The equation is also useful for estimating the pH of a buffer solution and finding the equilibrium pH in acid-base reactions. ...more on Wikipedia about "Henderson-Hasselbalch equation"
The HSAB concept, also known as HSAB theory, is widely used in chemistry for explaining stability of compounds, reaction paths etc. ...more on Wikipedia about "HSAB concept"
In chemistry, a Lewis acid can accept a pair of electrons and form a coordinate covalent bond, after the American chemist Gilbert Lewis. The Lewis acid and Lewis base theory is one of several acid-base reaction theories, therefore the term acid is ambiguous; it should always be clarified as being a Lewis acid (only) or a Brønsted-Lowry acid. ...more on Wikipedia about "Lewis acid"
A Lewis base is any molecule or ion that can form a new coordinate covalent bond, by donating a pair of electrons. The term base is ambiguous. This is one interpretation. ...more on Wikipedia about "Lewis base"
Neutralization is a chemical reaction, also called a water forming reaction, in which an acid and a base or alkali (soluble base) react and produce a salt and water. ...more on Wikipedia about "Neutralization"
pH (abbr. power of hydrogen ** ) is a measure of the activity of hydrogen ions (H+) in a solution and, therefore, its acidity or alkalinity. In aqueous systems, the hydrogen ion activity is dictated by the dissociation constant of water (Kw = 1.011 × 10−14 at 25 °C) and interactions with other ions in solution. Due to this dissociation constant a neutral solution (hydrogen ion activity equals hydroxide ion activity) has a pH of approximately 7. Aqueous solutions with pH values lower than 7 are considered acidic, while pH values higher than 7 are considered alkaline. ...more on Wikipedia about "PH"
A pH meter is a specific type of voltmeter with a very high impedance of the input channels. The high impedance is a necessary part of the equipment because of high resistance of the pH glass electrode typically used with pH meters (usually between 20 and 100 MΩ). ...more on Wikipedia about "PH meter"
This article is licensed under the GNU Free Documentation License.
It uses material from the Wikipedia . Direct links to the original articles are in the text.
If you use exact copy or modified of this article you should preserve above paragraph and put also : It uses material from the Shortopedia article about "Acid-bases".
|MAIN PAGE||MAIN INDEX||CONTACT US|