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Lecture

Proton Exchange: Part 1

Description

This lecture covers proton exchanges in acid-base reactions and titrations, including the product of water autoionization, pH, pOH, strength of acids and bases, and pH calculations for different solutions. It also discusses the concept of acid-base couples, the definition of pH and pOH, and the color changes in different compounds based on pH levels.

Official source

Ontological neighbourhood

Chemistry

Inorganic chemistry: Topics in inorganic chemistry

Related concepts (30)

Acid

An acid is a molecule or ion capable of either donating a proton (i.e. hydrogen ion, H+), known as a Brønsted–Lowry acid, or forming a covalent bond with an electron pair, known as a Lewis acid. The first category of acids are the proton donors, or Brønsted–Lowry acids. In the special case of aqueous solutions, proton donors form the hydronium ion H3O+ and are known as Arrhenius acids. Brønsted and Lowry generalized the Arrhenius theory to include non-aqueous solvents.

Acid–base reaction

An acid–base reaction is a chemical reaction that occurs between an acid and a base. It can be used to determine pH via titration. Several theoretical frameworks provide alternative conceptions of the reaction mechanisms and their application in solving related problems; these are called the acid–base theories, for example, Brønsted–Lowry acid–base theory. Their importance becomes apparent in analyzing acid–base reactions for gaseous or liquid species, or when acid or base character may be somewhat less apparent.

Acid dissociation constant

In chemistry, an acid dissociation constant (also known as acidity constant, or acid-ionization constant; denoted K_a) is a quantitative measure of the strength of an acid in solution. It is the equilibrium constant for a chemical reaction HA A^- + H^+ known as dissociation in the context of acid–base reactions. The chemical species HA is an acid that dissociates into , the conjugate base of the acid and a hydrogen ion, .

Acid strength

Acid strength is the tendency of an acid, symbolised by the chemical formula HA, to dissociate into a proton, H+, and an anion, A-. The dissociation of a strong acid in solution is effectively complete, except in its most concentrated solutions. HA -> H+ + A- Examples of strong acids are hydrochloric acid (HCl), perchloric acid (HClO4), nitric acid (HNO3) and sulfuric acid (H2SO4). A weak acid is only partially dissociated, with both the undissociated acid and its dissociation products being present, in solution, in equilibrium with each other.

In chemistry, pH (piːˈeɪtʃ ), also referred to as acidity, historically denotes "potential of hydrogen" (or "power of hydrogen"). It is a scale used to specify the acidity or basicity of an aqueous solution. Acidic solutions (solutions with higher concentrations of hydrogen () ions) are measured to have lower pH values than basic or alkaline solutions. The pH scale is logarithmic and inversely indicates the activity of hydrogen ions in the solution. where [H+] is the equilibrium molar concentration (mol/L) of H+ in the solution.

Related lectures (33)

Acids and Bases: Definitions and Equilibrium

Explains acid-base definitions, equilibrium constants, pH scale, conjugate pairs, and buffers.

Acid-Base Equilibria

Explores acid-base equilibria, including pH calculations for weak acids and bases, diacids, strong/weak bases, and salt solutions.

Chemical Equilibria and Reactivity

Explores chemical equilibria, weak acids, buffers, titration curves, and indicators in acid-base reactions.

Acids and Bases: Equilibria and Reactions

Delves into the principles of acids and bases, their equilibria, and effects on solution pH.

Acids and Bases: Dissociation and pH

Covers the dissociation of molecules to determine if they are acids or bases and how to calculate pH levels.

Related concepts (30)

Acid

Acid–base reaction

Acid dissociation constant

Acid strength