Lecture

Q&A Session on Acids and Bases

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In course

CH-160(b): General chemistry

Cet enseignement vise l'acquisition des notions essentielles relatives à la structure de la matière, aux équilibres et à la réactivité chimiques. Le cours et les exercices fournissent la méthodologie permettant de résoudre par le raisonnement et le calcul ...

Description

This lecture covers a Q&A session on acids and bases, focusing on calculating minimal mass, buffer solutions, and practical problems related to buffer solutions. The instructor provides detailed explanations and examples, emphasizing the importance of understanding the concepts and solving challenging exercises. The session also addresses questions from students, clarifying concepts such as pH calculations, equilibrium reactions, and the behavior of strong bases. The instructor encourages active participation and offers support for students to enhance their understanding of acid-base chemistry.

Instructor

Samuel Terrettaz

Teaching & PhD Courses Advanced general chemistry CH-160(f) This course aims at the acquisition of essential notions on the structure of matter, chemical equilibria and reactivity. Theoretical teaching and exercise provide the methodology to analyze and solve by reasoning and calculation novel problems of general chemistry. Advanced general chemistry CH-160(g) This course aims at the acquisition of essential notions on the structure of matter, chemical equilibria and reactivi

Official source

Ontological neighbourhood

Chemistry

Inorganic chemistry: Topics in inorganic chemistry

Related concepts (24)

Lewis acids and bases

A Lewis acid (named for the American physical chemist Gilbert N. Lewis) is a chemical species that contains an empty orbital which is capable of accepting an electron pair from a Lewis base to form a Lewis adduct. A Lewis base, then, is any species that has a filled orbital containing an electron pair which is not involved in bonding but may form a dative bond with a Lewis acid to form a Lewis adduct. For example, NH3 is a Lewis base, because it can donate its lone pair of electrons.

Base (chemistry)

In chemistry, there are three definitions in common use of the word "base": Arrhenius bases, Brønsted bases, and Lewis bases. All definitions agree that bases are substances that react with acids, as originally proposed by G.-F. Rouelle in the mid-18th century. In 1884, Svante Arrhenius proposed that a base is a substance which dissociates in aqueous solution to form hydroxide ions OH−. These ions can react with hydrogen ions (H+ according to Arrhenius) from the dissociation of acids to form water in an acid–base reaction.

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.

Equilibrium constant

The equilibrium constant of a chemical reaction is the value of its reaction quotient at chemical equilibrium, a state approached by a dynamic chemical system after sufficient time has elapsed at which its composition has no measurable tendency towards further change. For a given set of reaction conditions, the equilibrium constant is independent of the initial analytical concentrations of the reactant and product species in the mixture.

Chemical equilibrium

In a chemical reaction, chemical equilibrium is the state in which both the reactants and products are present in concentrations which have no further tendency to change with time, so that there is no observable change in the properties of the system. This state results when the forward reaction proceeds at the same rate as the reverse reaction. The reaction rates of the forward and backward reactions are generally not zero, but they are equal. Thus, there are no net changes in the concentrations of the reactants and products.

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Covers acid-base equilibrium principles, pH scale, strong/weak acids, bases behavior, and pH calculation.

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

Acids and Bases: Fundamentals and Equilibria

Covers the fundamentals of acids and bases, including acid-base reactions, equilibrium constants, and amphoteric substances.

Acids and Bases: Equilibrium and Redox Reactions

Explores acids, bases, pH calculations, buffer solutions, and redox reactions.

Chemical Equilibria and Reactivity