Lecture

Laboratory Experiment: Safety and Titration of a Diprotic Acid

Graph Chat

Chat with Graph Search

Ask any question about EPFL courses, lectures, exercises, research, news, etc. or try the example questions below.

DISCLAIMER: The Graph Chatbot is not programmed to provide explicit or categorical answers to your questions. Rather, it transforms your questions into API requests that are distributed across the various IT services officially administered by EPFL. Its purpose is solely to collect and recommend relevant references to content that you can explore to help you answer your questions.

In course

ENV-300: Pollutants analysis in the environment

Évaluation de la qualité d'une rivière en utilisant des méthodes d'observation ainsi que des méthodes physico-chimiques et biologiques. Collecte d'échantillons sur le terrain et analyses de laboratoire. Détermination pratique et utilisation des constantes ...

Description

This lecture covers laboratory safety procedures, including wearing protective gear and proper waste disposal. It also explains the titration process of a diprotic acid, from calibration to determining masses for solution preparation.

This video is available exclusively on Mediaspace for a restricted audience. Please log in to MediaSpace to access it if you have the necessary permissions.

Watch on Mediaspace

Instructors (2)

Florian Frédéric Vincent Breider

Florian Breider obtained his PhD in the field of the stable isotope biogeochemistry from the University of Neuchatel in 2013. This was followed by seven months of postdoc at EPFL in the Atmospheric Particles Research Laboratory and two years as research associate at Tokyo Institute of Technology (Japan) where he conducted studies on nitrous oxide biogeochemistry in oceans. From 2015 to 2018, he was research scientist in the Laboratory for Water Quality and Treatment at EPFL where he conducted research on disinfection by-products and antibiotic resistant bacteria. Since May 2018, he is director of the Central Environmental Laboratory at the Institute of Environmental Engineering of EPFL.

Christian Ludwig

2005 - today: Adjunct Professor at EPFL in the field of Solid Waste Treatment and head of the Chemical Processes and Materials research group (CPM) at Paul Scherrer Institute (PSI). Joint EPFL-PSI Professorship on Solid Waste Treatment. 2000 - today: Head, Group of Chemical Processes and Materials (CPM) at Paul Scherrer Institut (PSI). In 2009 the LEM unit was closed and the CPM group is now affiliated to the Bioenergy and Catalysis Laboratory (LBK) of the Energy and Environment Research Division (ENE). Since June 2002 permanent position ("tenure"). 1997 - 1999: Senior Scientist. Paul Scherrer Institut (PSI), General Energy Research Department, Element Cycles Section. 1995 - 1997: Research Fellow. Swiss Federal Institute for Environmental Science and Technology (EAWAG), Department of Resource and Waste Management. 1993 - 1995: Post-doc Fellow. University of California Davis, Department of Land, Air, and Water Resources (LAWR). 1990 - 1993: PhD Student. University of Berne, Department of Inorganic, Analytical, and Physical Chemistry. 1989 - 1990: Master Student. University of Berne, Department of Inorganic, Analytical, and Physical Chemistry.

Official source

Ontological neighbourhood

Chemistry

Inorganic chemistry: Topics in inorganic chemistry

Related concepts (13)

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–base homeostasis

Acid–base homeostasis is the homeostatic regulation of the pH of the body's extracellular fluid (ECF). The proper balance between the acids and bases (i.e. the pH) in the ECF is crucial for the normal physiology of the body—and for cellular metabolism. The pH of the intracellular fluid and the extracellular fluid need to be maintained at a constant level. The three dimensional structures of many extracellular proteins, such as the plasma proteins and membrane proteins of the body's cells, are very sensitive to the extracellular pH.

Buffer solution

A buffer solution (more precisely, pH buffer or hydrogen ion buffer) is an acid or a base aqueous solution consisting of a mixture of a weak acid and its conjugate base, or vice versa. Its pH changes very little when a small amount of strong acid or base is added to it. Buffer solutions are used as a means of keeping pH at a nearly constant value in a wide variety of chemical applications. In nature, there are many living systems that use buffering for pH regulation.

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, .

Brønsted–Lowry acid–base theory

The Brønsted–Lowry theory (also called proton theory of acids and bases) is an acid–base reaction theory which was first developed by Johannes Nicolaus Brønsted and Thomas Martin Lowry independently in 1923. The basic concept of this theory is that when an acid and a base react with each other, the acid forms its conjugate base, and the base forms its conjugate acid by exchange of a proton (the hydrogen cation, or H+). This theory generalises the Arrhenius theory.

Related lectures (46)

Chemical Equilibria and Reactivity

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

Acid-Base Equilibrium

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

Acids and Bases: Definitions and Equilibrium

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

Acid-Base Titrations

Explains acid-base titrations, including standard solutions, equivalence point, indicators, and distribution diagrams.

Acids and Bases: Equilibria and Reactions