Notes on Bronsted Lowry Acids/Bases
Notes on Bronsted Lowry Acids/Bases chem 10061-001
Popular in general chemistry 2
verified elite notetaker
Popular in Chemistry
This 2 page Class Notes was uploaded by Matthew Goetz on Wednesday April 13, 2016. The Class Notes belongs to chem 10061-001 at Kent State University taught by David bowers in Summer 2015. Since its upload, it has received 12 views. For similar materials see general chemistry 2 in Chemistry at Kent State University.
Reviews for Notes on Bronsted Lowry Acids/Bases
Report this Material
What is Karma?
Karma is the currency of StudySoup.
You can buy or earn more Karma at anytime and redeem it for class notes, study guides, flashcards, and more!
Date Created: 04/13/16
Gen Chem 2 Notes: Hydrohalic acids are strong. Oxoacids are strong if: O>(OH)+2. # of O’s are greater than or equal to # of OH’s +2. Oxoacids are weak if O=(OH) or O=(OH)+1 HF is a weak acid. Organic acids like –COOH are weak too. An acid is weak if O’s are not bound to O’s or halogens (H2S, or HCN). Bases are strong if they feature metals from group 1 or 2. Ammonia and water are weak bases. Amines are weak bases too. Kb is the equilibrium constant in relation to bases. pH= log(hydronium ions) pOH= log(hydroxide ions) pKa= logKa pKw= pH + pOH pKa is the measure of the strength of acid’s dissociation. We must know how to calculate pH from the molarity of the given solution or compound. Bronsted Lowry Acids: An acid that donates an H+. Bronsted Lowry Base: A base is an H+ acceptor. Must contain a lone pair of electrons for the H+ to bond at. Amines, ammonia, and fluorine are examples. These acid base reactions form conjugate acids and bases: An example of this process is above. In a conjugate acid an extra H+ is present than before, and in conjugate bases one less H+ is present. The net direction of acid basic reactions depend on the strength of acids and bases. If a Strong acid is a reactant and a weak acid is a product, then the products are favored. High Ka = strong acid. % dissociation = [HA dissolved]/[HA initial] Polyprotic acids: Acids with more than one ionizable proton. The dissociation of the first proton is easier than that of the second, which is similarly easier than that of the third proton. Examples of polyprotic acids are H2SO4, and H3PO4. All strong polyprotic acids become weak when they lose their first H+. Bronsted Lowry Base: A species that accepts H+’s. To accept an H+, as discussed before, a long pair must be present. Generally, a Base + H2O = (BH+) + (OH)
Are you sure you want to buy this material for
You're already Subscribed!
Looks like you've already subscribed to StudySoup, you won't need to purchase another subscription to get this material. To access this material simply click 'View Full Document'