CHE 131 Lecture Notes - Lecture 11: Sulfuric Acid, Standard Solution, Equivalence Point

• School: Stony Brook University
• Department: Chemistry
• Course: CHE 131
• Professor: Benjamin Hsiao, Jiangyong Jia, Roy Lacey

Document Summary

Lecture 11 - electrolyte, acid-base reaction, titration (09/23/16: ions exist in equilibrium w/ unionized substance, no ionization - no conduction of electrical current ex. aqueous solutions of sugar, strong electrolytes: Conduct current efficiently ex. solutions of nacl, hno3, hcl: weak electrolytes: Slight conductive ex. vinegar (aqueous solution of acetic acid); tap water: bronsted-lowry acids are proton (h+) donors, bronsted-lowry bases are proton acceptors. ex. Hcl(aq) + h2o(l) > h3o+(aq) + cl-(aq) ex. Nh3(aq) + hc2h3o2(aq) > nh4+(aq) + c2h3o2-(aq: amphiprotic substances can behave as either a proton acceptor or a proton donor. ex. H2o: strong acids/bases: completely ionized in aqueous solution, weak acids/bases: dissociate only partially. Use reverse arrows to indicate incomplete reaction to form ions: strong bases. Group 1a hydroxides: hcl + naoh > nacl + h2o. A neutralization reaction takes place when an acid reacts with a base and produces a solution of a salt and water.