[CHM1301] - Final Exam Guide - Everything you need to know! (90 pages long)

• School: University of Ottawa
• Department: Chemistry
• Course: CHM 1301
• Professor: Mathew L

Document Summary

The strength of an oxoacid or carboxylic acid increases as electron density is withdrawn from the o-h bond: Acid-base equilibrium are part of larger acid-base equilibria: Usually, we focus our attention on other major species (nh3) Need to consider the water equilibrium"s effect on h3o+ and oh- concentrations. Polyprotic acids : contains more than one acidic hydrogen. Polyprotic acids are best example where you need to calculate secondary equilibrium. Ka2 < ka1 due to charge effect. Carbonated water contains carbonic acid, a diprotic acid that forms when carbon dioxide dissolves in water. A typical carbonate beverage contains 0. 050 m h2co3. Determine the concentrations of the ions present in this solution. Co2 (g) + h2o (l) h2co3 (aq) First: consider the acid dissociation constant of the first proton: Hco3- (aq) + h2o (l) h3o+ (aq) + co32- (aq) Because ka1> ka2, we can say that ka1 is the dominant equilibria. So, we know the dominant equilibrium but: