Properties of Acids & Bases Taste Touch Reaction with Metals Sour Bitter Like H2O Slippery Yes, with most No, with most

Properties of Acids & Bases Both will conduct electricity when liquid or aqueous (electrolytes). Both take place in neutralization reactions.

Definitions of Acids Arrhenius Definition When dissolved in water, it separates to give off H+ ions. [http://wps.prenhall.com/wps/media/objects/476/488316/Instructor_Resources/Chapter_14/FG14_05.JPG]

H2SO4 (l)  2H+(aq) + SO4-2(aq) [http://wps.prenhall.com/wps/media/objects/476/488316/Instructor_Resources/Chapter_14/FG14_03-02b.JPG] H2SO4 (l)  2H+(aq) + SO4-2(aq) HNO3 (l)  H+(aq) + NO3-(aq)

Definitions of Acids Br∅nstead-Lowry Definition Donates H+ ions to other chemicals. [http://cwx.prenhall.com/bookbind/pubbooks/hillchem3/medialib/media_portfolio/text_images/CH15/FG15_00-03.JPG]

An acid will form the Hydronium Ion (H3O+) What about in H2O? An acid will form the Hydronium Ion (H3O+) [http://cwx.prenhall.com/bookbind/pubbooks/hillchem3/medialib/media_portfolio/text_images/CH15/FG15_00-02.JPG]

Definitions of Bases Arrhenius Definition When dissolved in water, it separates to give off OH- ions. [http://wps.prenhall.com/wps/media/objects/476/488316/Instructor_Resources/Chapter_14/FG14_06.JPG]

Definitions of Bases Br∅nstead-Lowry Def. Accepts H+ ions from other chemicals. [http://wps.prenhall.com/wps/media/objects/602/616516/Media_Assets/Chapter15/Text_Images/FG15_00-08UN.JPG]

Water becomes Hydroxide Ion (OH-) What about in H2O? Base accepts a H+ ion. Water becomes Hydroxide Ion (OH-) [http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/FG17_04_1C.JPG]

These dissociate completely in solution. Strong Acids & Bases These dissociate completely in solution. [http://wps.prenhall.com/wps/media/objects/476/488316/Instructor_Resources/Chapter_14/FG14_05.JPG] [http://wps.prenhall.com/wps/media/objects/476/488316/Instructor_Resources/Chapter_14/FG14_06.JPG]

Weak Acids & Bases These do not break up completely when placed in solution. Conjugate Acid Conjugate Base [http://wps.prenhall.com/wps/media/objects/476/488316/Instructor_Resources/Chapter_14/FG14_09-01un.JPG]

[http://wps.prenhall.com/wps/media/objects/476/488316/Instructor_Resources/Chapter_14/FG14_10.JPG]

Click here for a video clip on strong versus weak acids. [http://wps.prenhall.com/wps/media/objects/476/488316/Instructor_Resources/Chapter_14/FG14_12.JPG]

[http://cwx.prenhall.com/bookbind/pubbooks/mcmurry2/chapter15/medialib/FG15_001.JPG]

Weak Acids & Bases To determine how much an acid dissociates or “breaks-up” use this generic equation: HA(aq) + H2O(l) ⇆ H3O+(aq) + A-(aq)

Weak Acids & Bases Pg. 610

Weak Acids & Bases Example: If hydrofluoric acid (HF) has a starting concentration of 0.100 M, what will the concentration of H3O+ be? Ka for HF is 6.8 x 10-4

[H3O+] and [F-] are equal so… HF (aq) + H2O (l) ⇆ H3O+ (aq) + F- (aq) [H3O+] and [F-] are equal so… X = [H3O+] = 8.2x10-3 mol/L