Unit 9 Acids and BasesChapter 14
Acids:Any compound that releases H+ ions when dissolved in water.
An Arrhenius acid:
An Arrhenius acid:Contains H+, which is liberated
when dissolved in water.
An Arrhenius acid:Contains H+ which is liberated
when dissolved in water.
An Arrhenius base:
An Arrhenius acid:Contains H+ which is liberated
when dissolved in water.
An Arrhenius base:Contains OH-, which is liberated
when dissolved in water.
Naming acids: ! ! ! See notes from April 16! ! ! ! and pages 442-443
Strong Acids: acids that will 100% ionize in water.
Notable strong acids:
! ! HCl! ! ! ! HBr! ! ! ! ! HI! ! HNO3!! ! HClO4!! ! ! H2SO4
Notable strong acids:
! ! HCl! ! ! ! HBr! ! ! ! ! HI! ! HNO3!! ! HClO4!! ! ! H2SO4
Note: most acidsare weak acids
(which only partially ionize)
Organic acids are all weakacids that contain the carboxyl group: -COOH
Strong bases:All contain OH- and will 100% dissociate (ionize).
Strong bases:All contain OH- and will 100% dissociate (ionize).
Notable strong Bases:! ! NaOH!! ! ! KOH!! ! ! RbOH
Strong bases:All contain OH- and will 100% dissociate (ionize).
Notable strong Bases:! ! NaOH!! ! ! KOH!! ! ! RbOH! ! Ca(OH)2! ! Ba(OH)2! Sr(OH)2
A Brønsted-Lowry Acid:
A Brønsted-Lowry Acid:a proton donor
Brønsted-Lowry Base:
Brønsted-Lowry Base:a proton acceptor
Common Acid-Base Reactions:
1. Acid + Metal ---> H2(g) + *salt! ! ! ! ! ! ! *salt: an ionic compound ! ! ! ! ! ! ! composed of an anion ! ! ! ! ! ! ! from an acid.
1. Acid + Metal ---> H2(g) + saltNotable exceptions:Acid + Cu, Pt, Ag, or Au ! ! ! ! ! ! ! ! ! ----> No Reaction!! (these metals are less !! ! !! )
1. Acid + Metal ---> H2(g) + saltNotable exceptions:Acid + Cu, Pt, Ag, or Au ! ! ! ! ! ! ! ! ! ----> No Reaction!! (these metals are less active)
!
2. Neutralization reactions
2. Neutralization reactionsAcid + Base ---> H2O + salt
3. Acid + a carbonate
3. Acid + a carbonate! ! ! ! ! ! (CO32- or HCO3-)
3. Acid + a carbonate! ! ----> H2O + salt + CO2(g)
4. Nonmetal oxides + water:
4. Nonmetal oxides + water! ! ! ! ! ! ! ! ! ! ! ! ! ---> oxyacid
Best example:CO2(g) + H2O(l) --->
Best example:CO2(g) + H2O(l) ---> H2CO3(aq)
CO2(g) + H2O(l) --->
CO2(g) + H2O(l) ---> H2CO3This makes all water exposed to the atmosphere slightly acidic!
Acids can be,1. monoprotic (donates 1 proton)
An acid can be,1. monoprotic (donates 1 proton)2. diprotic (donates 2 proton)
An acid can be,1. monoprotic (donates 1 proton)2. diprotic (donates 2 proton)3. triprotic (donates 3 proton)
Conjugate acid-base pairs
Conjugate acid-base pairs: differ by one proton (hydrogen ion).
Amphoteric: Any substance that can behave as either an acid or a base. ! ! !! ! ! (e.g., H2O or HPO42-)
Properties of Acids:
Properties of Acids:• Ionize in water
Properties of Acids:• Ionize in water• An electrolyte
Properties of Acids:• Ionize in water• An electrolyte• Reacts with more active
metals
Properties of Acids:• Ionize in water• An electrolyte• Reacts with more active
metals• Affects the color of acid-base
indicators
Properties of Acids:• Ionize in water• An electrolyte• Reacts with more active
metals• Affects the color of acid-base
indicators • Sour taste
Properties of Bases:
Properties of Bases:• Ionize in water
Properties of Bases:• Ionize in water• An electrolyte
Properties of Bases:• Ionize in water• An electrolyte• Affects the color of acid-base
indicators
Properties of Bases:• Ionize in water• An electrolyte• Affects the color of acid-base
indicators• Feels slippery (soaps!)
Properties of Bases:• Ionize in water• An electrolyte• Affects the color of acid-base
indicators• Feels slippery (FYI: soaps are basic!)• Tastes bitter
Indicators: organic compounds used to determine the approximate pH of a solution.
Common IndicatorsCommon IndicatorsCommon IndicatorspH range pH range
phenolphthalein 0 - 8.3 (clear) greater than 8.1 (pink)litmus less than 4.7 (red) greater than 6.8 (blue)
methyl red less than 4.4 (red) greater than 6.0 (yellow)