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:

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:

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

The pH scale

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)