Things to PonderThings to Ponder

• The nicest thing about the future is that it always starts tomorrow.

Deal with the faultsof others as gentlyas with your own!

Deal with the faultsof others as gentlyas with your own!

Acid-BasesAcid-Bases

Lesson2

Acid ReactionsAcid Reactions

Problem Problem

• How would you prepare 5.0 L of a 1.5 M solution of glucose?

• First chemical formula for glucose is ?

• C6H12O6

WorkWork

• Find the molar mass of glucose

• Molar mass of glucose = 180.18 g C6H12O6

Work ContWork Cont• 1.5 mol C6H12O6 180.18 g C6H12O6 5.0 L solution

1 L solution 1 mol C6H12O6

• Answer= 1351.35 g C6H12O6

Write as Put 1351.35 g C6H12O6 in a 5.0 L

container and add enough water to get 5.0 L.

Properties of Acids and Bases

Properties of Acids and Bases

• Although taste is not a safe way to classify acids and bases, you probably are familiar with the sour taste of acids.

Acid Acid

• Contain hydrogen ion (H+) • pH < 7• Taste sour• Electrolyte• Reacts with metals that are more

reactive than H+ .• [acidus is latin for sour]

Examples of AcidsExamples of Acids

• Lemon juice

• Vinegar (Acetic Acid)

• Hydrochloric Acid

Metal Activity ChartMetal Activity Chart Li

KBaSrCaNa

MgAlMnZnCr

Most Active FeCdCoNiSn

Pb HCu

BiSbHgAgPtAu

Least Active

Corrosion Corrosion

• Oxidation of metals or substances.

Bases Bases

• Contain hydroxide ion (OH-)• pH > 7• Taste bitter• Feels slippery• Weak electrolyte

ExamplesExamples

• Soaps• Baking soda• Sodium Hydroxide

Alkaline solutions Alkaline solutions

• Another name for basic solutions

Hydronium ion Hydronium ion

• H3O+

• Is a H+ attached to a water molecule.

• Results in an acidic hydrogen

Monoprotic acids Monoprotic acids

• Have only one acidic hydrogen. (Ex: HCl)

Diprotic acid Diprotic acid • Has 2 acidic hydrogens.

Triprotic acid Triprotic acid

• Contains 3 acidic hydrogens.

ACID-BASE THEORIESACID-BASE THEORIESACID-BASE THEORIESACID-BASE THEORIES

• The most general theory for The most general theory for common aqueous acids and common aqueous acids and

bases is the bases is the BRØNSTED - BRØNSTED - LOWRY LOWRY theorytheory

•ACIDS DONATE HACIDS DONATE H++ IONS IONS

•BASES ACCEPT HBASES ACCEPT H++ IONS IONS

Bronsted - Lowrey Bronsted - Lowrey

• Came up with a theory that states an acid is a H+ donor, a base as a H+ acceptor.

pH range 0-14 pH range 0-14

Common acids/basesCommon acids/bases

Kw - ion - product constant for H2O = 1 x 10 -14 (mol / L)2

Kw - ion - product constant for H2O = 1 x 10 -14 (mol / L)2

Kw = [H+] x [OH -]

Remember Kw = 1 x 10 -14 (mol / L)2

Kw = [H+] x [OH -]

Remember Kw = 1 x 10 -14 (mol / L)2

Problem Problem • Find the [ OH-] if the [ H+ ] = 1 x 10-5 M

• Work

• 1 x 10 -14 (mol / L)2 = 1 x 10-5 M x [ OH-] • Answer:• [ OH-] = 1 x 10 -9 M

Problem Problem • Find the [ H+ ] if the [OH- ] = 1 x 10-3 M.

• Work• 1 x 10 -14 (mol / L)2 = 1 x 10-3 M x [ H+ ]

• Answer:• [ H +] = 1 x 10 -11 M

pH = - log [H +] pH = - log [H +]

Note: Must be the hydrogen ion NOT the hydroxide.

Number used to denote the hydrogen - ion concentration , of a solution it is the negative logarithm of the H+ ion concentration of a solution

Note: Must be the hydrogen ion NOT the hydroxide.

Number used to denote the hydrogen - ion concentration , of a solution it is the negative logarithm of the H+ ion concentration of a solution

Problem: Problem:

• Find the pH if the [H+] = 1 x 10 -10 M .

• Is this an acid or base.

• Answer• Base

WorkWork• Using calculator if you have the [H+ ]

put this number in then hit LOG and multiply by -1.

• pH = - ( 1 x 10 -10 M)

• hit LOG • Answer=• pH = 10 therefore this is a base.