I. Introduction toAcids & Bases

(p. 453 - 473)

Ch. 15 & 16 - Acids & Bases

15-1 Properties of Acids and Bases

electrolytes electrolytes

turn litmus red

sour taste

react with metals to form H2 gas

slippery feel

turn litmus blue

bitter taste

ChemASAP

vinegar, milk, soda, apples, citrus fruits

ammonia, lye, antacid, baking soda

Properties of Acids

Aqueous Solutions of Acids have a sour taste.• Citric Acid – Fruit

Acids change the color of Acid/Base indicators.• Litmus paper, pH paper, indicators…

Properties of Acids

Some metals react with metals to release hydrogen gas.• Use activity series to predict, pg. 266

Acids react with bases to produce “salts” and water.• “Neutralization”• HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)

Properties of Acids

Acids conduct an electric current.• “Electrolytes”

Nomenclature

“Binary Acids” – an acid that contains only two different elements.• HCl• HBr• HF• HI• H2S

Nomenclature

How to name?• Binary acids begin with “hydro-”• Root name of the second element.• Binary acid ends in “-ic”

Nomenclature

“Oxyacids”-an acid that is a compound of H and O + another element.• H2SO4

• HNO3

• HC2H3O2

• Name based on root of anion.

Industrial acids

Know the common uses of the industrial acids on pgs. 456-457

Properties of Bases

Aqueous Solutions of bases taste bitter.• Ex. Soap.

Bases change the color of acid/base indicators.• Ex. pH paper, litmus paper,

indicators…

Properties of Bases

Feel slippery.• Soap.

Bases react with acids to produce salts and water.• “neutralization”

Bases conduct electric current.• “electrolytes”

Definitions

“Arrhenius Acid” – a chemical compound that increases the concentration of H+ ions in aqueous solution.

“Arrhenius Base” – a chemical compound that increases the concentration of OH- ions in aqueous solution.

Definitions

ArrheniusArrhenius - In aqueous solution… - In aqueous solution…

HCl + H2O H3O+ + Cl– •AcidsAcids form hydronium ions (H3O+)

H

HH H H

H

Cl ClO O–+

acid

Definitions

ArrheniusArrhenius - In aqueous solution… - In aqueous solution…•BasesBases form hydroxide ions (OH-)

NH3 + H2O NH4+ + OH-

H

H

HH H

H

N NO O–+

HH

H H

base

Definitions

Know Strong Acids and Bases and Weak Acids and Bases• Pg. 460 and 461

15-2 Brøønsted-Lowry Acids and Bases

Brønsted-LowryBrønsted-Lowry

HCl + H2O Cl– + H3O+

•AcidsAcids are proton (H+) donors. •BasesBases are proton (H+) acceptors.

conjugate acidconjugate base

baseacid

Definitions

H2O + HNO3 H3O+ + NO3–

CBCAAB

Definitions

Amphoteric - can be an acid or a base. - can be an acid or a base.

NH3 + H2O NH4+ + OH-

CA CBB A

Definitions

F -

H2PO4-

H2O

HF

H3PO4

H3O+

Give the conjugate base for each of the following:

Polyprotic - an acid with more than one H - an acid with more than one H++

Definitions

Br -

HSO4-

CO32-

HBr

H2SO4

HCO3-

Give the conjugate acid for each of the following:

B. Definitions

LewisLewis•AcidsAcids are electron pair acceptors. •BasesBases are electron pair donors.

Lewis base

Lewis acid

C. Strength Strong Acid/BaseStrong Acid/Base

• 100% ionized in water• strong electrolyte

- +

HClHNO3

H2SO4

HBrHIHClO4

NaOHKOHCa(OH)2

Ba(OH)2

C. Strength Weak Acid/BaseWeak Acid/Base

• does not ionize completely• weak electrolyte

- +

HFCH3COOH

H3PO4

H2CO3

HCN

NH3