i. introduction to acids & bases (p. 453 - 473) ch. 15 & 16 - acids & bases
DESCRIPTION
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…TRANSCRIPT
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