a cids and bases. a cid, base, or neutral ? bitter taste doesn’t conduct electricity feels...
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ACIDS AND BASES
ACID, BASE, OR NEUTRAL? Bitter taste Doesn’t conduct electricity Feels slippery Dissolves metals Has no odor Has a strong, acrid odor Turns litmus blue Is unreactive Feels sticky Feels greasy Turns phenolphthalein solution red Dissolves grease Bubbles when baking soda is added Is oily
acid
base neutra
lbase
acidbase
or neutral
baseneutra
lneutra
l
acid
neutral
acidbase
acid
ARRHENIUS DEFINITION OF ACID AND BASE
ACID – hydrogen containing compound that ionizes to yield hydrogen ions (H+) in aqueous solution
BASE – compound that ionizes to yield hydroxide ions (OH-) in aqueous solution
IONIZABLE HYDROGENS Only hydrogens in very polar bonds
ionize.
Some acids have more than one ionizable hydrogen
DIPROTIC ACIDS 2 ionizable hydrogens (H2SO4 )TRIPROTIC ACIDS 3 ionizable hydrogens (H3PO4 )
This is the hydrogen that ionizes in acetic
acid
Carboxyl group
ARRHENIUS BASE OR ACID? Ca(OH)2
HNO3
KOH
C2H5COOH
HBr
H2SO4
Base Acid Base Acid Acid Acid
BRONSTED-LOWRY DEFINITION OF ACID AND BASE
ACID – hydrogen ion (H+) donor
BASE – hydrogen ion (H+) acceptor
IDENTIFY EACH REACTANT AS A HYDROGEN DONOR (ACID) OR HYDROGEN ACCEPTOR (BASE) HNO3 + H2O H3O+ + NO3
-
CH3COOH + H2O H3O+ + CH3COO-
NH3 + H2O NH4+ + OH-
H2O + CH3COO- CH3COOH + OH-
Acid
(donor)
Base
(acceptor)
Acid
(donor)
Acid
(donor)
Acid(donor)
Base
(acceptor)
Base
(acceptor)
Base(acceptor
)
Water acts as both a
hydrogen donor and hydrogen acceptor – it
acts as both an acid and a base.
It is AMPHOTERIC
CONJUGATE ACIDS & BASESCONJUGATE ACID – formed when a base
gains a hydrogen ionCONJUGATE BASE – formed when an
acid donates a hydrogen ion
NH3 and NH4+ are a
conjugate acid base pair
LABEL THE CONJUGATE ACID-BASE PAIRS HNO3 + H2O H3O+ + NO3
-
CH3COOH + H2O H3O+ + CH3COO-
NH3 + H2O NH4+ + OH-
H2O + CH3COO- CH3COOH + OH-
CBCA
CBCA
CACB
CBCA
LEWIS ACIDS AND BASES ACID – a substance
than can accept a pair of electrons to form a covalent bond
BASE – a substance than can donate a pair of electrons to form a covalent bond
SELF-IONIZATION OF WATER
2H2O (L) ⇆ H3O+(aq) + OH-(aq)
At any given time, there are only VERY small amounts of [H3O+] and [OH-] ions in water (1 molecule out of 550,000,000
dissociates) Water dissociates to form equal concentrations of
H3O+ and OH- making water neutralAt 25◦C, Kw = [H+] [OH-] = [1 x 10-7 ] [1 x 10-7 ] = 1 x 10-14
ION-PRODUCT CONSTANT OF WATER
ACIDIC SOLUTIONS VS. BASIC SOLUTIONS
[H+] is greater than [OH-]
[OH-] comes from self-ionization of water
Extra [H+] comes from substances that dissolve in water to create [H+]
[H+] is greater than 1x10-7
Acidic Solution Basic Solution
[H+] is less than [OH-] [H+] comes from self-
ionization of water Extra [OH-] comes from
substances that dissolve in water to create [H+]
[H+] is less than 1x10-7 Also known as alkaline
solution
ION CONCENTRATIONS IN ACIDIC, NEUTRAL AND BASIC SOLUTIONS
ACIDIC, BASIC OR NEUTRAL? [H+] = 6.0 x 10-10 M
[OH-] = 3.0 x 10-2 M
[H+] = 2.0 x 10-7 M
[OH-] = 1.0 x 10-7 M
[OH-][H+]= 1.0 x 10-
14
[H+]= 1.0 x 10-
14
3.0 x 10-
2 [H+] = 3.3 x 10-
13
Basic
Basic (hydrogen ion concentration is less than 1.0 x 10-7
Acidic (hydrogen ion concentration is greater than 1.0 x 10-7
Neutral
ACIDIC SOLUTIONS VS. BASIC SOLUTIONS
[H+] is greater than [OH-]
[OH-] comes from self-ionization of water
Extra [H+] comes from substances that dissolve in water to create [H+]
[H+] is greater than 1x10-7
pH < 7.0 pOH > 7.0
Acidic Solution Basic Solution
[H+] is less than [OH-] [H+] comes from self-
ionization of water Extra [OH-] comes from
substances that dissolve in water to create [H+]
[H+] is less than 1x10-7 Also known as alkaline
solution pH > 7.0 pOH < 7.0
MEASURING PH Acid-Base
Indicators – an acid or a base that: Dissociates in known
pH range Acid and base forms
are different colors in solution
Accuracy challenged by changes in temp & human error
pH meter Quick Accurate within .01
pH units
ACID RAIN
PH & POH
pH = –log[H+] pOH = –log[OH-] pH + pOH = 14
Use LOG key on calculator not LN to calculate pH!
Use antilog (10x) key on calculator to calculate M from pH
SAMPLE PROBLEMS
pH = -log[H+] pH = -log[8 x 10-11] pH = 10.10
Some calculators require that you push LOG key first while some require that you put in the # first then press LOG
pOH = -log[OH-] pOH = -log[2 x 10-3 ] pOH = 2.70
Some calculators may keep giving you errors if you try converting into – log. Just calculate using positive and switch the answer sign
What is the pH of a solution if the [H+] is 8 x 10-11 M?
What is the pOH of a solution if the [OH-] is 2 x 10-3 M?
SAMPLE PROBLEMS
pOH = -log[OH-] pOH = -log[3.5 x 10-
2 ] pOH = 1.46
pH + pOH = 14 14 – 1.46 = pH 12.54 = pH
M = mol solute / L solution35 g HNO3 / 63 g = .56 mol
M = .56 mol / 5.8 L = .097 M pH = -log[H+] pH = -log[.097 ] pH = 1.01
pH + pOH = 14 14 – 1.01 = 12.99 = pOH
What is the pH of a solution if the [OH-] is 3.5 x 10-2 M?
What is the pH & pOH of a solution made by adding water to 35 grams of nitric acid until the volume of the solution is 5800 mL?
PLACE THE FOLLOWING COMPOUNDS IN ORDER OF INCREASING [H+]
1M weak acid 1M strong acid 1M strong base 1M weak base
1M strong base 1M weak base 1M weak acid 1M strong acid
WRITE THE EXPRESSION FOR THE ACID DISSOCIATION CONSTANT OF THE STRONG ACID HF:
Ka = [H+ ][A- ]
[HA]
Ka = [H+ ][F- ]
[HF]
HF(aq) H+(aq) + F-
(aq)
WRITE THE EXPRESSION FOR THE BASE DISSOCIATION CONSTANT FOR THE WEAK BASE HYDRAZINE. HYDRAZINE REACTS WITH WATER TO FORM N2H5
+ ION
Kb = [OH- ][N2H5+ ]
[N2H4]
N2H4(aq) + H2O(l) N2H5+
(aq) + OH-(aq)
PLACE THE FOLLOWING ACIDS IN ORDER FROM WEAKEST TO STRONGEST (USE TABLE ON P.607)
HOOCCOOH HCO3
-
H2PO4-
HCOOH
HCO3-
H2PO4-
HCOOH HOOCCOOH
A .10M SOLUTION OF FORMIC ACID HAS AN EQUILIBRIUM [H+] = 4.2 X 10-3M. WHAT IS THE KA OF FORMIC ACID?
HCOOH(aq) H+(aq) + HCOO-
(aq)
(4.2 x 10-3 ) (4.2 x 10-3 ) (.10 – 4.2x10-3 )
Ka = 1.8 x 10-4