Acid and base
Acid and base
Iman AlAjeyan
Acid-Base Theory
Acid-Base Theory
Acids in water solutions show certain
properties. They taste sour and turn
litmus paper red. They react with
metals like zinc to give off hydrogen.
•
Arrhenus Theory
Arrhenus Theory
Acid-
Acid-
is any substance that ionizes partially or
is any substance that ionizes partially or
completely in water to give hydrogen ions
completely in water to give hydrogen ions
Base-
Base-
Any substance that ionizes in water to
Any substance that ionizes in water to
give hydroxide ions (OH-)
give hydroxide ions (OH-)
E.g: (NaOH)
E.g: (NaOH)
NaOH ---> Na+ + OH-
NaOH ---> Na+ + OH-
Brønsted – Lowry Theory
Acid
Acid
is a substance that can donate a proton (H+)
Base
Base
is a substance that can accept a proton (H+)
Acid = H
Acid = H
+
+
+ base
+ base
Lewis
Acid is a species that accepts a pair of electrons
from another species; in other words, it is an
electron pair acceptor.
Base is any species that donates a pair of
electrons to a Lewis acid
Lewis
Strong acids and bases complete
dissociate in water.
Weak acids and bases dissociate only
partially and reversibly.
Conjugate acid base pairs
Conjugate acid base pairs
•
Conjugate base
Conjugate base
:
:
the species that remains after
an acid has given up a proton
•
Conjugate acid
Conjugate acid
:
:
the species that is formed
when a base gains a proton
NH
3
+ H
2
O
4
+
+ OH
-
acid
base
•
In the two examples water first acts as a base,
then as an acid.
•
Any species which can both accept and
receive protons is called
amphiprotic
.
(also
known as amphoteric)
pH Scale
The concentration of hydrogen ions in a
solution is very important for living things.
The concentration of hydrogen ions is
commonly expressed in terms of the pH
scale.
Low pH
corresponds to
high hydrogen
ion concentration
and vice versa.
A substance that when added to water
increases the concentration of hydrogen
ions(lowers the pH) is called an
acid
. A
substance that reduces the concentration
of hydrogen ions(raises the pH) is called a
base
.
pH Scale
pH Scale
•
Measures the degree of acidity (0 – 14)
•
Most biologic fluids are in the pH range from
6 – 8
•
Each pH unit represents a tenfold difference
in the concentration of hydrogen ions (scale
is logarithmic)
–
A small change in pH actually indicates a
substantial change in H
+
and OH
-
concentrations.
–
When the concentration of H+ ions in a solution
is 10
-14
, the pH is 14.
–
In pure water, the average concentration of H+
ions is 10
-7
Buffers
Buffers
•
Solutions which resist changes in pH
when a small amount of an acid or base
is added, or when the solution is diluted.
This is a very useful for maintaining the
pH for a reaction at an optimum value.
A buffer solution consists of a mixture of a
weak acid and its conjugate base or a weak
base and its conjugate acid. That is we have
a weak acid and its salt or a weak base and
its salt
Buffers
Buffers
Buffers help organisms maintain the pH of
body fluids within the narrow range
necessary for life.
Buffers are combinations of H+ acceptors
and donors forms in a solution of weak
acids or bases.
Work by accepting H+ from solutions when
they are in excess and by donating H+ when
they have been depleted.
Buffers
Buffers
Buffering Capacity
The amount of acid or base that can be added without
causing a large change in pH.
Physiological buffers
Normal blood pH : 7.3 – 7.45
Blood maintain to pH due to presence of buffers in it.
Yours buffer system in Blood.
Hemoglobin & oxyhemoglobin : 62%
H
2
PO
-
4
/ HPO
2-
4
: 22%
Plasma protein: 11%
Bicarbonate : 5%
Review 2:
Name the acid, base, conjugate acid and base for each reaction.
CH
3
NH
2
+ H
2
O
CH
3
NH
3
+
+
OH
-
H
3
PO
4
+ H
2
O
H
3
O
+
+
H
2
PO
4
-
HC
2
H
3
O
2
+ H
2
O
H
3
O
+
+
C
2
H
3
O
2
-
CH
3
NH
3
+
+ H
2
PO
4
-
H
3
PO
4
+ CH
3
NH
2
base
base
base
base
acid
acid
acid
acid
conjugate acid
conjugate acid
conjugate acid
conjugate acid
conjugate base
conjugate base
conjugate base
conjugate base
Review 2:
Name the acid, base, conjugate acid and base for each reaction.
H
2
PO
4
-
+ OH
-
HPO
4
2-
+
H
2
O
HCN + H
2
O
CN
-
+
H
3
O
+
NH
3
+ H
2
O
N
H
4
+
+
OH
-
NO
2
-
+ HCO
3
-
CO
3
2-
+ HNO
2
acid
base
acid
acid
base
acid
base
base
conjugate base
conjugate base
conjugate acid
conjugate base
conjugate acid
conjugate acid
conjugate base
conjugate acid
Cluster shape-based techniques are explored to enhance the spatial resolution of the Belle II SVD and PXD detectors through the analysis of various pixel cluster configurations. This study, conducted at the 6th Belle II PXD/SVD workshop in Pisa, Italy, presents findings on cluster categorization, hit position estimation for different cluster sizes, and bias correction methods. The use of cluster shape information allows for improved accuracy in determining hit positions, with a focus on addressing biases in center-of-gravity estimates. The research, led by Peter Kody from Charles University in Prague, showcases advancements in tracking technology for particle detection at Belle II.
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Presentation Transcript
Acid and base Iman AlAjeyan
Acid Acid- -Base Theory Base Theory
Acids in water solutions show certain properties. They taste sour and turn litmus paper red. They react with metals like zinc to give off hydrogen.
Arrhenus Theory Acid completely in water to give hydrogen ions Acid- - is any substance that ionizes partially or Base give hydroxide ions (OH-) E.g: (NaOH) NaOH ---> Na+ + OH- Base- - Any substance that ionizes in water to
Brnsted Lowry Theory Acid Base Acid is a substance that can donate a proton (H+) Base is a substance that can accept a proton (H+) Acid = H Acid = H+ + + base + base
Lewis Acid is a species that accepts a pair of electrons from another species; in other words, it is an electron pair acceptor. Lewis Base is any species that donates a pair of electrons to a Lewis acid
Strong acids and bases complete dissociate in water. Weak acids and bases dissociate only partially and reversibly.
Table of Common Acids Hydrochloric - Carbonic - Sulfuric - Acetic - Nitric - Phosphoric - Citric - Lactic - Table of Common Acids - - HCl H2CO3 H2SO4 HC2H3O2 HNO3 H3PO4 H3C6H8O6 HC3H5O
Table of Common Bases Sodium Hydroxide Potassium Hydroxide Magnesium Hydroxide Calcium Hydroxide Ammonium Hydroxide Ammonia Sodium Carbonate Sodium Phosphate NaOH KOH Mg(OH)2 Ca(OH)2 NH4OH NH3 Na2CO3 Na3PO4
Conjugate acid base pairs Conjugate acid base pairs Conjugate an acid has given up a proton Conjugate base an acid has given up a proton base: the species that remains after the species that remains after Conjugate when a base gains a proton Conjugate acid when a base gains a proton acid: : the species that is formed the species that is formed
base acid NH3 + H2O NH4+ + OH- conjugate base conjugate acid
In the two examples water first acts as a base, then as an acid. Any species which can both accept and receive protons is called amphiprotic known as amphoteric) amphiprotic. (also
pH Scale pH Scale The concentration of hydrogen ions in a solution is very important for living things. The concentration of hydrogen ions is commonly expressed in terms of the pH scale. Low pH corresponds to high hydrogen ion concentration and vice versa.
pH Scale pH Scale A substance that when added to water increases the concentration of hydrogen ions(lowers the pH) is called an acid. A substance that reduces the concentration of hydrogen ions(raises the pH) is called a base.
pH Scale pH Scale Measures the degree of acidity (0 14) Most biologic fluids are in the pH range from 6 8 Each pH unit represents a tenfold difference in the concentration of hydrogen ions (scale is logarithmic) A small change in pH actually indicates a substantial change in H+ and OH- concentrations. When the concentration of H+ ions in a solution is 10-14, the pH is 14. In pure water, the average concentration of H+ ions is 10-7
Buffers Buffers Solutions which resist changes in pH when a small amount of an acid or base is added, or when the solution is diluted. This is a very useful for maintaining the pH for a reaction at an optimum value.
Buffers Buffers A buffer solution consists of a mixture of a weak acid and its conjugate base or a weak base and its conjugate acid. That is we have a weak acid and its salt or a weak base and its salt
Buffers Buffers Buffers help organisms maintain the pH of body fluids within the narrow range necessary for life. Buffers are combinations of H+ acceptors and donors forms in a solution of weak acids or bases. Work by accepting H+ from solutions when they are in excess and by donating H+ when they have been depleted.
Buffering Capacity The amount of acid or base that can be added without causing a large change in pH. Buffering Capacity Physiological buffers Normal blood pH : 7.3 7.45 Blood maintain to pH due to presence of buffers in it. Physiological buffers Yours buffer system in Blood. Hemoglobin & oxyhemoglobin : 62% H2PO-4 / HPO2-4 : 22% Plasma protein: 11% Bicarbonate : 5%
Review 2: Name the acid, base, conjugate acid and base for each reaction. CH3NH3+ + conjugate acid OH - CH3NH2 + H2O conjugate base base acid H3O + conjugate acid H2PO4- conjugate base H3PO4 + H2O + acid base H3O + C2H3O2- HC2H3O2 + H2O + acid base conjugate acid conjugate base CH3NH3+ + H2PO4- acid H3PO4 conjugate acid + CH3NH2 conjugate base base
Review 2: Name the acid, base, conjugate acid and base for each reaction. H2PO4- + OH- HPO42- conjugate base + H2O conjugate acid acid base CN- + H3O + conjugate base HCN + H2O conjugate acid acid base NH4+ OH - NH3 + H2O + base acid conjugate acid conjugate base NO2- + HCO3- base CO32- conjugate base + HNO2 conjugate acid acid
