This document discusses acid-base concepts including definitions of acids and bases according to different theories like Arrhenius, Brønsted-Lowry, and Lewis. It describes types of salts like acidic, basic, and neutral salts formed from strong and weak acids and bases. Buffers are discussed including bicarbonate, phosphate, and protein buffers. The roles of the respiratory and renal systems in acid-base regulation are summarized. Respiratory and metabolic acidosis and alkalosis are also briefly covered.

1. Niamat Ullah
Post Rn BScN
Life Saving SON

2.  ACID BASE CONCEPT
 TYPES OF SALT
 BUFFER AND ITS TYPES RELATION WITH
RESPIRATORY AND RENAL SYSTEM
2LIFE SAVING SON

3.  Acid: a substance that produces H+ when
dissolved in water (e.g., HCl, H2SO4)
 Base: a substance that produces OH-
when
dissolved in water (NaOH, KOH)
 What about water?
3LIFE SAVING SON

4.  Acids – produce H+
 Bases - produce OH-
 Acids – donate H+
 Bases – accept H+
 Acids – accept e-
pair
 Bases – donate e-
pair
Arrehenius
Bronsted-Lowry
Lewis
only in water
any solvent
used in organic chemistry,
wider range of substances
4LIFE SAVING SON

5. The Swedish chemist Svante Arrhenius proposed the first
definition of acids and bases.
(Substances A and B became
known as acids and bases)
According to the Arrhenius model:
“acids are substances that dissociate in water to
produce H+
ions and bases are substances that
dissociate in water to produce OH-
ions”
NaOH (aq)  Na+
(aq) + OH-
(aq) Base
HCl (aq)  H+
(aq) + Cl-
(aq) Acid
5LIFE SAVING SON

6. +
e-
+
Hydrogen (H) Proton (H+
)
6LIFE SAVING SON

7. Unknown to Arrhenius free H+
ions do not exist in water. They
covalently react with water to produce hydronium ions, H3O+
.
or:
H+
(aq) + H2O (l)  H3O+
(aq)
This new bond is called a coordinate covalent bond since
both new bonding electrons come from the same atom
7LIFE SAVING SON

8. Memorized Strong Acids
1. HClO4
2. H2SO4
3. HI
4. HBr
5. HCl
6. HNO3
Memorized Strong Bases
Hydroxides of group 1 and 2
metals, excluding Be and Mg
Strong Acids and Bases
8LIFE SAVING SON

9. Johannes Brønsted and Thomas Lowry revised
Arrhenius’s acid-base theory to include this behavior.
They defined acids and bases as follows:
“An acid is a hydrogen containing species that
donates a proton. A base is any substance that
accepts a proton”
HCl (aq) + H2O (l)  Cl-
(aq) + H3O+
(aq)
In the above example what is the Brønsted acid? What is
Bronsted Lowry
Bronsted Lowry Theory
9LIFE SAVING SON

10.  The Brønsted-Lowry acid: any substance able to
give a hydrogen ion (H+-a proton) to another
molecule
◦ Monoprotic acid: HCl, HNO3, CH3COOH
◦ Diprotic acid: H2SO4
◦ Triprotic acid: H3PO3
 Brønsted-Lowry base: any substance that accepts a
proton (H+) from an acid
◦ NaOH, NH3, KOH
10LIFE SAVING SON

11.  A proton is transferred from one substance (acid)
to another molecule
Ammonia (NH3) + acid (HA) → ammonium ion (NH4
+
) + A-
◦ Ammonia is base
◦ HA is acid
◦ Ammonium ion (NH4
+
) is conjuagte acid
◦ A-
is conjugate base
11LIFE SAVING SON

12. 12LIFE SAVING SON

13. 13LIFE SAVING SON

14. In the early days of chemistry chemists were organizing
physical and chemical properties of substances. They
discovered that many substances could be placed in two
different property categories:
Substance A
1. Sour taste
2. Reacts with carbonates to make CO2
3. Reacts with metals to produce H2
4. Turns blue litmus pink
5. Reacts with B substances to make
salt water
Substance B
1. Bitter taste
2. Reacts with fats to make soaps
3. Do not react with metals
4. Turns red litmus blue
5. Reacts with A substances make
salt and water
Arrhenius was the first person to suggest a reason why
substances are in A or B due to their ionization in water.
14LIFE SAVING SON

15.  Electrolytes
◦ Cations: sodium, potassium, hydrogen, magnesium,
and calcium
◦ Anions: chloride, bicarbonate, phosphate, and sulfate
 Non-electrolytes
◦ Glucose
◦ Urea
◦ Protein
◦ Lipids
◦ Creatinine
15LIFE SAVING SON

16. Major
electrolytes
1 Eq mEq/L Physiological
gram
Na+ = 23.1 g 136-145 ?
Cl- - 35.5 g 98-106 ?
Mg+2 (24.3)/2 = 12.15 g 3 ?
Ca2+ (40.1/2) = ~20.05
g
4.5-6.0 ?
K+ 39.1 g 3.4-5.0 ?
HCO3- 61 g 25-29 ?
SO3-2
and HPO4
3- 2 ?
16LIFE SAVING SON

17. pH
2 3 4 5 6 7 8 9 10 11 12
neutral @ 25o
C
(H+
) = (OH-
)
distilled water
acidic
(H+
) > (OH-
)
basic or alkaline
(H+
) < (OH-
)
natural waters
pH = 6.5 - 8.5
normal rain (CO2)
pH = 5.3 – 5.7
acid rain (NOx, SOx)
pH of 4.2 - 4.4 in
Washington DC area
0-14 scale for the chemists
fish populations
drop off pH < 6 and
to zero pH < 5
17LIFE SAVING SON

18. Salts are the ionic product of an acid base neutralization
reaction.
Acidic Salts are formed from a strong acid and a weak base.
Neutral salts are formed from a strong acid and strong base.
Basic salts are formed from a strong base and a weak acid.
Give the acid and base the following salts were formed from
and label the salts as acidic, basic, or neutral.
1. NaCl
2. NaC2H3O2
3. NH4Cl
18LIFE SAVING SON

19. Salts are the ionic product of an acid base neutralization
reaction.
Acidic Salts are formed from a strong acid and a weak base.
Neutral salts are formed from a strong acid and strong base.
Basic salts are formed from a strong base and a weak acid.
Give the acid and base the following salts were formed from
and label the salts as acidic, basic, or neutral.
1. NaCl
1. NaC2H3O2
1. NH4Cl
NaCl + HOHReactants are?
19LIFE SAVING SON

20. Salts are the ionic product of an acid base neutralization
reaction.
Acidic Salts are formed from a strong acid and a weak base.
Neutral salts are formed from a strong acid and strong base.
Basic salts are formed from a strong base and a weak acid.
Give the acid and base the following salts were formed from
and label the salts as acidic, basic, or neutral.
1. NaCl
2. NaC2H3O2
3. NH4Cl
NaCl + HOHHCl + NaOH
NaC2H3O2 + HOH
S.A. s.b.
20LIFE SAVING SON

21. Salts are the ionic product of an acid base neutralization
reaction.
Acidic Salts are formed from a strong acid and a weak base.
Neutral salts are formed from a strong acid and strong base.
Basic salts are formed from a strong base and a weak acid.
Give the acid and base the following salts were formed from
and label the salts as acidic, basic, or neutral.
1. NaCl
2. NaC2H3O2
3. NH4Cl
NaCl + HOHHCl + NaOH
NaC2H3O2 + HOH
S.A. s.b.Neutral salt
21LIFE SAVING SON

22. Salts are the ionic product of an acid base neutralization
reaction.
Acidic Salts are formed from a strong acid and a weak base.
Neutral salts are formed from a strong acid and strong base.
Basic salts are formed from a strong base and a weak acid.
Give the acid and base the following salts were formed from
and label the salts as acidic, basic, or neutral.
1. NaCl
2. NaC2H3O2
3. NH4Cl
NaCl + HOHHCl + NaOH
NaC2H3O2 + HOHHC2H3O2 + NaOH
Neutral salt s.a. s.b.
22LIFE SAVING SON

23. Salts are the ionic product of an acid base neutralization
reaction.
Acidic Salts are formed from a strong acid and a weak base.
Neutral salts are formed from a strong acid and strong base.
Basic salts are formed from a strong base and a weak acid.
Give the acid and base the following salts were formed from
and label the salts as acidic, basic, or neutral.
1. NaCl
2. NaC2H3O2
3. NH4Cl
NaCl + HOHHCl + NaOH
NaC2H3O2 + HOHHC2H3O2 + NaOH
w.a. s.b.
Neutral salt s.a. s.b.
23LIFE SAVING SON

24. Salts are the ionic product of an acid base neutralization
reaction.
Acidic Salts are formed from a strong acid and a weak base.
Neutral salts are formed from a strong acid and strong base.
Basic salts are formed from a strong base and a weak acid.
Give the acid and base the following salts were formed from
and label the salts as acidic, basic, or neutral.
1. NaCl
2. NaC2H3O2
3. NH4Cl
NaCl + HOHHCl + NaOH
NaC2H3O2 + HOHHC2H3O2 + NaOH
w.a. s.b.basic salt
Neutral salt s.a. s.b.
24LIFE SAVING SON

25. Salts are the ionic product of an acid base neutralization
reaction.
Acidic Salts are formed from a strong acid and a weak base.
Neutral salts are formed from a strong acid and strong base.
Basic salts are formed from a strong base and a weak acid.
Give the acid and base the following salts were formed from
and label the salts as acidic, basic, or neutral.
1. NaCl
2. NaC2H3O2
3. NH4Cl
NaCl + HOHHCl + NaOH
NaC2H3O2 + HOHHC2H3O2 + NaOH
w.a. s.b.basic salt
Neutral salt s.a. s.b.
NH4Cl + HOH
25LIFE SAVING SON

26. Salts are the ionic product of an acid base neutralization
reaction.
Acidic Salts are formed from a strong acid and a weak base.
Neutral salts are formed from a strong acid and strong base.
Basic salts are formed from a strong base and a weak acid.
Give the acid and base the following salts were formed from
and label the salts as acidic, basic, or neutral.
1. NaCl
2. NaC2H3O2
3. NH4Cl
NaCl + HOHHCl + NaOH
NaC2H3O2 + HOHHC2H3O2 + NaOH
w.a. s.b.basic salt
Neutral salt s.a. s.b.
NH4Cl + HOHNH4OHHCl +
26LIFE SAVING SON

27. Salts are the ionic product of an acid base neutralization
reaction.
Acidic Salts are formed from a strong acid and a weak base.
Neutral salts are formed from a strong acid and strong base.
Basic salts are formed from a strong base and a weak acid.
Give the acid and base the following salts were formed from
and label the salts as acidic, basic, or neutral.
1. NaCl
2. NaC2H3O2
3. NH4Cl
NaCl + HOHHCl + NaOH
NaC2H3O2 + HOHHC2H3O2 + NaOH
w.a. s.b.basic salt
Neutral salt s.a. s.b.
NH4Cl + HOHNH4OHHCl +
s.a. w.b.
27LIFE SAVING SON

28. Salts are the ionic product of an acid base neutralization
reaction.
Acidic Salts are formed from a strong acid and a weak base.
Neutral salts are formed from a strong acid and strong base.
Basic salts are formed from a strong base and a weak acid.
Give the acid and base the following salts were formed from
and label the salts as acidic, basic, or neutral.
1. NaCl
2. NaC2H3O2
3. NH4Cl
NaCl + HOHHCl + NaOH
NaC2H3O2 + HOHHC2H3O2 + NaOH
w.a. s.b.basic salt
neutral salt s.a. s.b.
NH4Cl + HOHNH4OHHCl +
s.a. w.b.acidic salt 28LIFE SAVING SON

29. Three Types:
Bicarbonate Buffers
Phosphate Buffers
Protein Buffers

30.  WHAT IS BUFFER?
30LIFE SAVING SON

31. Buffer solution is typically made by mixing a weak acid
and one of its salts OR mixing a weak base with one of its
salts. Another way of saying this is that a buffer solution
consists of a mixture of a weak acid and its conjugate base
OR a weak base and its conjugate acid
.
Example: Consider a solution containing both acetic acid,
CH3
COOH, and acetate ions, CH3
COO-
. (Alternatively,
these could be called ethanoic acid and ethanoate ions.)
This solution could be made by dissolving sodium acetate
(sodium ethanoate) in acetic acid (ethanoic acid).
Any strong base that is added to the solution is
neutralized by the acetic acid:
CH COOH + OH-
CH COO-
+ H O 31LIFE SAVING SON

32. Any strong acid that is added to the solution is
neutralized by the acetate:
CH3
COO-
(aq)
+ H+
(aq)
CH3
COOH (aq)
The amount of strong acid or base that a buffer
can neutralize is called the buffer capacity.
32LIFE SAVING SON

33.  Major extracellular buffering system
 HCO3
-
functions as a weak base while H2CO3
functions as a weak acid.
 Example:
HCl + NaHCO3- H2CO3 + NaCl
33LIFE SAVING SON

34.  Important in urine and intracellular buffering
systems
 However NaH2PO4 acts as the weak acid and
Na2HPO4 serves as the weak base.
 Example:
HCl + Na2HPO4 NaH2PO4 + NaCl
34LIFE SAVING SON

35.  Most abundant buffering system in the body
including intracellular and extracellular
compartments.
 Carboxyl groups (COOH) and amine groups (NH3)
act as either an acid or a base respectively.
35LIFE SAVING SON

36. Two Types:
Respiratory Buffering System
Renal Buffering System

37.  Rising plasma H+
causes deeper, rapid breathing which
decreases CO2blood thereby decreasing H+
ions.
37LIFE SAVING SON

38. Reabsorption of HCO3
-
is coupled to H+
secretion
38LIFE SAVING SON

39.  Respiratory acidosis
 Increased CO2=increased H+
=decreased pH
 Cause: Hypoventilation
 To compensate: Kidney function=increase excretion of H+ or
by increased reabsorption of HCO3-
 Respiratory alkalosis
 Decreased CO2=decreased H+
=increased pH
 Cause: Hyperventilation
 To compensate: Kidney function=decreased H+ excretion or
by decreased reabsorption of HCO3-
39LIFE SAVING SON

40.  Metabolic acidosis
 Decreased HCO3
-
=increased H+
=decreased pH
 Cause: Diarrhea, ketosis, renal dysfunction
 To compensate: Hyperventilation and kidney function
 Metabolic alkalosis
 Increased HCO3
-
=decreased H+
=increased pH
 Cause: Vomiting, diuretics, alkaline drug use
 To compensate: Hypoventilation and kidney function
40LIFE SAVING SON

41. 41LIFE SAVING SON