This document provides information about acids and bases. It defines acids as substances that donate protons and bases as those that accept protons, according to the Bronsted-Lowry theory. Examples of strong acids that ionize completely in water are provided. Acids and bases are both electrolytes that form ions and conduct electricity in water. The pH scale is introduced as a measure of the concentration of hydrogen ions in a solution, with lower pH indicating higher acidity.
Chapter No 1 : Acids, Bases and BuffersChetan Jain
This is chapter No 1 of Pharmaceutical Chemistry - I for Diploma in Pharmacy (D. Pharmacy)
Details notes for Diploma in Pharmacy (D.Pharmacy) Students.
In chemistry, acids and bases have been defined differently by three sets of theories. One is the Arrhenius definition, which revolves around the idea that acids are substances that ionize (break off) in an aqueous solution to produce hydrogen (H+) ions while bases produce hydroxide (OH-) ions in solution.
Chapter No 1 : Acids, Bases and BuffersChetan Jain
This is chapter No 1 of Pharmaceutical Chemistry - I for Diploma in Pharmacy (D. Pharmacy)
Details notes for Diploma in Pharmacy (D.Pharmacy) Students.
In chemistry, acids and bases have been defined differently by three sets of theories. One is the Arrhenius definition, which revolves around the idea that acids are substances that ionize (break off) in an aqueous solution to produce hydrogen (H+) ions while bases produce hydroxide (OH-) ions in solution.
19.1 acids, base and salts By Hamdy KarimHamdy Karim
Students will be able to compare between Arrhenius, Bronsted-Lowry, and Lewis theories to identify the acids and bases concept. They also will study the conjugated acids and bases in addition to the Amphoteric Substances as well!
Discusses the definitions, properties and calculations associated with acid / base chemistry
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
19.1 acids, base and salts By Hamdy KarimHamdy Karim
Students will be able to compare between Arrhenius, Bronsted-Lowry, and Lewis theories to identify the acids and bases concept. They also will study the conjugated acids and bases in addition to the Amphoteric Substances as well!
Discusses the definitions, properties and calculations associated with acid / base chemistry
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
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The three main categories of chemical compounds are acids, bases and salts. These compounds are always part of our daily lives in terms of what we eat and use. The human body contains some very common acids like dilute hydrochloric acid in the stomach, which aids in digestion of food. If the contents of our stomach become too acidic, it results to a burning sensation in the stomach. Acids and bases also regulate metabolic activities in the human body through equilibrium processes. Acids contain hydrogen ions (H+). A base is a substance, which on dissolving in water yields hydroxyl ions (OH-) as the only negative ions. Salts are formed by the combination of an acid and base.
Acids, Bases And Buffers Pharmaceutical Inorganic chemistry UNIT-II (Part-I)
Acids, Bases are defined by Four main theories,
1.Traditional theory / concept
2.Arrhenius theory
3.Bronsted and Lowry theory
4.Lewis theory
Importance of acids and bases in pharmacy
Buffers: Buffer action
Buffer capacity Buffers system
Types of Buffers : Generally buffers are of two types:
1. Acidic buffers
2. Basic buffers
There are some other buffer system:
3. Two salts acts as acid-base pair. Ex- Potassium hydrogen phosphate and potassium dihydrogen phosphate.
4. Amphoteric electrolyte. Ex- Solution of glycine.
5. Solution of strong acid and solution of strong base. Ex- Strong HCl with KCl Mechanism of Buffer action: Mechanism of Action of acidic buffers: Buffer equation-Henderson-Hasselbalch equation:
Standard Buffer Solutions Preparation of Buffer Solutions: Buffers in pharmaceutical systems or Application of buffer: Stability of buffers Buffered isotonic solution Types of Buffer Isotonic solution
1. Isotonic Solutions:
2. Hypertonic Solutions:
3. Hypotonic Solution:
Measurement of Tonicity: 1. Hemolytic method: 2. Cryoscopic method or depression of freezing point:
Methods of adjusting the tonicity:
Class I methods:
In this type, sodium chloride or other substances are added to the solution in sufficient quantity to make it isotonic. Then the preparation is brought to its final volume withan isotonic or a buffered isotonic diluting solution.
These methods are of two types:
Cryoscopic method
Sodium chloride equivalent method.
Class II methods:
In this type, water is added in sufficient quantity make the preparation isotonic. Then the preparation is brought to its volume with an isotonic or a buffered isotonic diluting solution.
These methods are of two types:
White-Vincent method
Sprowls method.
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Thesis Statement for students diagnonsed withADHD.ppt
Acidsandbases 120223093455-phpapp01(1)
1.
2. Look at some examples,Look at some examples,
and see if you can figureand see if you can figure
out what an acid is…out what an acid is…
HCl (Hydrochloric acid)HCl (Hydrochloric acid)
HNOHNO33 (Nitric acid)(Nitric acid)
HH22SOSO44 (Sulfuric acid)(Sulfuric acid)
HH33POPO44 (Phosphoric acid)(Phosphoric acid)
3. Acid/Base definitionsAcid/Base definitions
Definition #1: Arrhenius (traditional)Definition #1: Arrhenius (traditional)
Acid – has hydrogen in the formula, and produces HAcid – has hydrogen in the formula, and produces H++
ions in waterions in water
Base – has OH in the formula, and produces OHBase – has OH in the formula, and produces OH--
ionsions
in waterin water
4. Acids and bases inAcids and bases in
water:water:
Arrhenius Acid:Arrhenius Acid:
HCl (aq)HCl (aq) HH++
+ Cl+ Cl--
HCl is an acid because it has H in the formula,HCl is an acid because it has H in the formula,
and increases the amount of Hand increases the amount of H++
in water.in water.
Arrhenius Base:Arrhenius Base:
NaOH (aq)NaOH (aq) NaNa++
+ OH+ OH--
NaOH is a base because it has OH in the formulaNaOH is a base because it has OH in the formula
and increases the amount of OHand increases the amount of OH--
in water.in water.
5. The ArrheniusThe Arrhenius
definition had adefinition had a
problem…problem…
Some bases (like ammonia, NHSome bases (like ammonia, NH33) don’t) don’t
have OH in the formula.have OH in the formula.
6. Bronsted-Lowry definitions:Bronsted-Lowry definitions:
(new and improved(new and improved
definitions)definitions)
Acids are substances thatAcids are substances that give awaygive away hydrogenhydrogen
ions. (This definition is practically the same.)ions. (This definition is practically the same.)
Bases are substances thatBases are substances that acceptaccept hydrogen ions.hydrogen ions.
7. Bronsted-LowryBronsted-Lowry
definition:definition:
Acids are substances that give away hydrogenAcids are substances that give away hydrogen
ions.ions.
Example: HCl gives away hydrogen to water:Example: HCl gives away hydrogen to water:
HCl (aq) + HHCl (aq) + H22OO HH33O+ (aq) + Cl- (aq)O+ (aq) + Cl- (aq)
Draw the hydrogen ion. What does it consist of?Draw the hydrogen ion. What does it consist of?
8. A hydrogen ion isA hydrogen ion is
simply a proton.simply a proton.
Acids are also called “proton donors.”Acids are also called “proton donors.”
9. Bronsted-LowryBronsted-Lowry
definition:definition:
A base is a hydrogen ion acceptor.A base is a hydrogen ion acceptor.
Another way of saying the same thing:Another way of saying the same thing:
A base is a proton acceptor.A base is a proton acceptor.
10. An acid is a proton donor
A base is a proton acceptor
acidbase
11. Practice question:Practice question:
In the reactionIn the reaction
HBr(HBr(aqaq) + NH) + NH33((aqaq)) NHNH44
++
((aqaq) + Br) + Br––
((aqaq))
Identify the acid and the base.Identify the acid and the base.
12. Practice questionPractice question
In the reactionIn the reaction
HSOHSO44
––
+ H+ H22OO HH33OO++
+ SO+ SO44
2-2-
Identify the acid and the base.Identify the acid and the base.
13. Practice question:Practice question:
In the equationIn the equation
HCl(HCl(gg) + H) + H22O(O(ll)) HH33OO++
((aqaq) + Cl) + Cl––
((aqaq))
which formula is a Brønsted-Lowry acid?which formula is a Brønsted-Lowry acid?
14. Tell-tale signs of anTell-tale signs of an
acid:acid:
sour tastesour taste
(orange juice and lemonade contain(orange juice and lemonade contain
citric acid)citric acid)
turns litmus paper redturns litmus paper red
(by reacting with a chemical in(by reacting with a chemical in
the litmus paper)the litmus paper)
reacts with metals to producereacts with metals to produce
hydrogen gashydrogen gas
15. Chemists write the formulas forChemists write the formulas for
acids with the H at the front, soacids with the H at the front, so
they’re easy to identify as acids:they’re easy to identify as acids:
HCl (Hydrochloric acid)HCl (Hydrochloric acid)
HNOHNO33 (Nitric acid)(Nitric acid)
HH22SOSO44 (Sulfuric acid)(Sulfuric acid)
HH33POPO44 (Phosphoric acid)(Phosphoric acid)
16. Tell-tale signs of aTell-tale signs of a
base:base:
bitter tastebitter taste
slippery feelslippery feel
turns litmus paper blueturns litmus paper blue
(Conveniently, base, bitter, and blue all(Conveniently, base, bitter, and blue all
start with B!)start with B!)
17. Some substances,Some substances,
like water act likelike water act like
an acid sometimesan acid sometimes
and act like a baseand act like a base
other times.other times.
Substances that can act as anSubstances that can act as an
acid or a base are calledacid or a base are called
amphoteric.amphoteric.
18. Neutralization reactions:Neutralization reactions:
If you combine an acidIf you combine an acid
with a base…with a base…
Predict the products:Predict the products:
HCl + NaOHHCl + NaOH ??
Hint: It’s a special kind of double replacementHint: It’s a special kind of double replacement
reaction!reaction!
19. If you combine an acidIf you combine an acid
with a base…with a base…
HCl + NaOHHCl + NaOH HH22O + NaClO + NaCl
This is called aThis is called a neutralization reactionneutralization reaction
because the acid and base neutralizebecause the acid and base neutralize
each other.each other.
20. If you combine an acidIf you combine an acid
with a base…with a base…
HCl + NaOHHCl + NaOH HH22O + NaClO + NaCl
The products of any neutralization reactionThe products of any neutralization reaction
are water and a salt.are water and a salt.
21. Acid/Base reactions:
Produce water and a salt (and sometimes carbon dioxide).
Hint: concentrate on the water first. Remember, water
has the formula HOH.
Complete and balance the following:
HCl + KOH →
HCl + Ca(OH)2 →
HOH + KCl
2
Require equal numbers
2HOH + CaCl2
23. Everyday application:Everyday application:
The stomach secretes acids to help digestThe stomach secretes acids to help digest
foods. These acids, which includefoods. These acids, which include
hydrochloric acid, have a molarity ofhydrochloric acid, have a molarity of
about 0.1M.about 0.1M.
Antacids, like Tums, Maalox, Mylanta andAntacids, like Tums, Maalox, Mylanta and
Alka-seltzer are simple bases thatAlka-seltzer are simple bases that
neutralize stomach acids.neutralize stomach acids.
24. Acids and Bases:Acids and Bases:
StrengthStrength
What makes an acid a strong acid?What makes an acid a strong acid?
It ionizes completely in water!It ionizes completely in water!
These are strong acids (in order of increasingThese are strong acids (in order of increasing
strength):strength):
1.1. HNOHNO33 (nitric acid)(nitric acid)
2.2. HCl (hydrochloric acid)HCl (hydrochloric acid)
3.3. HBr (hydrobromic acid)HBr (hydrobromic acid)
4.4. HI (hydroiodic acid)HI (hydroiodic acid)
5.5. HH22SOSO44 (sulfuric acid)(sulfuric acid)
6.6. HClOHClO44 (perchloric acid) (the strongest)(perchloric acid) (the strongest)
25. Strong acids:Strong acids:
HCl + HHCl + H22OO HH33OO++
+ Cl-+ Cl-
Remember, strong acids ionize completely in
water. The reaction goes all the way to the
right. A single arrow is used. There are
virtually no HCl molecules left intact.
26. One more reminder:One more reminder:
“Weak” does not mean the same“Weak” does not mean the same
thing as “diluted.”thing as “diluted.”
HCl, for example is always aHCl, for example is always a
strong acid. If you add 1000strong acid. If you add 1000
liters of water to it, it will beliters of water to it, it will be
diluted, but still strong becausediluted, but still strong because
what little there is will bewhat little there is will be
completely dissociated.completely dissociated.
27. Electrolytes:Electrolytes:
Acids and bases are both examples ofAcids and bases are both examples of
electrolytes.electrolytes.
Electrolytes are compounds that form ionsElectrolytes are compounds that form ions
when dissolved in water.when dissolved in water.
They’re called electrolytes because theyThey’re called electrolytes because they
can conduct electricity through water.can conduct electricity through water.
28. More on electrolytes:More on electrolytes:
If two wires connected to a light bulb and to a powerIf two wires connected to a light bulb and to a power
source are placed in a beaker of water, the lightsource are placed in a beaker of water, the light
bulb will not glow. If an electrolyte, such asbulb will not glow. If an electrolyte, such as
sodium chloride, is dissolved in the water, the lightsodium chloride, is dissolved in the water, the light
bulb will glow because the solution can nowbulb will glow because the solution can now
conduct electricity. The amount of electric currentconduct electricity. The amount of electric current
that can be carried by an electrolyte solution isthat can be carried by an electrolyte solution is
proportional to the number of ions dissolved.proportional to the number of ions dissolved.
Thus, the bulb will glow more brightly if theThus, the bulb will glow more brightly if the
amount of sodium chloride in the solution isamount of sodium chloride in the solution is
increased.increased.
30. Which of these couldWhich of these could
be used to determinebe used to determine
whether a substance iswhether a substance is
a base?a base?
A ThermometerA Thermometer
B Litmus paperB Litmus paper
C BalanceC Balance
D Bunsen burnerD Bunsen burner
31. An element common toAn element common to
all acids is –all acids is –
a. chlorinea. chlorine
b. hydrogenb. hydrogen
c. oxygenc. oxygen
d. sodiumd. sodium
33. TheThe pH scalepH scale is a wayis a way
of expressing theof expressing the
concentration of acids.concentration of acids.
Under 7 = acidUnder 7 = acid
7 = neutral7 = neutral
Over 7 = baseOver 7 = base
34. pH is the negative logpH is the negative log
of the Hof the H++
concentration.concentration.
35. pH is the negative logpH is the negative log
of the Hof the H++
concentration.concentration.
What????
36. It’s easier than itIt’s easier than it
sounds!sounds!
If HIf H++
is….is….
1 x 101 x 10-3-3
pH = 3pH = 3
1 x 101 x 10-7-7
pH = 7pH = 7
1 x 101 x 10-12-12
pH = 12pH = 12