Acids, Bases, And Salts (1)
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Transcript of Acids, Bases, And Salts (1)
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acids bases salts
E X P E R I ME N T 7
G R OU P S 8 & 9
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parts
I. Electrolytes and Common
Household Items
I. Conductivity Test
II. Preparation of 1 M NaOH using NaOH
pellets
III. Preparation of 0.1 M from 1 M NaOH
IV. Titration of an Acid and a Base
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concepts
o Electrolyte
oAcids
o Bases
o Neutralization
o Salts
o pH
electrolytes and common
household items
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concepts electrolyte
a substance that, when dissolved in water, results in a
solution that can conduct
electricity
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concepts acids
GENERAL PROPERTIES
sour taste color changes in plant dyes react with certain metals React with carbonates and bicarbonates to produce CO2 gas
Aqueous acid solutions conduct electricity
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concepts bases
GENERAL PROPERTIES
bitter taste slippery color changes in plant dyes aqueous base solutions conduct
electricity
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concepts acids vs. bases
ACIDS BASES
ARRHENIUS
CONCEPT
Ionize in water
solution to produce
H+(aq) or H3O+
Ionize in water
solution to produce
OH-(aq)
BRNSTED-LOWRY
CONCEPT
Proton donors Proton acceptors
LEWIS
CONCEPT
Electron-pair
acceptors Electron-pair donors
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concepts neutralization
a reaction between an acid and a base.
aqueous acid-base reactions produce water and a salt
acid + base salt + water
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concepts salts
ionic compounds made up of a cation other than H+
and an anion other than OH-
or O2-
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concepts pH
measure of acidity the negative logarithm of the hydrogen ion
concentration (in mol/L):
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concepts pH
INDICATORS
litmus paper phenolphthalein congo red pH paper
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procedure electrolytes and common
household items
NaOH NH4Cl HCl HC2H3O2 NaCl C12H22O11 C2H5OH H2O
Test with litmus paper, phenolphthalein, and congo red Classify whether acidic, basic, or neutral Test pH using pH paper
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procedure electrolytes and common
household items
shampoo conditioner feminine
wash
liquid
sosa
liquid
soap
fruit
juice
softdrink
Test with litmus paper, phenolphthalein, and congo red Classify whether acidic, basic, or neutral Test pH using pH paper
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results
Reagents
0.1 M
Solutions
Classification pH Classification
of Acid/Base
NaOH Base 12 Strong Base
NH4Cl Base 8 Weak Base
HCl Acid 2 Strong Acid
HC2H3O2 Acid 2 Strong Acid
NaCl Neutral 7 -
H2O Neutral 7 -
C6H12O11 Neutral 7 -
C2H5OH Base 12 Strong Base
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results Solution
Litmus
Paper Phenolphthalein Congo Red Classification
Shampoo R-R
B-R Colorless Red Base
Conditioner B-B-
R-R Colorless Red Acid
Feminine
Wash
B-B
R-R Colorless Colorless Acid
Liquid
Sosa
R-B
B-B Violet Red Base
Liquid
Soap
R-B
B-B Colorless Red Base
Softdrink B-R
R-R Cloudy Dark violet Acid
Fruit
Juice
R-R
B-R Cloudy Violet Acid
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concepts
o strong electrolytes
o weak electrolytes
o non-electrolytes
conductivity test
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concepts
dissociate completely into
ions and create a large current
strong electrolytes
dissociate into ions very little, and most of
their molecules remain intact.
weak electrolytes
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procedure conductivity test
Test conductivity of the solutions in 1-a
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results
Reagents
0.1 M Solutions Conductivity
Classification (based
on conductivity)
NaOH Good Strong Electrolyte
NH4Cl Good Strong Electrolyte
HCl Good Strong Electrolyte
HC2H3O2 Weak Weak Electrolyte
NaCl Good Strong Electrolyte
H2O - Non-electrolyte
C12H22O11 - Non-electrolyte
C2H5OH - Non-electrolyte
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concepts
o Concentration of solution
o Molarity
preparation of 1 M
NaOH using NaOH pellets
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concepts concentration
a measure of the quantity of solute dissolved in a given
quantity of solution
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concepts molarity
molar concentration, which is the number of
moles of solute per liter of
solution
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procedure
Calculate the weight of NaOH pellets needed to prepare 50.0 mL of 1 M NaOH
Weigh pellets in a watch glass and dissolve in 50 mL water
Transfer in 100-mL volumetric flask and dilute to the mark with water
preparation of 1 M
NaOH using NaOH pellets
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results
1 mol NaOH x 0.1 L x 40 g NaOH = 4g NaOH in
1 L 1 mol NaOH the beaker
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concepts
o dilution
preparation of 0.1 M
NaOH from 1 M NaOH
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concepts dilution
a procedure for preparing a less concentrated solution from
a more concentrated solution.
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procedure
Determine volume of NaOH from available concentration needed to
prepare 100 mL of 0.1 M NaOH
Dilute the measured volume to 100.00 mL with water in a
volumetric flask
M1V1=M1V2
preparation of 0.1 M
NaOH from 1 M NaOH
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results
M1V1=M1V2
1M (V1) = 0.1 M (250 mL)
V1 = 25 mL
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concepts
o titration
o equivalence point
o indicator
o end point
titration of an acid
with a base
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concepts titration
a method of determining the concentration of a solution by
monitoring its reaction with a
solution of known concentration.
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concepts equivalence
the point at which the acid has completely reacted with or been
neutralized by the base
point
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concepts indicators
are substances that have distinctly different colors in acidic and basic
media.
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concepts end point
the pH at which the indicator changes color.
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procedure titration of an acid
with a base
Wash base buret with soap and water then rise with 0.1 M NaOH.
Fill buret with 0.1 M NaOH and
remove airspace
Pipet a 10-mL aliquot of the unknown acid in an erlenmeyer flask, add 50 mL water then add
2-3 drops phenolphtalein. Titrate until pink
coloration. Calculate molarity of unknown acid
solution
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results
Trial 1 Trial 2 Trial 3
Volume of
0.1 M NaOH 2.8 mL 2.9 mL 3 mL
Volume of
unknown
acid solution 2mL 2mL 2mL
Molarity of
unknown
acid solution 0.14 M 0.145 M 0.15
Average
molarity of
unknown acid
solution
0.145 M
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5
results Trial 1:
MacidVacid=MbaseVbase Macid(2 mL) = (0.1 M)(2.8 mL)
Macid = 0.14 M Trial 2:
MacidVacid=MbaseVbase Macid(2 mL) = (0.1 M)(2.9 mL)
Macid = 0.145 M
Trial 3:
MacidVacid=MbaseVbase Macid(2 mL) = (0.1 M)(3 mL)
Macid = 0.15 M
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guide
1. From your results, what relationship can
you draw between the acidity/basicity of a
substance and its electrolyte property?
There is a direct relationship between the acidity/basicity
of a substance and its ability to conduct electricity. Strong
acids/bases have stronger conductive ability because of
their almost complete dissociation in an aqueous
substance. Although other properties must be considered
if an acid/base is also a salt, whether weak or strong, when
dissolved in water, it is also a good conductor of electricity.
questions
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guide
2. Why are electrolytes conductors of
electricity?
Electrolytes dissociate in aqueous solutions, thus they are ionized. Positively charged ions move toward the negative
electrode and negatively charged ions move to the positive
electrode. This resembles the movement of electrons along a metal
wire which explains the conductive property of electrolytes.
questions
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conclusion
Electrolytes are compounds that dissociate into
its constituent ions. Strong acids/bases completely
dissociate. Thus make a good conductor because
there is abundance in ions that would complete an
electrical circuit. Weak acids and bases, on the other
hand, do not completely dissociate. This partial
dissociation causes their low conductivity because
there is a low availability of ions that would complete
the circuit. Non-electrolytes do not produce ions at
all because they exist as uncharged molecules.
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recommendation
It is recommended that one be careful and
observant in using indicators when getting the pH of
the solution in order to obtain accurate results. For
the preparation of the titrant, one must accurately
measure the weight of NaOH pellets and the volume
of water to use. It must also be completely dissolved
in water before being diluted in a 100mL volumetric
flask. During the titration, one must be careful in
transferring of the titrant to the unknown solution in
order to avoid over-titration.
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references
Chang, R. (2010). Chemistry (10th ed.). New
York, NY: McGraw-Hill.
Silberberg, M.S. (2009). Chemistry: the
molecular nature of matter and change (5th
ed.). New York, NY: McGraw-Hill.