Acid Base Indicators Experiment #6. What are acids and bases? There are many different definitions...
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Transcript of Acid Base Indicators Experiment #6. What are acids and bases? There are many different definitions...
![Page 1: Acid Base Indicators Experiment #6. What are acids and bases? There are many different definitions for classifying a substance as an acid or a base. Definitions.](https://reader036.fdocuments.in/reader036/viewer/2022062322/56649ea95503460f94bad001/html5/thumbnails/1.jpg)
Acid Base Indicators
Experiment #6
![Page 2: Acid Base Indicators Experiment #6. What are acids and bases? There are many different definitions for classifying a substance as an acid or a base. Definitions.](https://reader036.fdocuments.in/reader036/viewer/2022062322/56649ea95503460f94bad001/html5/thumbnails/2.jpg)
What are acids and bases?There are many different definitions for classifying a substance as an acid or a base.
Definitions are based on different theories
Lewis’s theory of acids and bases
Lowry-Bronsted theory of acids and bases
Arrhenius theory of acids and bases
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Arrhenius theory of acids and bases
Proposed in 1884 by Svante Arrhenius
An acid is a substance that contains hydrogen and produces H+ in aqueous Solution. A base is a solution that contains the OH group and produces Hydroxide ions OH-, in aqueous solution
Neutralization is defined as the combination of H+ ions with OH- ions to form H2O molecules.
H+ (aq) + OH-(aq) H2O(l)
Very Limited in Scope!!
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Lowry-Bronsted theory
Proposed in 1923 by N. Bronsted and T.M.Lowry
An acid is defined as a proton donor, H+, and a base is Defined as a proton acceptor
The complete ionization of hydrogen chloride, HCl in wateris an acid-base reaction
Step 2: H+ (aq) + H2O(l) H3O+
An acid-base reaction is the transfer of a proton from an acid to a base
Overall: HCl(aq) + H2O(l) H3O+(aq) + Cl-(aq) (LB)
Step 1: HCl(aq) H+(aq) + Cl-(aq) (Arrehnius)
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Overall: HCl(aq) + H2O(l) H3O+(aq) + Cl-(aq) (LB)
acid conjugateacidbase conjugate
base
Overall: NH3(aq) + H2O(l) NH4+(aq) + OH-(aq) (LB)
base conjugateacidacid conjugate
base
Whether water can act as an acid or base depends on the other species present
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H2O (l) + H2O(l) H3O+ (aq) + OH-(aq)
Autoionization of water
Simplified notation
H2O(l) H+ (aq) + OH-(aq)
Water is said to be amphiprotic
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Strength of acidsAcids and bases are classified as strong or weakdepending on the extent to which they can ionize.
Higher ionization ≡ Strong
Strong acid does not necessarily mean that it is the most corrosive acid. HF is a weak acid but it is one of the most corrosive acids.
Strength of some acids:HClO4 > HI > HBr > HCl > HNO3
H2SO4 > HNO3
Strong acids and strong bases are completely ionized
Weak acids and weak bases are partially ionized
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Lewis theory
An acid is any species that can accept a share in an electron pair. A base is any species that can make available or donate a share in an electron pair.
A more broader definition. There is no need for the molecule to have hydrogens.
Proposed in 1923 by G. N. Lewis
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What happens when salts are dissolved in water?
HCl(aq) + NaOH(aq) NaCl(aq) + H2O(aq)
Acid Base Salt Water
NaCl(s) + H2O NaOH(aq) + HCl(aq)
Salt Water Base Acid
Depending on the strength of the acid and base that are formed in solution, the medium will be either acidic or basic
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How do I know if the resulting solution is acidic or basic?
Measure pH of the solution
What is pH?
It is the measure of hydrogen ions in solution
OHLogpH 3
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What is pH?
pH=1.0
pH=14.0
pH=7.0
Acidic
Neutral
Basic
OHLogpH 3
HLogpH
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What are some of the ways to measure pH?
1. Using an acid-base indicator
2. Using pH paper
3. Using pH meter
4. ……………..
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What are acid-base indicators? How do they work?
An organic dye, whose color depends on the concentration of H3O+ or pH
HIn(aq) + H2O(l) H3O+(aq) + In-(aq)
acid conjugateacidbase conjugate
baseWhen the indicator is added to the solution of interest, depending on the pH of the solution, the indicator stays in either its acid form or its conjugate form.
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Indicator "Acidic" Color "Basic" color(MO)methyl orange Red below pH 4.0 Yellow above pH 4.4(BG)bromcresol green Yellow below pH 4.5 Blue above pH 4.8(BB)bromthymol blue Yellow below pH 6.9 Blue above pH 7.3(TB)thymol blue Yellow below pH 8.0 Blue above pH 8.4(P)Phenolphthalein Colorless below pH 9.3 Pink above pH 9.7(AY)alizarin yellow Yellow below pH 10.8 Red above pH 11.2
If we are to pick a suitable indicator for following the pH change in the reaction,We have to pick one that is suitable over the pH range of the reaction.
Indicators cannot give a particular numerical value for pH. They can only give a range for the pH of the solution.
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Ionization of acids
All acids undergo ionization. Strong acids ionize more than the weak ones. Strong acids are almost100% ionized. Since the weak acids are partially ionized, the measure of the extent of ionization is given by an expression called acid ionizationconstant, Ka.
In our experiment today, we would like to measurethe Ka for a weak monoprotic acid.
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What is a monoprotic acid?
Usually acids have one or more hydrogen atoms (H)which they end up donating as protons (H+).
# of H atoms Name Example
1 monoprotic acid (HA) HCl – hydrochloric acid CH3COOH - acetic acid
2 diprotic acid (H2A) H2SO4 – sulfuric acid
3 triprotic acid (H3A) H3PO4 – Phosphoric acid
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Ionization constant of an acidFor a monoprotic weak acid (HA) dissolved in water,
HA(aq) + H2O(l) H3O+(aq) + A-(aq)
acid conjugateacidbase conjugate
base
eqbeqb
eqbeqb
eq OHHA
AOHK
2
3
cOHthatassumewillweOHOHSinceeqbinitialeqb
222 ,
cHA
AOHK
eqb
eqbeqb
eq
3
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Ionization constant of an acid
cHA
AOHK
eqb
eqbeqb
eq
3
eqb
eqbeqb
eqa HA
AOHcKK
3
eqb
eqbeqb
a HA
AOHK
3
Ionization constant of the acid
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eqb
eqbeqb
a HA
AOHK
3
Ionization constant of an acid
Taking log of the equation on both sides,
eqb
eqbeqb
a HA
AOHLogLogK
3
][][
3 HAA
LogOHLogLogKa
cb
LogaLogaswrittenbecancab
LogSince )()(
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Ionization constant of an acid
][][
3 HAA
LogOHLogLogKa
Multiplying both sides of the equation by -1
][][
3 HAA
LogOHLogLogKa
pHOHLogandpKLogKbut aa 3,
][][
HAA
LogpHpKa
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Ionization constant of an acid
][][
HAA
LogpHpKa
][][
HAA
LogpKpH a
Henderson-Hasselbach equation
In the above equation, if we can make the [A-] = [HA]
][][
HAHA
LogpKpH a
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Ionization constant of an acid
][][
HAHA
LogpKpH a
)1(LogpKpH a
0 apKpH
apKpH
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250mL
Vinitial
0.2 MNaOH
250mL
Vfinal
100mL
1.0 g of HAIn 100mL ofwater
50 mL of HA+ 2 drops phenolphthalein
Vfinal- Vinitial =Vused
Add Vused amount ofwater to the solution in the volumetric flask
Mix the solution involumetric flask to theSolution in the erlenmeyerflask
Measure the pH of thefinal solution with indicators and pH paper