This document defines different types of acids and bases and their properties. It discusses Bronsted-Lowry acids and bases, which are defined by their ability to donate or accept protons. Arrhenius acids and bases are defined by their ability to produce H+ or OH- ions when dissolved in water. Lewis acids are electron acceptors while Lewis bases are electron donors. Strong acids fully dissociate in water producing H+ ions, while weak acids only partially dissociate. Concentrated acids have more moles of solute per liter than diluted acids. The pH scale is used to measure acidity, with lower pH indicating more acidic solutions.
This is a summary of the topic "Carboxylic Acids" in the GCE O levels subject: Chemistry. Students taking pure chemistry will find this useful. These slides are prepared according to the learning outcomes required by the examinations board.
This is a summary of the topic "Carboxylic Acids" in the GCE O levels subject: Chemistry. Students taking pure chemistry will find this useful. These slides are prepared according to the learning outcomes required by the examinations board.
Acids are divided into two categories based on the ease with which they can donate protons to the solvent: i) strong acids and ii) weak acids
Strong acids are acids that completely dissociate in water. The reaction of an acid with its solvent (typically H2O) is called an acid dissociation reaction.
Weak acids are acids that dissociate partially in water. The extent of dissociation is given by the equilibrium constant.
Note:
A measure of the relative strength of an acid is: i) the equilibrium constant ka of the dissociation reaction of the acid in water (depends on temperature) ii) the degree of dissociation α of the acid in water (depends on the concentration of the acid an on temperature).
THIS PRESENTATION IS FOR THE STUDENTS STUDYING IN SENIOR CLASSES .IT WILL HELP THE CHILD TO RECALL THE CONTENT IN SHORT TIME IT WILL HELP TO BUILD THE STRONG AND CLEAR CONCEPT KNOWLEDGE.
Acids are divided into two categories based on the ease with which they can donate protons to the solvent: i) strong acids and ii) weak acids
Strong acids are acids that completely dissociate in water. The reaction of an acid with its solvent (typically H2O) is called an acid dissociation reaction.
Weak acids are acids that dissociate partially in water. The extent of dissociation is given by the equilibrium constant.
Note:
A measure of the relative strength of an acid is: i) the equilibrium constant ka of the dissociation reaction of the acid in water (depends on temperature) ii) the degree of dissociation α of the acid in water (depends on the concentration of the acid an on temperature).
THIS PRESENTATION IS FOR THE STUDENTS STUDYING IN SENIOR CLASSES .IT WILL HELP THE CHILD TO RECALL THE CONTENT IN SHORT TIME IT WILL HELP TO BUILD THE STRONG AND CLEAR CONCEPT KNOWLEDGE.
Macroeconomics- Movie Location
This will be used as part of your Personal Professional Portfolio once graded.
Objective:
Prepare a presentation or a paper using research, basic comparative analysis, data organization and application of economic information. You will make an informed assessment of an economic climate outside of the United States to accomplish an entertainment industry objective.
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Knowledge and skills frameworks, generally called competency frameworks, for ELT teachers, trainers and managers have existed for a few years now. However, until I created one for my MA dissertation, there wasn’t one drawing together what we need to know and do to be able to effectively produce language learning materials.
This webinar will introduce you to my framework, highlighting the key competencies I identified from my research. It will also show how anybody involved in language teaching (any language, not just English!), teacher training, managing schools or developing language learning materials can benefit from using the framework.
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The US House of Representatives is deeply concerned by ongoing and pervasive acts of antisemitic
harassment and intimidation at the Massachusetts Institute of Technology (MIT). Failing to act decisively to ensure a safe learning environment for all students would be a grave dereliction of your responsibilities as President of MIT and Chair of the MIT Corporation.
This Congress will not stand idly by and allow an environment hostile to Jewish students to persist. The House believes that your institution is in violation of Title VI of the Civil Rights Act, and the inability or
unwillingness to rectify this violation through action requires accountability.
Postsecondary education is a unique opportunity for students to learn and have their ideas and beliefs challenged. However, universities receiving hundreds of millions of federal funds annually have denied
students that opportunity and have been hijacked to become venues for the promotion of terrorism, antisemitic harassment and intimidation, unlawful encampments, and in some cases, assaults and riots.
The House of Representatives will not countenance the use of federal funds to indoctrinate students into hateful, antisemitic, anti-American supporters of terrorism. Investigations into campus antisemitism by the Committee on Education and the Workforce and the Committee on Ways and Means have been expanded into a Congress-wide probe across all relevant jurisdictions to address this national crisis. The undersigned Committees will conduct oversight into the use of federal funds at MIT and its learning environment under authorities granted to each Committee.
• The Committee on Education and the Workforce has been investigating your institution since December 7, 2023. The Committee has broad jurisdiction over postsecondary education, including its compliance with Title VI of the Civil Rights Act, campus safety concerns over disruptions to the learning environment, and the awarding of federal student aid under the Higher Education Act.
• The Committee on Oversight and Accountability is investigating the sources of funding and other support flowing to groups espousing pro-Hamas propaganda and engaged in antisemitic harassment and intimidation of students. The Committee on Oversight and Accountability is the principal oversight committee of the US House of Representatives and has broad authority to investigate “any matter” at “any time” under House Rule X.
• The Committee on Ways and Means has been investigating several universities since November 15, 2023, when the Committee held a hearing entitled From Ivory Towers to Dark Corners: Investigating the Nexus Between Antisemitism, Tax-Exempt Universities, and Terror Financing. The Committee followed the hearing with letters to those institutions on January 10, 202
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IB Chemistry on Acid Base, pH Scale and Ionic Product Water, Kw
1. Brønsted-Lowry Acid - substance that donate proton/proton donor
Bronsted-Lowry Base – substance that accept proton/proton acceptor
One species donate proton – one species accept proton
Arrhenius acid - substance dissociate in water produce H+ ion.
Arrhenius base – substance dissociate in water produce OH-ion.
All Arrhenius acid are Bronsted Lowry acid and water must be present
HCI → H+ + CI-
HCI + H2O ↔ H3O+ + CI-
NaOH → Na+ + OH-
NH3 + H2O ↔ NH4
+
+ OH-
CO3
2- + H2O ↔ HCO3
- + OH-
Water/aqueous medium
Water/aqueous medium
Other solvent medium possible
Definition of Acid and Bases
Arrhenius acid Arrhenius baseH+ OH-
2
1
gain H+
Acid + Base ↔ Conjugate Base + Conjugate Acid
lose H+
HCI (acid) - CI- (conjugate base)
lose H+
H2O (base) - H3O+ (conjugate acid)
HCI + H2O ↔ CI- + H3O+
gain H+
Lewis Acid - substance that accept electron/electronacceptor, empty orbital/electrondeficient
Lewis Base – substance that donate electron/electrondonor, lone pair electron
Lewis Base - donate electron pair forming dative/coordinatebond with Lewis acid
3
HCI + H2O → CI- + H3O+
H2O donate e-
HCI accept e-
Lewis acid Lewis base
Conjugate acid
base pair differ
by one proton
2. Physicalproperties of Acid
• Substancedissolvesin water produce
hydrogen ion/H+ or hydronium /H3O+
• HCI → H+ + CI-
• Conduct electricity – free movingions
• Sour, pH < 7
• Turn blue litmus red
• Turn phenolphthaleincolourless
• Turns methyl orange to red
Properties of Acids and Bases
Acid+ Metal (above H) → Salt + H2 gas
2HCI + Mg → MgCI2 + H2
Acid + Base → Salt + Water + product.
Bases are - Metal Hydroxide,Metal Oxide, Metal Carbonates
Acid + Metal Hydroxide → Salt + Water
Acid + Metal Oxide → Salt + Water
Acid + Metal Carbonate → Salt + Water + Carbon Dioxide
Acid + Ammoniaaq and Amines → Salt + water
HCI + NH4OH → NH4CI + H2O
HCI + CH3NH2 → CH3NH3 + CI-
Chemical properties of Acids / Bases
Physical properties of Acid
Physical properties of Bases
• Substance dissolvesin water produce
hydroxide/OH- ion
• NaOH → Na+ + OH-
• Conduct electricity– free moving ions
• Bitter, pH > 7
• Turns red litmus blue
• Turns phenolphthalein pink
• Turns methyl orange to yellow
Physical properties of Base
Physical Properties Chemical Properties
Physical Properties
Chemical Properties
Hydronium/Hydroxonium/Oxonium
3. Physicalproperties of Acid
• Electrolytes,produce H3O+,hydronium ion
• Conduct electricity
• Sour, pH < 7
• Turn litmus red
• Turn phenolphthaleincolourless
• Turn methyl orange to red
Physicalproperties of Base
• Bitter,pH > 7
• Turn litmus blue
• Turn phenolphthaleinpink
• Turn methyl orange to yellow
Physical/ChemicalProperties of Acids and Bases
Chemical properties of Acid / BasePhysical properties of Acid/Base
Bases
Acid + Metal Hydroxide (Alkali) → Salt + Water
LiOH + HCI → LiCI + H2O
NaOH + HNO3 → NaNO3 + H2O
KOH + H2SO4 → K2SO4 + H2O
Acid + Metal Hydroxide (Insoluble) → Salt + Water
Ca(OH)2 + 2HCI → CaCI2 + 2H2O
Fe(OH)2 + 2HNO3 → Fe(NO3)2 + 2H2O
Mg(OH)2 + H2SO4 → MgSO4 + 2H2O
Acid + Metal Oxide → Salt + Water
CaO + 2HCI → CaCI2 + H2O
CuO + 2HCI → CuCI2 + H2O
Acid + Alkali
Acids + Metal Oxide
Acid + Metal Hydroxide
Acid + Metal Carbonate
Acid + Metal Carbonate → Salt, Water + CO2
CaCO3 + 2HCI → CaCI2 + H2O + CO2
CuCO3 + 2HCI → CuCI2 + H2O + CO2
Acid+ Metal (above H) → Salt + H2 gas
2HCI + Mg → MgCI2 + H2
Acid + Base → Salt + Water + product.
Bases are - Metal Hydroxide,Metal Oxide, Metal Carbonate
Acid + Metal Hydroxide → Salt + Water
Acid + Metal Oxide → Salt + Water
Acid + Metal Carbonate → Salt + Water + Carbon Dioxide
Acid + Ammoniaaq and Amines → Salt + water
HCI + NH4OH → NH4CI + H2O
HCI + CH3NH2 → CH3NH3 + CI-
4. CH3COOH ↔ H+ + CH3COO-
(1 mole) (0.01 mole)
Strong Acid / Base Weak Acid / Base
Strong acid – ionise/dissociate completelyproducing H+
ion
Strong base – ionise/dissociate completelyproducing OH-
ion
All are in ions state, NO molecule left
Strong electrolytewith high conductivity ↑
Weak acid – ionise/dissociate partially producing H+
ion
Weak base – ionise/dissociate partiallyproducing OH-
ion
Most in undissociated molecule form
Poor electrolytewith low conductivity↓
HCI → H+ + CI-
HBr → H+ + Br−
Monoprotic acid - 1 mole H+
ion
Diprotic acid - 2 mole H+
ion
H2SO4 → 2H+
+ SO4
2-
(1 mole) (2 mole)
Strong Acid - HI, HBr, HCI, HNO3, H2SO4, HCIO3, HCIO4
Strong Base - LiOH, KOH, NaOH, CsOH, Ca(OH)2, Ba(OH)2
Weak Acid - CH3COOH, HF, HCN, H2CO3, H3BO3, HNO2, H3PO4
Weak Base - NH3, C2H5NH2 , CH3NH2, (CH3)2NH, C3H5O2NH2
Weak acid dissociate partially produce few H+ ion
NH3 + H2O ↔ NH4
+ + OH-
C2H5NH2 + H2O ↔ C2H5NH3
+
+ OH-
CO3
2-
+ H2O ↔ HCO3
-
+ OH-
Weak base dissociate partially produce few OH- ion
Vs
Example of Strong Acid/Base Example of Weak Acid/Base
Ba(OH)2 → Ba2+ + 2OH−
(1 mole) (2 mole)
(1 mole) (1 mole)
Dissociatecompletely
No moleculesleft
All ion form Few ions
form
Dissociatepartially
Molecules left
Monoprotic base - Accept 1 mole H+ ions by 1mole OH-
Na(OH) → Na+ + OH−
(1 mole) (1 mole)
All ion form
Dissociatecompletely
No moleculesleft
Few ions
form
Dissociatepartially
Molecules left
H3PO4 ↔ H+ + H2PO4
-
H2PO4
- ↔ H+ + HPO4
2-
HPO4
2-
↔ H+ + PO4
3-
H3PO4 ↔ 3H+
+ PO4
3-
Diprotic base - Accept 2 mole H+ ions by 2 mole OH-
Weak triprotic acid dissociate partially produce few H+ ion
One way reversible
reversible
One way
One way
reversible
5. CH3COOH ↔ H+ + CH3COO-
(1 mole) (0.01 mole)
Strong Acid / Base Weak Acid / Base
Strong acid – ionise/dissociate completelyproducing H+
ion
Strong base – ionise/dissociate completelyproducing OH-
ion
All are in ionic ions state
Strong electrolytewith high conductivity ↑
Weak acid – ionise/dissociate partiallyproducing H+
ion
Weak base – ionise/dissociate partiallyproducing OH-
ion
Most in undissociated molecule form
Poor electrolytewith low conductivity↓
HCI → H+ + CI-
HBr → H+ + Br−
Monoprotic acid - produce 1 mole H+
ions
Diprotic acid - 2 mole H+
H2SO4 → 2H+
+ SO4
2-
Strong acid - HI, HBr, HCI, HNO3, H2SO4, HCIO3, HCIO4
Strong base - LiOH, KOH, NaOH, CsOH, Ca(OH)2, Ba(OH)2
(1 mole) (2 mole)
Weak Acid - CH3COOH, HF, HCN, H2CO3, H3BO3, H3PO4
Weak Base - NH3, C2H5NH2 , (CH3)2NH, C3H5O2NH2
Weak acid dissociate partially produce few H+
ion
NH3 + H2O ↔ NH4
+ + OH-
C2H5NH2 + H2O ↔ C2H5NH3
+
+ OH-
CO3
2-
+ H2O ↔ HCO3
-
+ OH-
Weak bases dissociate partially produce few OH-
ion
Vs
Example Strong Acid/Base Example Weak Acid/Base
Concentrated Acid / Base Diluted Acid / Base
Concentrated Acid – High number of mole/amt of solute per dm3
1 M HCI – 1 mole of HCI moleculesin 1 dm3
10 M HCI – 10 mole of HCI moleculesin 1 dm3
Diluted Acid – Low number of mole/amt of solute per dm3
0.1M HCI – 0.1 mole of HCI molecule in 1 dm3
0.01M HCI – 0.01 mole of HCI molecule in 1 dm3
ConcentratedAcid may NOT be a Strong Acid
10M CH3COOH – Concentrated Acid ↑ but Weak Acid ↓
DilutedAcid may be a Strong Acid
0.01M HCI – DilutedAcid ↓ but Strong Acid ↑
10M CH3COOH - CONCENTRATED WEAK acid because 10M acid molecule will dissociate partially forming few H+
ions
0.01M HCI - DILUTED STRONG acid because all 0.01M acid molecule dissociate fully forming H+
ions
Vs
Diprotic base - 2 mole OH-
Ba(OH)2 → Ba2+ + 2OH−
(1 mole) (2 mole)
(1 mole) (1 mole)
6. Strong/Weak Acid and Base
Strong Acid/Weak Acid
Strong acid - HI, HBr, HCI, HNO3, H2SO4, HCIO3, HCIO4
Weak Acid - CH3COOH, HF, HCN, H2CO3, H3BO3, H3PO4
Strong Base/ Weak Base
Strong base - LiOH, KOH, NaOH, CsOH, Ca(OH)2
Weak Base - NH3, C2H5NH2, (CH3)2NH, C3H5O2NH2
Distinguishbet strong and weak acid
ElectricalconductivityRate of rxn pH
Strongacid
Strong acid → High ionization → High conc H+ → High conductivity→ High rate rxn → Lower pH
Strong acid
Oxoacid
O atom > number ionizable proton
HNO3, H2SO4, HCIO3,HCIO4
Hydrohalicacid
HI, HBr, HCI
Weak acid
Hydrohalicacid
HF
Oxoacid
O atom ≥ number ionizable protonby 1
HCIO, HNO2, H3PO4
Carboxylicacid
COOH
Strong base – containOH- or O2-
LiOH, NaOH, CaO, K2O Ca(OH)2, Ba(OH)2
Weak base – contain electronrich nitrogen, N
NH3, C2H5NH2, (CH3)2NH, C3H5O2NH2
Strong base Weak base
1 2 3
Weak acid
0.1 M HCI 0.1 M CH3COOH
H+ 0.1 mole 0.0013 mole
pH 1 (Low) 2.87 (High)
Electrical conductivity High (Ionize completely) Low (Ionize partially)
Rate with magnesium Fast Slow
Rate with calcium
carbonate
Fast Slow
Weaker acid → Low ionization → Low conc H+ → Low conductivity→ Low rate rxn → High pH
Strong acid
HA A-H+
H+ H+
H+
H+ H+
H+
H+A-
A-
A-
A- A-
A-
Ionizes completely
Weak acid
HA
HA
H+ A-
H+
H+
A-
A-
HA
HA
HA
HA
HA
HA
Ionizes partially
7. Easier using pH scale than Conc [H+]
• Conc H+ increase 10x from 0.0001(10-4) to 0.001(10-3)
- pH change by 1 unit from pH 4 to 3
• pH 3 is (10x) more acidic than pH 4
• 1 unit change in pH is 10 fold change in Conc [H+]
Conc OH-
increase ↑ by 10x
pH increase ↑ by 1 unit
pOH with Conc OH-
pOH = -log [OH-
]
[OH-
] = 0.0000001M
pOH = -log [0.0000001]
pOH = -log1010-7
pOH = 7
pH + pOH = 14
pH + 7 = 14
pH = 7 (Neutral)
pH with Conc H+
pH = -log [H+
]
[H+
] = 0.0000001M
pH = -log [0.0000001]
pH = -log1010-7
pH = 7 (Neutral)
Conc H+
increase ↑ by 10x
pH decrease ↓ by 1 unit
pH measurement of Acidity of solution
• pH is the measureof acidity of solutionin logarithmicscale
• pH = powerof hydrogenor minuslogarithmto base ten of hydrogenion concentration
← Acidic – pH < 7 Alkaline – pH > 7 →
pOH with Conc OH-
pOH = -log [OH-
]
[OH-
] = 0.1M
pOH = -log[0.1]
pOH = 1
pH + pOH = 14
pH + 1 = 14
pH = 13 (Alkaline)
pH with Conc H+
pH = -log [H+
]
[H+
] = 0.01M
pH = -log [0.01]
pH = -log1010-2
pH = 2 (Acidic)
Easier pH scaleConc H+
11. Number sig fig in log calculation
Significant number in log calculation
log10(3575)=3.55327 = 3.5532
log10(3.000x104) = 4.477121 = 4.4771
log10(3.3 x 104) = 4.5185 = 4.51
Calculation involve pH = -log10[H+]
Conc H+ = 1.9 x 10-4
pH= -log10[1.9 x 10-4] = 3.721 = 3.72
Measurement scale not linear
• Simple average CANNOT be used
• Average of pH 7, pH 8, pH 9
pH scale is logarithmic, pH = -log[H+]
Correct average = convert to H+ conc
pH 7 = -log10[H+] → H+ = 10-7
pH 8 = -log10[H+] → H+ = 10-8
pH 9 = -log10[H+] → H+ = 10-9
pH pH= -lg10H+ Conc H+
0 0 = -lg10100 1.0
1 1 = -lg1010-1 0.1
2 2 = -lg1010-2 0.01
3 3 = -lg1010-3 0.001
4 4 = -lg1010-4 0.0001
5 5 = -lg1010-5 0.00001
6 6 = -lg1010-6 0.000001
7 7 = -lg1010-7 0.0000001
8 8 = -lg1010-8 0.00000001
9 9 = -lg1010-9 0.000000001
10 10= -lg1010-10 0.0000000001
11 11= -lg1010-11 0.00000000001
12 12= -lg1010-12 0.000000000001
13 13= -lg1010-13 0.0000000000001
14 14= -lg1010-14 0.00000000000001
Easier using pH scale than Conc [H+]
• Low pH – High H+ conc – More acidic
• High pH – Low H+ conc – Less acidic
• pH 3 (10x) more acidic > than pH 4
• 1 unit change in pH is 10 fold change in Conc [H+]
Relationship between pH and Conc H+
Uncertainty involving pH
8
3
987
Average
Uncertainty involving pH
4 sig fig 5 sig fig/4 decimal place
4 sig fig 5 sig fig/4 decimal place
Conc H+ = 3.2 x 10-5 M
pH = - log10[3.2 x 10-5]= 4.4948 = 4.49
2 sig fig 3 sig fig/2 decimal place
2 sig fig3sig fig/2 decimal place
2 sig fig3sig fig/2 decimal place
2 sig fig 3sig fig
2 sig fig3 sig fig
2 sig fig 3 sig fig
pH solution = 7.40. Cal conc of H+ ions
7.40 = -log10 [H+]
[H+] = 10-7.40
= 4.0 x 10-8
3 sig fig 2 sig fig
2 sig fig
4.7
]107.3lg[
107.3
3
101010
8
8
987
pH
pH
Average
Average
12. What is pH for [H+
] = 1 x 10-12
M
pH = -lg [10-12
]
pH = 12
What is conc of H+
of pH 3.20?
3.20 = -lg [H+
]
[H+
] = 10 –2.20
[H+
] = 6.3 x 10-4
pH = -log10[H+] pOH = -log10[OH-] pH + pOH = 14 Kw = [H+][OH-]
Formula acid/basecalculation
2 sig fig 1 sig fig 3 sig fig 2 sig fig
What is pH for [OH-
] = 0.15M
pOH = -lg [0.15]
pOH = 0.823
pH + pOH = 14
pH = 14 – 0.823 = 13.2
pOH = -log[OH-]
3 sig fig 2 sig fig
Calculate conc of H+, OH-
and pH for 0.0010M HCI.
1 2 3
4
CIHHCI
0.001 ↔ 0.001 0.001
OHHOH2
HCIH2O
OHHKw
Assuming H+ all from HCI = 0.0010
)()( 2OHHHCIHH
= 0.001 Negligible / too little
OHH14
100.1
0.3
001.0log
log
10
10
pH
pH
HpH
0.31114
11
101
001.0
100.1
001.0100.1
11
14
14
pH
pOH
OH
OH
or
Cal conc OH-
/pH when3.o x 10-4
H+
add water
HCI
H2O
CIHHCI
OHHOH2
OHHKw
OHH14
100.1
11
4
14
414
103.3
100.3
100.1
100.3100.1
OH
OH
3x10-4 ↔ 3x10-4
52.3
100.3log
log
4
10
10
pH
pH
HpH
13. pH weak acid at variousconcentration
HCOOCHOHCOOHCH 2323
Extendof dissociationdependon initialconcentrationacid
Conc of acid Observed pH CH3COOH CalculatedpH HCI
0.10 2.7 1.0
0.010 3.0 2.0
0.0010 3.5 3.0
0.00010 4.2 4.0
CIHHCI
Weak acid Strong acid
Dissociate partially Dissociate completely
At same acid concentration
• HCI has HIGHER[H+] > CH3COOH
• HCI has LOWER pH < CH3COOH
• HCI dissociate completely - Strong acid
• CH3COOH dissociatepartially - Weak acid
At decreasing acid concentration
• Extend of dissociation for CH3COOH increase
• pH weak acid closer to strong acid
• Dilution increase the extend of dissociation
Conc decrease
HCOOCHOHCOOHCH 2323
Trends
Addition Water
Dilution shift equilibrium to right
Decreaseconc of CH3COOH,CH3COO- andH+
Conc on left side is more effecteddue to CH3COO- and H+
Equilibrium shift to right to increase
conc of CH3COO- and H+ again
Extend of dissociation for acid increase (shift to right)
О
О
Concept Map
[H+] [OH-]
pH pOH
Kw = [H+] x [OH-] = 1 x 10-14
pH + pOH = 14
pH = -lg [H+] [H+] = 10-pH pOH = -lg [OH-] [OH-] = 10-pOH
14. Question on Acid and Base
Which list contains only strong acids ?
A. CH3COOH, H2CO3, H3PO4
B. HCI, HNO3, H2CO3
C. CH3COOH, HNO3, H2SO4
D. HCI, HNO3, H2SO4
When equal volume of four 1M solutions are arranged in order of increasing pH (lowest pH first), what is the correct order?
A. CH3COOH < HNO3 < CH3CH2NH2 < KOH
B. HNO3 < CH3COOH < CH3CH2NH2 < KOH
C. CH3CH2NH2 < HNO3 < CH3COOH < KOH
D. KOH < CH3CH2NH2 < CH3COOH < HNO3
pH of a solution changes from pH =2 to pH =5. What happens to the concentrationof H+ ions during this pH change?
A. Decrease by factor of 1000
B. Increase by factor of 1000
C. Decrease by factor of 100
D. Increase by a factor of 100
Solution of acid A has a pH of 1 and a solution of acid B has a pH of 2. Which statement is correct ?
A. AcidA is stronger than acid B
B. [A] > [B]
C. Concentrationof H+ ions in A is higher than B
D. Concentrationof H+ ions in B is twice the concentrationof H+ in A
100ml of NaOH solution of pH 12 is mixed with 900ml of water. What is the pH of resulting solution?
A. 1
B. 3
C. 11
D. 13
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4
5
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List two ways to distinguish between strong and weak acid/base6
By Conductivitymeasurement
1M StrongAcid – Ionise completely– More H+ ion – pH lower ↓
1M Weak Acid – Ionise partially – Less H+ ion – pH higher ↑
1M StrongAcid – Ionise completely– More H+ ion – Conductivityhigher ↑
1M Weak Acid – Ionise partially – Less H+ ion – Conductivitylower ↓
By pH measurement
Which methodwill distinguishbet equimolarstrong base and strong acid?
i) Add magnesiumto each solutionand observeformationbubbles
ii) Add aqueoussodium hydroxideto each solutionand measuretemp change
iii) Use each solutionin circuit with battery/lampto see brightnesslamp
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15. Click here on pH calculation Click here on Bronsted Lowry/ Lewis Acid/Base
Video on Acid/ Base
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