4961157
Description
Mind Map by madi.stewardson, updated more than 1 year ago
|
Created by madi.stewardson
over 8 years ago
|
|
The Acidic Environment
- Indicators
- Bromothymol blue (yellow)6.2-7.6(blue)
-Methyl orange (red)3.1-4.4(yellow)
-phenolphthalein (colourless)8.3-10.0(pink)
- Bromothymol blue (yellow)6.2-7.6(blue)
-Methyl orange (red)3.1-4.4(yellow)
-phenolphthalein (colourless)8.3-10.0(pink)
- pH of oxides
- non-metal
oxides- acidic
- metal oxides-
basic
- amphoteric-
can be both eg.
H2O
- non-metal
oxides- acidic
- Le Chatelier’s Principle
- counteract
any change
in
equilbrium
- counteract
any change
in
equilbrium
- oxide production
- sulfur oxides
- volcanoes-burning of
fossil fuels - smelting
metal ores
- volcanoes-burning of
fossil fuels - smelting
metal ores
- nitrogen oxides
- lightning- vechicles
- lightning- vechicles
- sulfur oxides
- acid rain
- pH <5 - SO or NO in H2O
Annotations:
- SO2(g) + H2O(l) -> H2SO3(aq) 2NO2(g) + H2O(l) -> HNO3(aq) + HNO2(aq) 2H2SO3(aq) + O2(g) -> 2H2SO4(aq) 2HNO2(aq) + O2(g) -> 2HNO3(aq)
- effects
- kill aquatic ecosystem
-leeches minerals needed
for plants -erodes buildings
- kill aquatic ecosystem
-leeches minerals needed
for plants -erodes buildings
- pH <5 - SO or NO in H2O
- acids
- weak
- 1-99% ionised - CH3COOH
(ethonoic acid - C6O7H8
(citric acid)
- 1-99% ionised - CH3COOH
(ethonoic acid - C6O7H8
(citric acid)
- strong
- 100% ionised -HCl - H2SO4
- 100% ionised -HCl - H2SO4
- weak
- pH = -log10[H+]
- %ionisation = [H+]
divide [acid] x 100
- History
- Lavosier- acid oxygen
- Davy- replaceable hydrogen
- Arrhenius- H+ and OH-
- Bronsted and Lowry-
acid proton donor base
proton accepter
- Lavosier- acid oxygen
- Conjugate acid/base
- molecules related by the loss or gain of a
proton eg. H20 (acid) and H30+
(conjugate base(accepted))
- molecules related by the loss or gain of a
proton eg. H20 (acid) and H30+
(conjugate base(accepted))
- neutralisation reactions
- salt based on stronger acid/base
-strong+strong=neutral salt + H2O
- salt based on stronger acid/base
-strong+strong=neutral salt + H2O
- Buffer
- weak acid and
conjugate base eg.
HCO3- and CO3 2-
- used in blood, minimises pH change
- weak acid and
conjugate base eg.
HCO3- and CO3 2-
- Titration
- reacting a solution of unknown
concentration with a standard
- method
Annotations:
- (1) Choose indicator which has an end point suitable to equivalence point (2) Rinse glassware with distilled water, and then with the acid/base (3) Wash conical flask with distilled water (4) Fill 25mL pipette with aliquot of standard solution in volumetric flask (5) Add 3 drops of indicator to the flask (6) Fill burette with titrant, using dropper to add the final volumes (7) Assemble retort stand and equipment appropriately (8) Titrate with the left hand and swirl with right. Repeat 3 times for accuracy.
- reacting a solution of unknown
concentration with a standard
- acids in food
- -flavour enhancers
-preservative
-anti-oxidant
- -flavour enhancers
-preservative
-anti-oxidant
- carbon dioxide
- high pressure- CO2 gas dissolves
- temperature - dissolving of gas is exothermic
- Acidity- acid would create more CO2 gas
- high pressure- CO2 gas dissolves
Want to create your own Mind Maps for free with GoConqr? Learn more.