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Applications of neutralisation reactions - Coggle Diagram
Applications of neutralisation reactions
industrial processes
Waste water
if too acidic/alkaline
can damage environment
too acidic
use calcium oxide
neutralisation
SO2(g) + CaO -> CaSO3(s)
too alkaline
sulfuric acid, hydrochloric acid, nitric acid
agriculture
fertilisers
made from neutralisation
sulfuric acid + ammonia gas
NH3(g) + H2SO4(aq) -> (NH4)2SO4(aq)
ability of plants to take up nutrients
affected by acids and bases
some plants grow better in acidic or basic soils
industry spills
acid spills
use sodium carbonate, sodium hydrogen carbonate
acidic water from mining activities
flows into nearby waterways
base spills
dilute sulfuric/hydrochloric acid
mining
acidic discharge
can occur naturally
large scale disturbances of rocks
increase acid drainage
bacteria accelerates oxidation and acidification
bases
smelting of metals
leached out during mining operations
soil acidification
deposition of acidic substances in soil
drop in pH can be low enough to affect plant growth
acidic soils
lime and dolomite
neutralise acids
manufacturing and bases
alkalis (sodium hydroxide)
released into waste water
everyday life
toothpaste
tooth enamel
basic
easily decayed by acid
Ca5(PO4)3OH + 4H+ -> 5Ca2+ 3(HPO4)2- + H2O
flouride in toothpaste
strengthens tooth enamel
replaces OH- in hydroxyapatite
forming flourhydroxyapatite
resistant to acids
contains mild abrasives
remove food particles
neutralise acids
antacids
reduce acid levels in stomach
contain magnesium hydroxide bases
Mg(OH)2(s) + H2O(l) -> MgCl2(aq) + 2H2O(l)
baking soda
sodium hydrogen carbonate
combines with acidic ingredients
dough rises
cleaning products
usually basic
often washed into sewers
eventually reach waterways
require neutralisation
gases in the atmosphere
acidic oxides
present as gases in the atmosphere
dissolve in falling rain
CO2(g) + H2O(l) -> H2CO3(aq)
carbon dioxide
present naturally
human made - industrial
acidic and basic soils
acid sulfate soils
in estuaries
include iron sulfide minerals
if drained, exposed
sulfides in soil are oxidised
soil more acidic
soil produce acidic waterways
alkaline soils
accumulation of metal ions
usually toxic levels
naturally alkaline
calcium carbonate
bicarbonate
often salty
most crops will not grow
waterways
increases waters ability to corrode
should be neutralised before being discharged
neutralisation reaction
acid + base -> salt + water
H+(aq) + OH-(aq) -> H2O(l)
example
HCl(aq) + KOH(aq) -> H2O(l) + KCl(aq)