Acids
1.Arrhenius
defines acids as a substance that ionises in water produce hydrogn
ions, H+ .
2.Hydrochloric acid, HCl, is an acid as
it dissociates in water to form hydrogen ions.
3.HCl (g) + aq ® H+ (aq) + Cl- (aq)
4.The hydrogen ion interacts strongly with a water molecule to
form hydroxonium ion, H3O+ .
5. The simplified
form of hydroxonium ion, H3O+ is hydrogen ion, H+.
6. The higher the concentration of H+ , the stronger the acid is.
7. An example of a monoprotic acid is hydrochloric acid, HCl.
8. An example of a diprotic acid is sulphuric acid, H2SO4.
Physical properties of
acids
1.Sour taste
2.Corrosive
3.pH lower than 7
4.Turns blue litmus red
5.Conducts electricity
Bases
1.Bases is defined as a substance that can
neutralize acids to form salt and water.
2.A base which is soluble in water is known as
an alkali.
3.An alkali is a substance that ionises in
water to produce hydroxide ions, OH-
4. NaOH (s) + aq ® Na+ (aq) + OH- (aq)
Physical properties of
alkalis
1.Bitter taste
2.Slippery feel
3.pH higher than 7
4.Turns red litmus blue
5.Conducts electricity
Uses of acids, bases and
alkalis
1.Citric acid in lemon juice
can be used to clean brass and bronze ornaments as the acid
reacts with
copper(II) oxide that builds on the surface of the ornaments.
2.Hydrochloric acid is used
in cleaning metals before they are electroplated.
3.Ammonia is used as a
cleaning agent as it is a good solvent for grease.
4. Calcium oxide (quicklime) is used to neutralize the acidity of factory effluents before discharging it into nearby streams and rivers.
5. Methanoic acid aids the coagulation of latex by neutrailising the negative charges on rubber particles.
6. Sodium hydroxide is used to make soaps, detergents and bleaching agents.
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Enjoy yourself with the following video.
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