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List common acids (6)
- Hydrochloric acid - HCl
- Sulfuric acid - H2SO4
- Nitric acid - HNO3
- Phosphoric acid - H3PO4
- Ethanoic Acid - CH3COOH
- Carbonic Acid - H2CO3
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acid + metal
- salt + hydrogen
- not Cu, Hg or Ag
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Common bases
- Ammonia - NH3
- Metal Hydroxides
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Alkalis
bases that dissolve in water (group 1 hydroxides)
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An acid
is a proton donor
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A base
Is a proton acceptor
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Behavious of acids and bases
- isonisation - acid donates a proton to water, water acts as base and forms a hydronium H3O+
- Hydrolysis - anion reacts with water to produce OH-, cation reacts with water to produce H3O+
- Dissociation - when ionic base dissolves in water, it separates into ions
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strengths of acids/bases
ability to readily donate or accept protons
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concentrations of acids and bases
relates to the amount of the substance that is dissolved in a given volume of water
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strong acids
- nitric
- sulfuric
- hydrochloric
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weak acid
acetic/ethanoic acid
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strong bases
- sodium hydroxide
- potassium hydroxide
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indicator
- weak acid/base
- different colour in acidic/basic solutions
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OIL RIG
- Oxidation is loss .... of electrons
- Reduction is gain ... of electrons
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Oxidation
a substance that is oxidised is the one that loses electrons and is thus an electon donor
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Reduction
A substrance that is reduced is the one that gains electrons and is thus an electron acceptor
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Oxidant
- Causes oxidation of another substance
- it itself undergoes reduction
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Reductant
- causes reduction of another substance
- it itself undergoes oxidation
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simple ions
Cl-, S2-
ON - charge of ion
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hydrogen
- +1
- -1 in metal hydrides (NaH)
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Oxygen
- -2
- -1 in peroxides (H2O2, BaO2)
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electronegative element
- The most electronegative element in a compound has the negative oxidation number
- F>O>Cl>N
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Balancing half equations
- key elemnet
- oxygen
- hydrogen
- charge
- states
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Commonly used oxidants
- permanganate ion (MnO4-)
- dichromate ion (Cr2O7-)
- iodine (I2)
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Commonly used reductants
- thiosulfate ion (S2O3 2-)
- oxalate ion (C2O42-)
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