Acids and Redox (4)
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acid
releases H+ protons when dissolved in water
strong acid
releases all H+ protons when in water, it fully dissociates
weak acid
only releases a small amount of H+ protons when i water, and partially dissociates
base
metal oxide, metal hydroxide It neutralises an acid by reacting with the H+ and accepting a proton.
alkali
a base that when dissolved in water, releases OH- ions
salt
a product of a neutralisation reaction where an H+ in an acid has been replaced by a metal or ammonium ion.
acid + base
→ salt + water
acid + alkali
→ salt + water
acid + metal carbonate
→ salt + water + carbon dioxide
acid + metal
→ salt + hydrogen
hydrochloric acid (HCl)
chloride
sulphuric acid (H2SO4)
sulphate
nitric acid (HNO3)
nitrate
phosphoric acid (H3PO4)
phosphate
ethanoic acid (CH3COOH)
ethanoate
titration
technique used with a burette and a pipette. Put acid in burette, put alkali in flask with indicator. See it go from purple to colourless, that’s the end point. Can calculate concentration
concordant
result that are within 0.1cm3 of each other
oxidation numbers in elements
always zero
oxidation numbers for compounds or ions
the number of their charge is their oxidation number e.g. O2 is -2
sum of oxidation numbers
total number of charge
redox reaction
oxidation and reduction happening at the same time
oxidation
addition of oxygen, loss of electrons or increase of oxidation numbers
reduction
reduction of oxygen, gain of electrons or decrease in oxidation number
percentage uncertainty
uncertainty/measurement x100