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acids + metals →
salt + H2
acids + bases →
salt + H2O
acids + carbonates →
salt + H2O + CO2
acids effect on litmus
red
acids effect on methyl orange
red
acids effect on thymolphthalein
colourless
define the term ‘bases’
oxides or hydroxides of metals
define the term ‘alkali’
soluble bases that release hydroxide ions in solution
bases + ammonium salts →
salt + water + NH3
ex: NH4Cl + NaOH → NaCl + H2O + NH3
alkali effect on litmus
blue
alkali effect on thymolphthalein
blue
alkali effect on methyl orange
yellow
what ions do aqueous solutions of acids contain?
H+ ions
what ions do aqueous solutions of alkalis contain?
OH- ions
ph scale
acids: pH less than 7
alkalis: pH greater than 7
neutral: pH exactly 7
(check from book)
neutralization reaction (water)
H+ (aq.) + OH- (aq.) → H2O (l)
acids are proton ____
donors
bases are proton ____
acceptors
strong acid
an acid that is completely dissociated in aqueous solution
weak acid
an acid that is partially dissociated in aqueous solution
strong acid and its symbol equation
hydrochloric acid
HCl (aq) → H+ (aq) Cl- (aq)
weak acid and its symbol equation
ethanoic acid
CH3COOH (aq) ⇌ H+ (aq) + CH3COO- (aq)
3 types of oxides
acidic (non-metal oxides)
basic (metal oxides)
amphoteric
acidic oxides
non-metal oxides
SO2
CO2
basic oxides
metal oxides
CaO
CuO
amphoteric oxides
react with acids and with bases to produce a salt and water
ZnO
Al2O3
ZaP