Chapter 7

Changes colour to match pH scale (depending on pH of solution)

• red in acidic solutions • purple in neutral solutions • blue in alkaline solutions

• Red litmus paper -> turns blue in alkaline solutioms • Blue litmus paper -> turns red in acidic solutions

• Red in acidic solutions • Yellow in alkaline solutions

• Colourless in acidic soloutions • Blue in alkaline solutions

H+ donor/proton donor

H+ receiver/ proton acceptor

Base that is soluble in water

Reaction between an acid and a base/alkali -> products are neutral

Contain H+ ions -> this is because acids ionise (split up) in solution to produce a hydrogen ion, H+, and another ion Eg: HCl -> H+ + Cl -

Contain OH- ions -> this is because acids ionise (split up) in solution to produce a hydroxide ion, OH- and another ion Eg: NaOH -> Na+ + OH-

Acid + base (metal oxide or hydroxides) -> salt (sulfates, nitrates or chlorides) + water

Acid + ammonia -> ammonium salt

Acid + metal -> salt + hydrogen

Acid + metal carbonate -> salt + water + carbon dioxide

Base + ammonium salt -> salt + water + ammonia

• react with bases • are non-metal oxides -> on right side of periodic table Eg: SO2 and CO2

• react with acids • are metal oxides -> on left side of periodic table Eg: CaO and CuO

• reacts with bothe acids and bases to form salt and water • only zin oxide (ZnO) and aluminium oxide (Al2O3) • experiment: to prove amphoteric add ZnO to acid and base -> should dissolve in both

Acid that is completely ionised (dissociated) in aqueous solution -> releasing lots of H+ ions

Acid that is partially ionised (dissociated) in aqueous solution -> releasing fewer H+ ions

Soluble: ALL Insoluble: NONE

Soluble: ALL Insoluble: NONE

Soluble: ALL Insoluble: NONE