An acid that completely disassociates in aqueous solution to form H+ ions.
An acid that partially disassociates in aqueous solution to form H+ ions.
Aqueous solutions of bases contain OH- ions.
Acid - Red
Base - Blue
Neutral - Purple
Acid - Colourless
Base - Blue
Acid: Red
Base : Yellow
1) Only metals above hydrogen in the reactivity series will react with dilute acids. (MAZIT metals)
Acid + Metal → Salt + Hydrogen
2) Soluble salt is prepared by filtration -> evaporation -> crystallisation
1) Metal oxides and metal hydroxides (alkalis) can act as bases
2) When they react with acid, a neutralisation reaction occurs
Acid + Base → Salt + Water
3) The soluble salt can be prepared by evaporation -> crystallisation
Acid + Metal Carbonate → Salt + Carbon Dioxide + Water
1) Soluble salt can be prepared by Filtration -> Evaporation -> Crystallisation.
1) Ammonium salts undergo decomposition to form ammonia when warmed with an alkali
Ammonium Salt+ Alkali → Salt+ Water+ Ammonia
2) Presence of ammonia can be checked by turning damp red litmus blue.
Acidic, including SO2 and CO2.
Basic, including CuO and CaO
Oxides that react with BOTH acids and bases to form salt + water.
Eg. Al2O3 and ZnO (Aluminium oxide, zinc oxide)
1) Made by precipitation
Soluble salt (AX) + Soluble Salt (BY) -> Soluble Salt (AY) + Insoluble Salt (BX)
2) Insoluble salt can be prepared by Filtration -> Washing -> Drying
Hydrated - Chemically combined with water
Anhydrous - Substance containing no water
Water of crystallisation - Water molecules present in hydrated crystals.
1) Sodium, Potassium, Ammonium Salts are soluble
2) Nitrates are soluble
3) Chlorides are soluble except lead and silver
4) Sulfates are soluble except barium, calcium and lead
5) Carbonates are insoluble except sodium, potassium and ammonium
6) Hydroxides are insoluble, except sodium, potassium, ammonium and calcium