inorganic Flashcards
Acid + alkali.
NaOH+HCl
NaOH (aq) + HCl (aq) → NaCl (aq) + H2O(l) NH3 (aq) + HCl (aq) → NH4Cl (aq)
Dissolving sodium hydroxide in water
NaOH (s) → Na+(aq) + –OH(aq)
Ammonia + water
NH3 (g) + H2O (l) → NH4 +(aq) + –OH(aq)
Acid + metal oxide
CaO (s) + 2HCl (aq) → CaCl2 (aq) + H2O (l)
Acid + carbonate
CaCO3 (s) + 2HCl (aq) → CaCl2 (aq) + H2O (l) + CO2 (g)
Magnesium and water + Magnesium and Steam
Mg (s) + 2H2O (l) → Mg(OH)2 (s) + H2 (g) (very slow) NOTE: Mg(OH)2 is sparingly soluble
Ca, Sr and Ba all react readily with cold water to form the hydroxide and hydrogen
Mg(s) + H2O(g) → MgO (s) + H2(g) (reacts readily)
MgO is formed because the hydroxide is unstable at higher temps:
Mg(OH)2 → MgO + H2O
Reaction with oxygen
Ca (s) + ½O2 (g) → CaO (s)
Reaction of group II chlorides with NaOH - shows the solubilities of group 2 hydroxides
MgCl2 (aq) + 2NaOH (aq) → Mg(OH)2 (s) + 2NaCl (aq)
white ppt
e.g. BaCl2(aq) + 2NaOH(aq) → Ba(OH)2 (aq) + 2NaCl(aq
colourless sol
Reaction of group II hydroxides with acid
Mg(OH)2 + 2HCl → MgCl2 + 2H2O
Ca(OH)2 + H2SO4 → CaSO4 + 2H2O
Test for sulphate ion
STEP 1: Add d.HCl to remove ions which might interfere with the test:
2H+ + CO32- → CO2 + H2O
STEP 2: Add barium chloride:
Full eqn: BaCl2 (aq) + Na2SO4 (aq) → BaSO4 (s) + 2NaCl (aq)
Ionic Eqn: Ba2+ (aq) + SO42- (aq) → BaSO4 (s)
white ppt
Extraction of Titanium using Mg
TiCl4 + 2Mg → Ti + 2MgCl2
Equation to show halogen, X2, acting as an oxidising agent:
Cl2 + 2e- → 2Cl-
Displacement Reactions
Cl2 (aq) + 2Br- (aq) → Br2 (aq) + 2Cl- (aq
Colourless sol to orange sol
Cl2 (aq) + 2I- (aq) → I2 (aq) + 2Cl- (
colourless sol to brown sol
2I- (aq) + Br2 (aq) → I2 (aq) + 2Br- (aq)
colourless sol to brown sol
Reaction of halide Ions with c.H2SO4
To form the hydrogen sulphate (white solid) and HX (misty white fumes) – NOT REDOX
NaX (s) + H2SO4 (aq) → NaHSO4 (s) + HX
Testing for halide Ions in solution
STEP 1: Add d.HNO3 to remove ions that might interfere with the test:
2HNO3 + Na2CO3 → 2NaNO3 + CO2 + H2O
otherwise: 2Ag+ (aq) + CO32- (aq) → Ag2CO3 (s) ∴ CO32- gives a ppt if not removed
STEP 2: Add AgNO3 (aq)
PPt formed with halide ions in sol (Ag+)
Ag+ (aq) + F- (aq) → AgF (aq) no ppt so doesn’t work as a test
Ag+ (aq) + Cl- (aq) → AgCl (s) ppt dissolves in d.NH3
AgCl(s) + 2NH3 (aq) → [Ag(NH3)2]+(aq) + Cl-(aq)
Ag+ (aq) + Br- (aq) → AgBr (s) ppt does not dissolve in d.NH3 but dissolves in c.NH3
Ag+ (aq) + I- (aq) → AgI (s) ppt does not dissolve in d.NH3 or c.NH
form chloric(I)acid and HCl – DISPROPORTIONATION REACTION
Cl2 + H2O ⇌ HCl + HClO
decomposition of Cl2 in water in presence of sunlight
2Cl2 (g) + 2H2O (l) → 4H+ (aq) + 4Cl- (aq) + O2 (g)
Reaction of chlorine with sodium hydroxide (bleach)
DISPROPORTIONATION
Cl2 (g) + 2NaOH (aq) → NaClO (aq) + NaCl (aq) + H2O (l)
