Salts:
Ionic compounds formed by replacement of H+ ion in an acid by metal ion or NH4+ ion.
Naming salts:
1st part of the name comes from :
Metal
Metal carbonate
OR
Metal hydroxide
Last part of the name comes from the acid:
HCl = chloride salt
H2SO4 = sulfate salt
HNO3 = nitrate salt
Examples:
Mg + 2HCl MgCl2 + H2
Mg + H2SO4 MgSO4 + H2
Mg + 2HNO3 Mg(NO3)2 + H2
Sr.# Type Of Salt Solubility In Water
1 Nitrates NO3- All are soluble.
2 Halides: All are soluble except Pb2+ and Ag+
Chloride ( Cl- )
Bromides ( Br- )
Iodides ( I- )
3 Sulfates All are soluble except Pb2+, Ag+, Ba2+, Ca2+
4 Carbonates (CO32- ) All are insoluble except Na+, K+, NH4+
5 Oxides and Hydroxides All are insoluble except Na+, K+
6 Cations All Na+, K+, NH4+ salts are soluble.
Write if the following salts are soluble OR insoluble:
Sodium nitrate_____________________
Silver chloride_____________________
Lead sulfate________________________
Barium sulfate________________________
Lead nitrate_________________________
Magnesium chloride__________________
Calcium sulfate_____________________
Ammonium carbonate__________________
Write the formula of salts that can be prepared from these ions:
Ca2+ , H+, Mg2+, NO3-, Cl-
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Methods Of Preparation Of Salts:
Insoluble salts:
• By precipitation method.
• Solutions of 2 soluble salts are mixed together to form insoluble salt.
barium nitrate(aq) + sodium sulfate(aq) barium sulfate(s) + sodium nitrate(aq)
• Insoluble salt can be separated from the mixture by filtration.
• Crystals of soluble salt can be obtained by crystallization method.
Soluble Salts:
Titration
By excess method
Reaction of :
Reaction of:
Alkali + acid salt + water
Metal + acid salt + hydrogen
KOH + H2SO4 K2 SO4 + H2O
Metal carbonate+ acid salt + carbon dioxide
Method:
+water
• Put a measured amount of alkali in
Metal oxide + acid salt + water
the conical flask. Add a few drops
Method: of indicator.
• Dissolve metal/metal carbonate/metal oxide • Put the acid from the burette till
in acid. the indicator changes colour( end
• Continue dissolving till an excess is left at the point is reached). Note the volume
bottom of the beaker. of the acid used.
• Filter the excess metal/metal • Repeat the experiment without the
carbonate/metal oxide. indicator.
• Heat the filtrate till saturation point • Heat the salt solution till saturation
point.
• Cool the saturated solution till crystals form.
• Allow the saturated solution to cool
• Dry the crystals on a filter paper.
till crystals are formed.
• Dry the crystals on a filter paper.
Q) Potassium sulfate is a soluble salt. Outline the preparation of a pure, dry sample of
potassium sulfate, starting from dilute sulfuric acid.
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