2.34 - 2.42 acids, bases and salt preparations

Solubility of sodium compounds in water

All soluble

Solubility of potassium compounds in water

All soluble

Solubility of ammonium compounds in water

All soluble

Solubility of nitrates compounds in water

All soluble

Solubility of chloride compounds in water

All soluble excepts silver, lead chloride

Solubility of sulfate compounds in water

All soluble except lead, barium, calcium sulfates

Solubility of carbonates compounds in water

All insoluble except sodium, potassium, ammonium carbonate

Solubility of hydroxide compounds in water

All insoluble except sodium, potassium, ammonium

Difference between acids and bases in terms of proton transfer

Acids donate protons (H+)

Bases accept protons

Acid + base →

Salt + water

Acid + metal →

Salt + hydrogen

Acid + metal carbonate →

Salt + water + carbon dioxide

How to form the formula of the salt formed ?

• take the metal in the base/metal/carbonate

• Criss cross with the ion part of the acid which isn’t hydrogen to get the salt

Eg.

Acid + base → salt + water

H2SO4 + MgO → MgSO4 + H2O

SO^2- 4 Criss cross Mg2+ Which is MgSO4 because the 2- and 2+ cancel out

What are some examples of compounds that can act as bases

Metal oxides, metal hydroxides and ammonia

What are alkalis

Bases that are soluble in water

Describe an experiment to prepare a pure, dry sample of soluble salt, starting from an insoluble reactant

• add excess insoluble base to the acid

• Filter to remove unreacted base

• Heat the solution so that water evaporates and crystals of the salt remain