- All Group I (sodium, potassium) compounds are soluble.
- All ammonium salts are soluble.
- All nitrates are soluble.
- Examples of insoluble salts: AgCl, PbCl2, AgI,
PbI2, BaSO4, CaSO4.
Precipitation method: If it's insoluble, then the steps are simple. Mix two solutions in a beaker and the desired salt precipitates out. Then filter out the precipitate and dry it.
Worked Example: Describe, with the aid of balanced chemical and ionic equations, how you would prepare lead iodide.
[Solution]
Lead iodide PbI2 is an insoluble salt. So, use the precipitation method.
Choose two solutions of soluble compounds that are readily available in the laboratory: lead(II) nitrate and potassium iodide (Remember: All nitrates are soluble. All potassium salts are soluble.)
Steps:
- Add colorless solution of lead(II) nitrate to colorless
solution of potassium iodide in a beaker. A yellow precipitate of
lead(II) iodide is formed.
Ionic equation: Pb2+(aq) + 2I-(aq) --> PbI2(s)
- Filter the suspension to obtain the residue of lead(II)
iodide.
- Dry the lead(II) iodide salt under an infrared lamp.
Titration method: If it's a soluble salt of Group I metals or ammonium, use the titration method. The description of this method is pretty long. Basically, a titration between an acid and an alkali is performed using an indicator. This is to determine the volume of the acid or alkali needed to completely neutralize the other. The mixture is discarded and the step is repeated without the indicator. Now, you get the solution of the required salt. The salt is finally obtained from its solution by crystallization.
Worked Example: Describe how you would prepare rubidium sulfate.
[Solution]
Check the Periodic Table and you find that rubidium is in Group I. So Rb2SO4 is soluble. The acid part of the salt clearly comes from H2SO4 while the base part of the salt can come from rubidium hydroxide RbOH (similar to NaOH and KOH). The titration method should be used.
Steps:
- Place RbOH in a burette.
- Pipette 25.0 cm3 of H2SO4
into a conical flask.
- Add an indicator into the H2SO4.
- Run RbOH from the burette into the acid until the indicator
just changes color.
- Repeat the above steps without the indicator so that you
obtain a colorless Rb2SO4 solution.
- Evaporate some of the water to obtain a saturated solution of
Rb2SO4. Let the saturated solution to cool so
that Rb2SO4 crystallizes out. Filter the
crystals and dry them under an infrared lamp.
Now, salts of Group I metals and ammonium are not the only soluble salts. What if you are asked to prepare copper(II) sulfate or zinc chloride? You cannot simply suggest titrating Cu(OH)2 or Zn(OH)2 with H2SO4 or HCl because Cu(OH)2 and Zn(OH)2 are insoluble solids (precipitates) if you remember your Qualitative Tests for Metals. Here are other methods you can use.
- acid + insoluble base --> salt + water
- acid + insoluble carbonate --> salt + water + carbon
dioxide
- acid + metal --> salt + hydrogen gas
- Most bases (e.g. CuO) are insoluble. Only oxides of Group I
metals and some Group II metals are soluble.
- Most carbonates (e.g. CaCO3, CuCO3) are
insoluble. Only ammonium carbonate, Group I carbonates are soluble.
- Copper does not react with dilute HCl and H2SO4.
Do not suggest preparing CuSO4 or CuCl2 by
reacting Cu with dilute acids.
Worked Example: Describe how you would prepare copper(II) sulfate.
[Solution]
The acid part of copper(II) sulfate is clearly from sulfuric acid. The base part can come from CuO or CuCO3 but not from Cu because Cu does not react with dilute H2SO4.
Steps:
- Add excess CuO (a black solid powder) or CuCO3 (a
green solid powder) to a beaker of dilute H2SO4
and stir. The solid dissolves and the solution turns blue.
Or: CuCO3(s) + H2SO4(aq) --> CuSO4(aq) + H2O(l) + CO2(g)
- Filter the unreacted CuO or CuCO3 to obtain the
blue filtrate solution of CuSO4.
- Evaporate some of the water to obtain a saturated solution of
CuSO4. Let the saturated solution to cool so that CuSO4
crystallizes out. Filter the crystals and dry them under an infrared
lamp.
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