Friday, July 10, 2009
Preparing an insoluble salt
Two soluble metal salts react with each other to form one soluble salt and one insoluble salt. Lead nitrate solution and sodium chloride solution react to produce solid lead chloride, leaving soluble sodium nitrate in solution. The lead chloride can be recovered by filtration.
Read our standard health & safety guidance
Most classes should be able to perform this experiment as a class experiment, but if there are real doubts about safe behaviour or adequate manipulative skills while solutions are being heated, or hot solutions being poured into the filter paper, then student-aided demonstrations of these may be more sensible.
Apparatus and chemicals
Eye protection
Each working group requires:
Test-tubes (100 x 16 mm), 2 Rubber stopper to fit test-tube, Beakers (100 cm3), 2 Teat pipette
Glass rod (15 cm), Measuring cylinder (25 cm3), Wash bottle with purified (distilled or eionised) water, Filter funnel (65 mm diameter), Filter paper, Bunsen burner, Tripod, Gauze
Heat resistant mat
Lead(II) nitrate solution, 1 mol dm-3 (Toxic, Dangerous for the environment), 5 cm3 (in a small bottle)
Sodium chloride solution, 2 mol dm-3 (Low hazard), 10 cm3 (in a small bottle)
Technical notes
Lead(II) nitrate solution (Toxic, Dangerous for the environment)
Sodium chloride solution (Low hazard)
Lead(II) chloride (Toxic, Dangerous for the environment)
1 If a centrifuge is not available the solid can be separated by filtration, however the crystals obtained will not be as pure using this method.
2 At the end of the experiment the lead chloride should NOT be discarded into the rubbish. Collect together and place in a labelled bottle, for future use (if you think it is pure enough) or for eventual disposal as hazardous waste by a licensed contractor.
Procedure
HEALTH & SAFETY: Wear eye protection
Stage 1
a Add 5 cm3 of 1 mol dm-3 lead(II) nitrate solution to a test-tube. Then add an equal volume of 2 mol dm-3 sodium chloride solution, stopper the tube and shake gently to mix thoroughly.
b Centrifuge the suspension, and pour away the clear liquid. Add a few cm3 of purified water to the solid in the test-tube, stopper and shake to wash the precipitate. Centrifuge again, and pour away the clear liquid.
If a centrifuge is not available, filter the precipitate using a filter paper and filter funnel. Wash the precipitate by pouring a small amount of purified water over the residue and allowing it to filter through.
Stage 2
a If a centrifuge was used, add a little more purified water to the test-tube, stopper and shake to mix. Quickly pour the mixture into a beaker, and use more purified water to rinse any remaining solid from the test-tube to the beaker. Make up the volume of liquid in the beaker to about 30 cm3 with more purified water.
If the precipitate was obtained by filtration, transfer the solid residue to a beaker and add about 30 cm3 of purified water.
b Heat the suspension in the beaker gently over a medium Bunsen flame, with stirring, until the suspension has all dissolved in the hot water. Remove the flame and allow to cool. Crystals should form on cooling. They can be collected by filtration and dried on a paper towel. At the end of this experiment, you MUST wash your hands to remove any toxic lead compounds that may have splashed onto them.
Teaching notes
There may be problems associated with younger students heating beakers perched on tripods, and with lifting hot glassware off a hot tripod after heating. They should not be sitting down while carrying out these operations. Using tongs of suitable size is a good solution for lifting the hot beakers, but some schools may not have these. If there is any doubt about the safety of this step, you should assist students when lifting each beaker down onto the heat resistant mat.
Students should be told to be careful when handling the lead nitrate solution and the solid lead chloride produced. Insist that they wash their hands after any splashes and at the end of the preparation.
Students who have not used a centrifuge before need to be instructed on how to use it, especially the need for a balancing tube with a similar volume of water.
The balanced equation for the reaction is only relevant for older students:
Pb(NO3)2(aq) + 2NaCl(aq) → PbCl2(s) + 2NaNO3(aq)
Otherwise, a simple word equation is sufficient, but note that there is no easy way of demonstrating that sodium nitrate is the other product left in solution.
Read our standard health & safety guidance
Most classes should be able to perform this experiment as a class experiment, but if there are real doubts about safe behaviour or adequate manipulative skills while solutions are being heated, or hot solutions being poured into the filter paper, then student-aided demonstrations of these may be more sensible.
Apparatus and chemicals
Eye protection
Each working group requires:
Test-tubes (100 x 16 mm), 2 Rubber stopper to fit test-tube, Beakers (100 cm3), 2 Teat pipette
Glass rod (15 cm), Measuring cylinder (25 cm3), Wash bottle with purified (distilled or eionised) water, Filter funnel (65 mm diameter), Filter paper, Bunsen burner, Tripod, Gauze
Heat resistant mat
Lead(II) nitrate solution, 1 mol dm-3 (Toxic, Dangerous for the environment), 5 cm3 (in a small bottle)
Sodium chloride solution, 2 mol dm-3 (Low hazard), 10 cm3 (in a small bottle)
Technical notes
Lead(II) nitrate solution (Toxic, Dangerous for the environment)
Sodium chloride solution (Low hazard)
Lead(II) chloride (Toxic, Dangerous for the environment)
1 If a centrifuge is not available the solid can be separated by filtration, however the crystals obtained will not be as pure using this method.
2 At the end of the experiment the lead chloride should NOT be discarded into the rubbish. Collect together and place in a labelled bottle, for future use (if you think it is pure enough) or for eventual disposal as hazardous waste by a licensed contractor.
Procedure
HEALTH & SAFETY: Wear eye protection
Stage 1
a Add 5 cm3 of 1 mol dm-3 lead(II) nitrate solution to a test-tube. Then add an equal volume of 2 mol dm-3 sodium chloride solution, stopper the tube and shake gently to mix thoroughly.
b Centrifuge the suspension, and pour away the clear liquid. Add a few cm3 of purified water to the solid in the test-tube, stopper and shake to wash the precipitate. Centrifuge again, and pour away the clear liquid.
If a centrifuge is not available, filter the precipitate using a filter paper and filter funnel. Wash the precipitate by pouring a small amount of purified water over the residue and allowing it to filter through.
Stage 2
a If a centrifuge was used, add a little more purified water to the test-tube, stopper and shake to mix. Quickly pour the mixture into a beaker, and use more purified water to rinse any remaining solid from the test-tube to the beaker. Make up the volume of liquid in the beaker to about 30 cm3 with more purified water.
If the precipitate was obtained by filtration, transfer the solid residue to a beaker and add about 30 cm3 of purified water.
b Heat the suspension in the beaker gently over a medium Bunsen flame, with stirring, until the suspension has all dissolved in the hot water. Remove the flame and allow to cool. Crystals should form on cooling. They can be collected by filtration and dried on a paper towel. At the end of this experiment, you MUST wash your hands to remove any toxic lead compounds that may have splashed onto them.
Teaching notes
There may be problems associated with younger students heating beakers perched on tripods, and with lifting hot glassware off a hot tripod after heating. They should not be sitting down while carrying out these operations. Using tongs of suitable size is a good solution for lifting the hot beakers, but some schools may not have these. If there is any doubt about the safety of this step, you should assist students when lifting each beaker down onto the heat resistant mat.
Students should be told to be careful when handling the lead nitrate solution and the solid lead chloride produced. Insist that they wash their hands after any splashes and at the end of the preparation.
Students who have not used a centrifuge before need to be instructed on how to use it, especially the need for a balancing tube with a similar volume of water.
The balanced equation for the reaction is only relevant for older students:
Pb(NO3)2(aq) + 2NaCl(aq) → PbCl2(s) + 2NaNO3(aq)
Otherwise, a simple word equation is sufficient, but note that there is no easy way of demonstrating that sodium nitrate is the other product left in solution.
What is an insoluble salt?
An insoluble salt is a salt which dissolves very very little in water. Be careful! Very many say that insoluble means that it cannot dissole in water. It's not true. There is NO substance that cannot dissolve in water. They dissolve VERY little so it's considered that they don't dissolve.
Soluble salts are considered the ones having an alkali or an alkali earth metal in their structure. All the others are insoluble.
Soluble salts are considered the ones having an alkali or an alkali earth metal in their structure. All the others are insoluble.
Salts
A crystalline compounds composed of the negative ion of an acid and the positive ion of a base.
Neutralization: the reaction of a base and an acid to produce a salt and water.
sodium hydroxide + hydrochloric acid yields sodium chloride + water
While the reaction shown here usually comes to mind when salt production is mentioned, there are many reactions that produce salts. It is even possible to have salts that do not produce neutral solutions.
Salts can also be formed by the reaction of an acidic or basic anhydride with a corresponding base, acid, or anhydride.
* acidic anhydride + base salt
SO3 + 2NaOH Na2SO4 + H2O
* basic anhydride + acid salt
Na2O + H2SO4 Na2SO4 + H2O
* basic anhydride + acidic anhydride salt
Na2O + SO3 Na2SO4
Certain acids and bases react to produce only a partial neutralization. These reactions produce either acidic salts or basic salts.
* This reaction produces an acidic salt:
H2SO4 (aq) + NaOH (aq) NaHSO4 (aq) + H2O (l)
Sodium hydrogen sulfate is an acidic salt because it still contains an ionizable hydrogen atom.
Naming salts:
the name of a salt is related to the name of the acid that forms it.
* Binary acids produce salts ending with ide.
* Ternary acids ending in ic produce salts ending with ate.
* Ternary acids ending in ous produce salts ending with ite.
* Any prefixes in the ternary acid remain in the salt name.
* In naming acidic and basic salts, each ion in the salt is named separately.
o Hydrogen is named immediately before the names of any negative ions.
+ A prefix is used to indicate more than one hydrogen.
o Hydroxide is named immediately after the names of any positive ions.
+ The hydroxide is commonly placed in parenthesis.
material safety data sheets
Examples of Salts:
CaCl2 - calcium chloride
K2SO4 - potassium sulfate
NaHC2O4 - sodium hydrogen oxalate
NaHS - sodium hydrogen sulfide
NaH2PO4 - sodium dihydrogen phosphate
Sn(OH)NO3 - tin (II) hydroxide nitrate
Neutralization: the reaction of a base and an acid to produce a salt and water.
sodium hydroxide + hydrochloric acid yields sodium chloride + water
While the reaction shown here usually comes to mind when salt production is mentioned, there are many reactions that produce salts. It is even possible to have salts that do not produce neutral solutions.
Salts can also be formed by the reaction of an acidic or basic anhydride with a corresponding base, acid, or anhydride.
* acidic anhydride + base salt
SO3 + 2NaOH Na2SO4 + H2O
* basic anhydride + acid salt
Na2O + H2SO4 Na2SO4 + H2O
* basic anhydride + acidic anhydride salt
Na2O + SO3 Na2SO4
Certain acids and bases react to produce only a partial neutralization. These reactions produce either acidic salts or basic salts.
* This reaction produces an acidic salt:
H2SO4 (aq) + NaOH (aq) NaHSO4 (aq) + H2O (l)
Sodium hydrogen sulfate is an acidic salt because it still contains an ionizable hydrogen atom.
Naming salts:
the name of a salt is related to the name of the acid that forms it.
* Binary acids produce salts ending with ide.
* Ternary acids ending in ic produce salts ending with ate.
* Ternary acids ending in ous produce salts ending with ite.
* Any prefixes in the ternary acid remain in the salt name.
* In naming acidic and basic salts, each ion in the salt is named separately.
o Hydrogen is named immediately before the names of any negative ions.
+ A prefix is used to indicate more than one hydrogen.
o Hydroxide is named immediately after the names of any positive ions.
+ The hydroxide is commonly placed in parenthesis.
material safety data sheets
Examples of Salts:
CaCl2 - calcium chloride
K2SO4 - potassium sulfate
NaHC2O4 - sodium hydrogen oxalate
NaHS - sodium hydrogen sulfide
NaH2PO4 - sodium dihydrogen phosphate
Sn(OH)NO3 - tin (II) hydroxide nitrate
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