Nisus
21-09-2005, 09:28 AM
Preparing Silver Chloride By Precipitation
The Aim.
I had to do an experiment that had to produce an insoluble salt and silver chloride by precipitation.
The Safety Points.
The safety points that we had to obey by was -
à Safety glasses
à Clearing up spilled chemicals
à Standing up
à Chairs under the tables
à Clean droppers
à Only mixing the chemicals you are told to.
à Tie all long hair back
à Don’t run in the science lab
à No shouting
The Equipment List.
In my equipment list there are as followed –
à 10cm3 and 25cm3 measuring cylinders
à Clean beakers
à Silver nitrate solution
à Sodium chloride or dilute hydrochloric acid
à Stirring rod
à Filter paper
à Filter funnel
à Labels
à Balance
à Distilled water
à Conical flask
The Method.
This is what I had to do in the experiment –
à I had to carefully measure out 10cm3 of 0.1M silver nitrate using a 10cm3 measuring cylinder and a dropper
à Then I had to carefully pour the silver nitrate into a clean beaker
à After that I had to measure out 20cm3 of dilute hydrochloric acid using a 50cm3 measuring cylinder
à I had to pour the acid into a second clean beaker
à Then slowly added about 10cm3 of the dilute hydrochloric acid into the beaker containing the silver nitrate
à Then slowly stirred the solution
à And slowly added the remaining acid
à I labelled a piece of filter paper with my name
à I measured the mass of the filter paper
à I gradually filtered the solution using a funnel and conical flask
à I had to wash the precipitate with water to remove any unreacted silver nitrate and hydrochloric acid and to remove any other impurities
à Then I put the conical flask to one side
à Then I had to put the filter paper on a tray to dry
à Once it was dry I had to record the mass of the filter paper and silver chloride
à I had to record the actual yield of silver chloride obtained.
The Results.
AgNO3 (aq) +NaCL (aq) à NaNO3 (aq) +Agcl(s)
1 mole of AqNO3 is required to produce 1 mole of AgCL.
108 +14 (3x16)g AgNO3 is required to produce 108+35.5g AgCL.
170g AgNO3 is required to produce 143.5g AgCL.
1000cm3 solution contains 170g AgNO3
10cm3 of a 1 molar soln of silver chloride contains 1.7g AgNO3
1.7g of silver nitrate was used
Theoretical yield = 1.7x 143.5 = g
170
Theoretical yield =1.44g
(Mass of AgCL from experiment)
Actual yield = 0.65g
Percentage yield = actual yield x100
Theoretical yield
= 0.65 x100
1.449
=45.1%
The Evaluation.
In the experiment that I have done I could have done things wrong which I might not have even know like:
à Measured out the chemicals wrongly
à Accidentally mixed the mixtures
à Could of dropped hair in the solution or something
à I could have dropped the chemicals
à Tipped the chemicals
à Could of left something in the solution that wasn’t ment to be in there
à Could of got the wrong reading on the scales
à The equipment might not of been easy to use so I might of used them wrong
The Vocational Aspect
The Aim.
I had to do an experiment that had to produce an insoluble salt and silver chloride by precipitation.
The Safety Points.
The safety points that we had to obey by was -
à Safety glasses
à Clearing up spilled chemicals
à Standing up
à Chairs under the tables
à Clean droppers
à Only mixing the chemicals you are told to.
à Tie all long hair back
à Don’t run in the science lab
à No shouting
The Equipment List.
In my equipment list there are as followed –
à 10cm3 and 25cm3 measuring cylinders
à Clean beakers
à Silver nitrate solution
à Sodium chloride or dilute hydrochloric acid
à Stirring rod
à Filter paper
à Filter funnel
à Labels
à Balance
à Distilled water
à Conical flask
The Method.
This is what I had to do in the experiment –
à I had to carefully measure out 10cm3 of 0.1M silver nitrate using a 10cm3 measuring cylinder and a dropper
à Then I had to carefully pour the silver nitrate into a clean beaker
à After that I had to measure out 20cm3 of dilute hydrochloric acid using a 50cm3 measuring cylinder
à I had to pour the acid into a second clean beaker
à Then slowly added about 10cm3 of the dilute hydrochloric acid into the beaker containing the silver nitrate
à Then slowly stirred the solution
à And slowly added the remaining acid
à I labelled a piece of filter paper with my name
à I measured the mass of the filter paper
à I gradually filtered the solution using a funnel and conical flask
à I had to wash the precipitate with water to remove any unreacted silver nitrate and hydrochloric acid and to remove any other impurities
à Then I put the conical flask to one side
à Then I had to put the filter paper on a tray to dry
à Once it was dry I had to record the mass of the filter paper and silver chloride
à I had to record the actual yield of silver chloride obtained.
The Results.
AgNO3 (aq) +NaCL (aq) à NaNO3 (aq) +Agcl(s)
1 mole of AqNO3 is required to produce 1 mole of AgCL.
108 +14 (3x16)g AgNO3 is required to produce 108+35.5g AgCL.
170g AgNO3 is required to produce 143.5g AgCL.
1000cm3 solution contains 170g AgNO3
10cm3 of a 1 molar soln of silver chloride contains 1.7g AgNO3
1.7g of silver nitrate was used
Theoretical yield = 1.7x 143.5 = g
170
Theoretical yield =1.44g
(Mass of AgCL from experiment)
Actual yield = 0.65g
Percentage yield = actual yield x100
Theoretical yield
= 0.65 x100
1.449
=45.1%
The Evaluation.
In the experiment that I have done I could have done things wrong which I might not have even know like:
à Measured out the chemicals wrongly
à Accidentally mixed the mixtures
à Could of dropped hair in the solution or something
à I could have dropped the chemicals
à Tipped the chemicals
à Could of left something in the solution that wasn’t ment to be in there
à Could of got the wrong reading on the scales
à The equipment might not of been easy to use so I might of used them wrong
The Vocational Aspect