silver

[Nisus]

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

[Detox]

Huh? :s

[Victimized]

Umm... whats the thread actually about?

[Chopin.FF]

Huh? :s

lmao at detox hahaha

[Vitality]

Lol sounds easy :p