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| style="height:20px; width:200px; text-align:center;" |Blue
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====Halide Test====
The test for [[Halide]] [[anion]]s begins by adding dilute [[Nitric Acid]] to remove any possible [[Carbonate]]s. Then [[Silver Nitrate]] is added to form a [[precipitate]] of [[Silver Halide]].
#Add four [[spatula]]s of [[Sodium Halide]] to a 50ml beaker with 40ml [[water]] and stir with a [[Glass Rod|glass rod]] to [[dissolve]].
#Measure roughly 2ml of [[Sodium Halide]] [[solution]] using a [[pipette]].
#Add the [[solution]] to a [[Test Tube|test tube]].
#Add 4 drops of 0.4[[Molarity|M]] [[Nitric Acid]] to remove any [[Carbonate]]s.
#Measure roughly 2ml 0.05[[Molarity|M]] [[Silver Nitrate]] [[solution]] using a clean [[pipette]].
#Add the [[Silver Nitrate]] to the [[Test Tube|test tube]].
#Use the following information to identify the [[Halide]] present.
<chem>NaCl(aq) + AgNO3(aq) -> NaNO3(aq) + AgCl(s)</chem>
: A white [[precipitate]] is formed.
<chem>NaBr(aq) + AgNO3(aq) -> NaNO3(aq) + AgBr(s)</chem>
: A cream coloured [[precipitate]] is formed.
<chem>NaI(aq) + AgNO3(aq) -> NaNO3(aq) + AgI(s)</chem>
: A yellow [[precipitate]] is formed.
====Sulphate Test====
The test for [[Sulphate]] [[anion]]s begins by adding dilute [[Hydrochloric Acid]] to remove any possible [[Carbonate]]s. Then [[Barium Chloride]] is added to form a [[precipitate]] of [[Barium Sulphate]].
#Add four [[spatula]]s of [[Metal Sulphate]] to a 50ml beaker with 40ml [[water]] and stir with a [[Glass Rod|glass rod]] to [[dissolve]].
#Measure roughly 2ml of [[Metal Sulphate]] [[solution]] using a [[pipette]].
#Add the [[solution]] to a [[Test Tube|test tube]].
#Add 4 drops of 0.4[[Molarity|M]] [[Hydrochloric Acid]] to remove any [[Carbonate]]s.
#Measure roughly 2ml 0.1[[Molarity|M]] [[Barium Chloride]] [[solution]] using a clean [[pipette]].
#Add the [[Barium Chloride]] [[solution]] to the [[Test Tube|test tube]].
#If a [[Sulphate]] is present:
<chem>Na2SO4(aq) + BaCl2(aq) -> 2NaCl(aq) + BaSO4(s)</chem>
: a white [[precipitate]] is formed.
====Carbonate Test====
The test for [[carbonate]] [[anion]]s begins by adding [[Hydrochloric Acid]] to the [[solution]]. This [[product|produces]] a [[gas]] which is collected and bubbled through [[Limewater]] to identify if [[Carbon Dioxide]] has been [[product|produced]]. If [[Carbon Dioxide]] has been [[product|produced]] then the [[Limewater]] will turn from [[transparent]] to cloudy.
#Add two [[spatula]]s of [[Metal Carbonate]] [[solution]] to a [[Test Tube|test tube]].
#Measure roughly 2ml of [[Limewater]] [[solution]] using a [[pipette]].
#Add the [[Limewater]] to a second [[Test Tube|test tube]].
#Measure 2ml 0.4[[Molarity|M]] [[Hydrochloric Acid]] [[solution]] using a clean [[pipette]].
#Add the [[Hydrochloric Acid]] [[solution]] to the first [[Test Tube|test tube]] containing the [[Metal Carbonate]] [[Solution]].
#Immediately attach a [[bung]] with a [[Delivery Tube|delivery tube]] to pass the [[gas]] through the [[Limewater]] in the second [[Test Tube|test tube]].
<chem>Na2CO3(aq) + 2HCl(aq) -> 2NaCl(aq) + H2O(l) + CO2(g)</chem>
: A [[gas]] is [[product|produced]] and bubbled through [[Limewater]].
<chem>CO2(g) + CaO(aq) -> CaCO3(s)</chem>
: The [[Calcium Carbonate]] makes the [[Limewater]] appear cloudy.
====Unknown Compound Test====
To identify an unknown [[Ionic Compound|ionic compound]] use each [[experiment]] mentioned above and record the [[results]] to compare with the expected [[results]] for each [[Metal Compound]].