GCSE Chemistry Required Practical: Identifying Unknown Compounds - Revision history

NRJC: /* Carbonate Test */

2020-01-19T19:03:17Z

‎Carbonate Test

NRJC: /* Sulphate Test */

2020-01-19T19:02:42Z

‎Sulphate Test

NRJC: /* Sulphate Test */

2020-01-19T19:02:22Z

‎Sulphate Test

NRJC: /* Sulphate Test */

2020-01-19T19:02:11Z

‎Sulphate Test

NRJC: /* Halide Test */

2020-01-19T19:01:57Z

‎Halide Test

NRJC: /* Halide Test */

2020-01-19T19:01:44Z

‎Halide Test

NRJC: /* Halide Test */

2020-01-19T19:01:23Z

‎Halide Test

NRJC at 11:32, 13 April 2019

2019-04-13T11:32:28Z

NRJC at 12:18, 29 January 2019

2019-01-29T12:18:14Z

NRJC: Created page with "==Key Stage 4== ===Meaning=== Use a variety of chemical tests to identify the ions in ionic compounds. ===Method=== ====Flame Test==== #Dip the end..."

2019-01-29T11:56:35Z

Created page with "==Key Stage 4== ===Meaning=== Use a variety of chemical tests to identify the ions in ionic compounds. ===Method=== ====Flame Test==== #Dip the end..."

New page

==Key Stage 4==
===Meaning===
Use a variety of [[chemical]] tests to identify the [[ion]]s in [[Ionic Compound|ionic compounds]].

===Method===
====Flame Test====
#Dip the end of an [[Inoculation Loop]] into [[concentration|concentrated]] [[Hydrochloric Acid]].
#Place the end of the [[Inoculation Loop]] into the powdered [[Metal Compound|metal compound]].
#Hold the end of the [[Inoculation Loop]] in a roaring blue [[Bunsen Burner]] flame.
#Observe and record the colour of the flame.
#Use the following table to identify the [[metal]] [[ion]].
{| class="wikitable"
|-
| style="height:20px; width:200px; text-align:center;" |'''Metal Ion'''
| style="height:20px; width:200px; text-align:center;" |'''Flame Colour'''
|-
| style="height:20px; width:200px; text-align:center;" |Lithium
| style="height:20px; width:200px; text-align:center;" |Red
|-
| style="height:20px; width:200px; text-align:center;" |Sodium
| style="height:20px; width:200px; text-align:center;" |Orange
|-
| style="height:20px; width:200px; text-align:center;" |Potassium
| style="height:20px; width:200px; text-align:center;" |Lilac (Purple)
|-
| style="height:20px; width:200px; text-align:center;" |Calcium
| style="height:20px; width:200px; text-align:center;" |Orange-red
|-
| style="height:20px; width:200px; text-align:center;" |Barium
| style="height:20px; width:200px; text-align:center;" |Brown-green
|-
| style="height:20px; width:200px; text-align:center;" |Copper
| style="height:20px; width:200px; text-align:center;" |Green-blue
|-
| style="height:20px; width:200px; text-align:center;" |Lead
| style="height:20px; width:200px; text-align:center;" |Blue
|}

@@ Line 73: / Line 73: @@
 #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>
+<math>Na2CO3(aq) + 2HCl(aq) \rightarrow 2NaCl(aq) + H2O(l) + CO2(g)</math>
 : A [[gas]] is [[product|produced]] and bubbled through [[Limewater]].
-<chem>CO2(g) + CaO(aq) -> CaCO3(s)</chem>
+<math>CO2(g) + CaO(aq) \rightarrow CaCO3(s)</math>
 : 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]].

@@ Line 62: / Line 62: @@
 #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
+#If a [[Sulphate]] is present a white [[precipitate]] is formed.
 <math>Na2SO4(aq) + BaCl2(aq) \rightarrow 2NaCl(aq) + BaSO4(s)</math>
 ====Carbonate Test====

@@ Line 62: / Line 62: @@
 #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:
+#If a [[Sulphate]] is present
 <math>Na2SO4(aq) + BaCl2(aq) \rightarrow 2NaCl(aq) + BaSO4(s)</math>
 : a white [[precipitate]] is formed.

@@ Line 63: / Line 63: @@
 #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>
+<math>Na2SO4(aq) + BaCl2(aq) \rightarrow 2NaCl(aq) + BaSO4(s)</math>
 : a white [[precipitate]] is formed.

@@ Line 49: / Line 49: @@
 <math>NaCl(aq) + AgNO3(aq) \rightarrow NaNO3(aq) + AgCl(s)</math>
 : A white [[precipitate]] is formed.
-<math>NaBr(aq) + AgNO3(aq) -> NaNO3(aq) + AgBr(s)</math>
+<math>NaBr(aq) + AgNO3(aq) \rightarrow NaNO3(aq) + AgBr(s)</math>
 : A cream coloured [[precipitate]] is formed.
-<math>NaI(aq) + AgNO3(aq) -> NaNO3(aq) + AgI(s)</math>
+<math>NaI(aq) + AgNO3(aq) \rightarrow NaNO3(aq) + AgI(s)</math>
 : A yellow [[precipitate]] is formed.

@@ Line 47: / Line 47: @@
 #Add the [[Silver Nitrate]] to the [[Test Tube|test tube]].
 #Use the following information to identify the [[Halide]] present.
-<math>NaCl(aq) + AgNO3(aq) -> NaNO3(aq) + AgCl(s)</math>
+<math>NaCl(aq) + AgNO3(aq) \rightarrow NaNO3(aq) + AgCl(s)</math>
 : A white [[precipitate]] is formed.
 <math>NaBr(aq) + AgNO3(aq) -> NaNO3(aq) + AgBr(s)</math>

@@ Line 1: / Line 1: @@
 ==Key Stage 4==
 ===Meaning===
 Use a variety of [[chemical]] tests to identify the [[ion]]s in [[Ionic Compound|ionic compounds]].

← Older revision		Revision as of 12:18, 29 January 2019
Line 36:		Line 36:
	\| style="height:20px; width:200px; text-align:center;" \|Blue		\| style="height:20px; width:200px; text-align:center;" \|Blue
	\|}		\|}
		+
		+	====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]].