introduction welcome to the virtual lab simulation of a common qualitative analysis lab. the goal of...
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IntroductionWelcome to the virtual lab simulation of a common
qualitative analysis lab. The goal of this lab will be toidentify several unknown chemicals based on their
reactive properties with other chemicals. In this first partof the lab you will observe what happens when you
mix a number of known chemicals together. You will then create a list of observations that will allow you to determine the identity of your unknown chemicals in the second portion
of the lab. Keep good notes on the color of the solutions thatare formed and also the precipitates that you observe. Keepin mind solubility rules and ion charges to create an accurate
picture of what is happening in each reaction.
Helpful Hints• If a precipitate forms, use the solubility rules to identify the
precipitate. You will be required to write out the total and net ionic equations for every precipitate that forms in both this and the next part of the lab.
• Remember that each of the chemicals that you are combining contain both a cation and an anion so you will end up with two new products. You must identify the complete compound (cation and anion) present in each unknown in the second part of the lab. Look at the animation below to understand what is happening when you react two compounds together. Using this general concept, you will be able to figure out what products are formed in each reaction.
++ - - Click here to show animation
Molecules involved
Pb2+
Ba2+Ag+Cu2+ Co2+
Fe3+Mg2+Na2+Li+
NO3- SO4
2- Cl- OH-
Every compound you will use will contain both an anion and a cation from those shown on this page. The solubility of each compound can be determined using the solubility rules on the next page. The colors of each ion will help you to identify them, the colors of the ions on this page correspond to the color of each ion in solution.
Solubility Rules
• Nitrates– Always Soluble
• Chlorides– Soluble; Exceptions: Ag+, Hg2
2+, Pb2+
• Hydroxides– Insoluble; Exceptions: Alkali Metals, Ba2+
• Sulfates– Soluble; Exceptions: Ba2+, Pb2+, Ag+
Below you will find solubility information for the chemicals that you will be using in this lab: Note: The solubility rules are far more complex and inclusive than what you are shown and can be found in your textbook on page 447.
Flame Tests
• One way in which we can identify the presence of a metal in a an unknown solution is by carrying out a flame test. – A loop made out of nichrome wire is used to collect a small
amount of the unknown. The wire is then inserted in a flame and the color of the flame is observed. The color of the flame can identify an element that is present. Click here to see a table of flame colors.
Click here to show animation
Barium Yellow-Green
Sodium Yellow
Copper Blue-Green
Lithium Red
Lead Pale Blue
Flame Test Color Reference
Problem Solving StrategyYou will need to develop an effective strategy to identify your unknowns. Answer
the following questions to demonstrate your understanding.
In the first part of the lab you should be able to predict whether a reaction between two products will produce a precipitate before you carry out the reaction. How will you know this?
a.) because I googled it
b.) because I looked at the solubility rules and determined the solubility of each of the new products formed
c.) because every combination of reactants in this experiment will result in a precipitate.
Correct:
The solubility rules will aid you in determining which reactions will form precipitates.
Click close to continue
X Close
Problem Solving Strategy You will need to develop an effective strategy to identify your unknowns. Answer
the following questions to demonstrate your understanding.
A compound containing OH- and any anion except _______ will produce a precipitate. Therefore, it will be easy to narrow down the identity of your unknown if it does not form a precipitate with a compound containing OH
a.)Li+ and Fe3+
b.)Li+ and Na+
c.) Ba2+, Ag+
Incorrect:
Fe3+ will form a precipitate
Click close to try again
X CloseIncorrect:
Ba2+ and Ag+ will form precipitates
Click close to try again
X CloseCorrect:
Per the solubility rules, the only cations that will not form a precipitate with OH- are Li+ and Na+
Click close to continue
X Close
Problem Solving Strategy You will need to develop an effective strategy to identify your unknowns. Answer
the following questions to demonstrate your understanding.
A flame test can be used to identify the presence of several different _______ by the color of the flame. Once you have done so, the solubility rules can be used to identify the _______.
a.) Cations, anion
b.) Anions, cation
c.) Solubility
Correct
Click close to continue
X CloseIncorrect:
This answer is incorrect, a flame test tells us nothing about the solubility of an unknown directly.
Click close to try again
X CloseIncorrect:
Incorrect, a flame test can be used in this experiment to identify cations
Click close to try again
X Close
Problem Solving Strategy You will need to develop an effective strategy to identify your unknowns. Answer the
following questions to demonstrate your understanding.
The presence of some compounds can be determined by the color of the solution. Which of the following compounds are correctly matched with their corresponding color in solution?a.) Iron- Red/Orange, Cobalt-Pink, Copper-Blue
b.) Iron- Red/Orange, Cobalt- blue, Copper-blue
c.) Barium-Yellow, Iron- Red/Orange, Cobalt-Pink
Correct
Click close to continue
X CloseIncorrect:
This answer is incorrect, Re-examine both Iron and Cobalt
Click close to try again
X CloseIncorrect:
Incorrect, take another look at barium
Click close to try again
X Close
Your Turn
• Now it is your turn to explore the reactive properties of the 9 different chemicals in this experiment. You may mix any combination of chemicals together as many times as you need to prepare yourself for the second portion of the lab. Use the problem solving strategies outlined previously and don’t forget to keep good notes of all of the reactive properties you observe.
Mg(NO3)2 NaSO4
CuSO4 Fe(NO3)3
Click on one of the above reagents to mix it with another reagent or click on the flame test button to see the results of a flame test using that solution. Keep
careful notes of what reagents you are mixing and the results of each reaction. You will use this information in the second part of this lab.
AgNO3 Pb(NO3)2 LiOH BaCl2 CoSO4
Flame test Flame test Flame test Flame test Flame test Flame test Flame test
Flame test Flame test
AgNO3 Pb(NO3)2 LiOH BaCl2 CoSO4 Mg(NO3)2 NaSO4 CuSO4
Fe(NO3)3
Choose which chemical you want to mix with Fe(NO3)3 and click on it to see the results.
Click back to return to main selection page
Fe(NO3)3
AgNO3
Yield: brownish/red solution; no precipitate
Click back to return to selection page
Fe(NO3)3
Pb(NO3)2
Yield: brownish/red solution; no precipitate
Click back to return to selection page
Fe(NO3)3
BaCl2
Yield: brownish/red solution; no precipitate
Click back to return to selection page
Fe(NO3)3
CoSO4
Yield: salmon solution; no precipitate
Click back to return to selection page
Fe(NO3)3
LiOH
Yield: clear solution; rust colored precipitate
Click back to return to selection page
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
Fe(NO3)3
Mg(NO3)2
Yield: brownish/red solution; no precipitate
Click back to return to selection page
Fe(NO3)3
NaSO4
Yield: brownish/red solution; no precipitate
Click back to return to selection page
Fe(NO3)3
AlCl3
Yield: brownish/red solution; no precipitate
Click back to return to selection page
Fe(NO3)3
CuSO4
Yield: brown solution; no precipitate
Click back to return to selection page
AgNO3 Pb(NO3)2 LiOH BaCl2 CoSO4 Mg(NO3)2 NaSO4 Fe(NO3)3
CuSO4
Choose which chemical you want to mix with CuSO4 and click on it to see the results.
Click back to return to main selection page
CuSO4
AgNO3
Yield: blue solution; white precipitate
Click back to return to selection page
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
CuSO4
Pb(NO3)2
Yield: blue solution; white precipitate
Click back to return to selection page
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
CuSO4
LiOH
Yield: clear solution; blue/green precipitate
Click back to return to selection page
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
CuSO4
BaCl2
Yield: blue solution; white precipitate
Click back to return to selection page
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
CuSO4
CoSO4
Yield: purple solution; no precipitate
Click back to return to selection page
CuSO4
Mg(NO3)2
Yield: blue solution; no precipitate
Click back to return to selection page
CuSO4
NaSO4
Yield: blue solution; no precipitate
Click back to return to selection page
CuSO4
AlCl3
Yield: blue solution; no precipitate
Click back to return to selection page
CuSO4
Fe(NO3)3
Yield: brown solution; no precipitate
Click back to return to selection page
AgNO3 Pb(NO3)2 LiOH BaCl2 CoSO4 Mg(NO3)2 CuSO4Fe(NO3)3
NaSO4
Choose which chemical you want to mix with NaSO4 and click on it to see the results.
Click back to return to main selection page
Na(SO4)
AgNO3
Yield: clear solution; white precipitate
Click back to return to selection page
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
Na(SO4)
Pb(NO3)2
Yield: clear solution; white precipitate
Click back to return to selection page
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
Na(SO4)
LiOH
Yield: clear solution; no precipitate
Click back to return to selection page
Na(SO4)
BaCl2
Yield: clear solution; white precipitate
Click back to return to selection page
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
Na(SO4)
CoSO4
Yield: pink solution; no precipitate
Click back to return to selection page
Na(SO4)
Mg(NO3)2
Yield: clear solution; no precipitate
Click back to return to selection page
Na(SO4)
AlCl3
Yield: clear solution; no precipitate
Click back to return to selection page
Na(SO4)
CuSO4
Yield: blue solution; no precipitate
Click back to return to selection page
Na(SO4)
Fe(NO3)3
Yield: brownish red solution; no precipitate
Click back to return to selection page
AgNO3 Pb(NO3)2 LiOH BaCl2 CoSO4 NaSO4 CuSO4Fe(NO3)3
Mg(NO3)2
Choose which chemical you want to mix with Mg(NO3)2 and click on it to see the results.
Click back to return to main selection page
Mg(NO3)2
AgNO3
Yield: clear solution; no precipitate
Click back to return to selection page
Mg(NO3)2
Pb(NO3)2
Yield: clear solution; no precipitate
Click back to return to selection page
Mg(NO3)2
LiOH
Yield: clear solution; white precipitate
Click back to return to selection page
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
Mg(NO3)2
BaCl2
Yield: clear solution; no precipitate
Click back to return to selection page
CoSO4
Yield: pink solution; no precipitate
Click back to return to selection page
Mg(NO3)2
Mg(NO3)2
NaSO4
Yield: clear solution; no precipitate
Click back to return to selection page
Mg(NO3)2
AlCl3
Yield: clear solution; no precipitate
Click back to return to selection page
CuSO4
Yield: blue solution; no precipitate
Click back to return to selection page
Mg(NO3)2
Fe(NO3)3
Yield: brownish/red solution; no precipitate
Click back to return to selection page
Mg(NO3)2
AgNO3 Pb(NO3)2 LiOH BaCl2Mg(NO3)2 NaSO4 CuSO4Fe(NO3)3
CoSO4
Choose which chemical you want to mix with CoSO4 and click on it to see the results.
Click back to return to main selection page
CoSO4
AgNO3
Yield: light pink solution; white precipitate
Click back to return to selection page
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
CoSO4
Pb(NO3)2
Yield: light pink solution; white precipitate
Click back to return to selection page
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
CoSO4
LiOH
Yield: clear solution; no precipitate
Click back to return to selection page
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
CoSO4
BaCl2
Yield: light pink solution; white precipitate
Click back to return to selection page
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
CoSO4
Mg(NO3)2
Yield: light pink solution; no precipitate
Click back to return to selection page
CoSO4
NaSO4
Yield: light pink solution; no precipitate
Click back to return to selection page
CoSO4
AlCl3
Yield: light pink solution; no precipitate
Click back to return to selection page
CoSO4
CuSO4
Yield: purple solution; no precipitate
Click back to return to selection page
CoSO4
Fe(NO3)3
Yield: salmon colored solution; no precipitate
Click back to return to selection page
AgNO3 Pb(NO3)2 LiOH CoSO4Mg(NO3)2 NaSO4 CuSO4Fe(NO3)3
BaCl2
Choose which chemical you want to mix with ZnCl2 and click on it to see the results.
Click back to return to main selection page
AgNO3
Yield: clear solution; white precipitate
Click back to return to selection page
BaCl2
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
Pb(NO3)2
Yield: clear solution; white precipitate
Click back to return to selection page
BaCl2
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
LiOH
Yield: clear solution; white precipitate
Click back to return to selection page
BaCl2
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
CoSO4
Yield: light pink solution; white precipitate
Click back to return to selection page
BaCl2
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
Mg(NO3)2
Yield: clear solution; no precipitate
Click back to return to selection page
BaCl2
NaSO4
Yield: clear solution; white precipitate
Click back to return to selection page
BaCl2
Woah! A precipitate has formed. Write the complete ionic equation of the reaction in your notebook. Be sure to pay attention to valence!
Click close to return
X Close
AlCl3
Yield: clear solution; no precipitate
Click back to return to selection page
BaCl2
CuSO4
Yield: blue solution; white precipitate
Click back to return to selection page
BaCl2
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
Fe(NO3)3
Yield: brownish/red solution; no precipitate
Click back to return to selection page
BaCl2
AgNO3 Pb(NO3)2 BaCl2 CoSO4Mg(NO3)2 NaSO4 CuSO4Fe(NO3)3
LiOH
Choose which chemical you want to mix with LiOH and click on it to see the results.
Click back to return to main selection page
LiOH
AgNO3
Yield: clear solution; black/brown precipitate
Click back to return to selection page
LiOH
Pb(NO3)2
Yield: clear solution; white precipitate
Click back to return to selection page
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
BaCl2
Yield: clear solution; white precipitate
Click back to return to selection page
LiOH
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
CoSO4
Yield: clear solution; rose/red precipitate
Click back to return to selection page
LiOH
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
Mg(NO3)2
Yield: clear solution; white precipitate
Click back to return to selection page
LiOH
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
NaSO4
Yield: clear solution; no precipitate
Click back to return to selection page
LiOH
AlCl3
Yield: clear solution; white precipitate
Click back to return to selection page
LiOH
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
CuSO4
Yield: clear solution; blue/green precipitate
Click back to return to selection page
LiOH
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
Fe(NO3)3
Yield: clear solution; rust colored precipitate
Click back to return to selection page
LiOH
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
AgNO3 LiOH BaCl2 CoSO4Mg(NO3)2 NaSO4 CuSO4Fe(NO3)3
Pb(NO3)2
Choose which chemical you want to mix with Pb(NO3)2 and click on it to see the results.
Click back to return to main selection page
AgNO3
Yield: clear solution; no precipitate
Click back to return to selection page
Pb(NO3)2
LiOH
Yield: clear solution; white precipitate
Click back to return to selection page
Pb(NO3)2
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
BaCl2
Yield: clear solution; white precipitate
Click back to return to selection page
Pb(NO3)2
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
CoSO4
Yield: light pink solution; white precipitate
Click back to return to selection page
Pb(NO3)2
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
Mg(NO3)2
Yield: clear solution; no precipitate
Click back to return to selection page
Pb(NO3)2
NaSO4
Yield: clear solution; white precipitate
Click back to return to selection page
Pb(NO3)2
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
AlCl3
Yield: clear solution; white precipitate
Click back to return to selection page
Pb(NO3)2
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
CuSO4
Yield: blue solution; white precipitate
Click back to return to selection page
Pb(NO3)2
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
Fe(NO3)3
Yield: brownish/red solution; no precipitate
Click back to return to selection page
Pb(NO3)2
Pb(NO3)2 LiOH BaCl2 CoSO4Mg(NO3)2 NaSO4 CuSO4Fe(NO3)3
AgNO3
Choose which chemical you want to mix with AgNO3 and click on it to see the results.
Click back to return to main selection page
Pb(NO3)2
Yield: clear solution; no precipitate
Click back to return to selection page
Ag(NO3)
LiOH
Yield: clear solution; black/brown precipitate
Click back to return to selection page
Ag(NO3)
BaCl2
Yield: clear solution; white precipitate
Click back to return to selection page
Ag(NO3)
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
CoCl2
Yield: light pink solution; white precipitate
Click back to return to selection page
Ag(NO3)
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
Mg(NO3)2
Yield: clear solution; no precipitate
Click back to return to selection page
Ag(NO3)
NaSO4
Yield: clear solution; white precipitate
Click back to return to selection page
Ag(NO3)
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
AlCl3
Yield: clear solution; white precipitate
Click back to return to selection page
Ag(NO3)
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
CuSO4
Yield: blue solution; white precipitate
Click back to return to selection page
Ag(NO3)
Woah! A precipitate has formed. Write the complete ionic equation and the net ionic equation of the reaction in your notebook. Be sure to pay attention to charges!
Click close to return
X Close
Fe(NO3)3
Yield: brownish/red solution; no precipitate
Click back to return to selection page
Ag(NO3)
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