Introduction Welcome to the virtual lab simulation of a common qualitative analysis lab. The goal of this lab will be to identify several unknown chemicals.

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Presentation transcript:

Introduction Welcome to the virtual lab simulation of a common qualitative analysis lab. The goal of this lab will be to identify several unknown chemicals based on their reactive properties with other chemicals. In this first part of 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 that are formed and also the precipitates that you observe. Keep in 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 Pb 2+ Ba 2+ Ag + Cu 2+ Co 2+ Fe 3+ Mg 2+ Na 2+ Li+ NO 3 - SO 4 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 +, Hg 2 2+, Pb 2+ Hydroxides – Insoluble; Exceptions: Alkali Metals, Ba 2+ Sulfates – Soluble; Exceptions: Ba 2+, Pb 2+, 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. here Click here to show animation

BariumYellow-Green SodiumYellow CopperBlue-Green LithiumRed LeadPale Blue Flame Test Color Reference

Problem Solving Strategy You 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. Incorrect: Google is a very handy tool, but it is much better to use your own chemical knowledge. Click close to try again X CloseIncorrect: Not all of the reactions in this lab will form precipitates. Refer to the solubility rules. Click close to try again X Close 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 Fe 3+ b.)Li + and Na + c.) Ba 2+, Ag + Incorrect: Fe 3+ will form a precipitate Click close to try again X Close Incorrect: Ba 2+ 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 Close Incorrect: 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 Close Incorrect: 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 dont forget to keep good notes of all of the reactive properties you observe.

Mg(NO 3 ) 2 NaSO 4 CuSO 4 Fe(NO 3 ) 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. AgNO 3 Pb(NO 3 ) 2 LiOHBaCl 2 CoSO 4 Flame test

AgNO 3 Pb(NO 3 ) 2 LiOHBaCl 2 CoSO 4 Mg(NO 3 ) 2 NaSO 4 CuSO 4 Fe(NO 3 ) 3 Choose which chemical you want to mix with Fe(NO 3 ) 3 and click on it to see the results. Click back to return to main selection page

Fe(NO 3 ) 3 AgNO 3 Yield: brownish/red solution; no precipitate Click back to return to selection page

Fe(NO 3 ) 3 Pb(NO 3 ) 2 Yield: brownish/red solution; no precipitate Click back to return to selection page

Fe(NO 3 ) 3 BaCl 2 Yield: brownish/red solution; no precipitate Click back to return to selection page

Fe(NO 3 ) 3 CoSO 4 Yield: salmon solution; no precipitate Click back to return to selection page

Fe(NO 3 ) 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(NO 3 ) 3 Mg(NO 3 ) 2 Yield: brownish/red solution; no precipitate Click back to return to selection page

Fe(NO 3 ) 3 NaSO 4 Yield: brownish/red solution; no precipitate Click back to return to selection page

Fe(NO 3 ) 3 AlCl 3 Yield: brownish/red solution; no precipitate Click back to return to selection page

Fe(NO 3 ) 3 CuSO 4 Yield: brown solution; no precipitate Click back to return to selection page

AgNO 3 Pb(NO 3 ) 2 LiOHBaCl 2 CoSO 4 Mg(NO 3 ) 2 NaSO 4 Fe(NO 3 ) 3 CuSO 4 Choose which chemical you want to mix with CuSO 4 and click on it to see the results. Click back to return to main selection page

CuSO 4 AgNO 3 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

CuSO 4 Pb(NO 3 ) 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

CuSO 4 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

CuSO 4 BaCl 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

CuSO 4 CoSO 4 Yield: purple solution; no precipitate Click back to return to selection page

CuSO 4 Mg(NO 3 ) 2 Yield: blue solution; no precipitate Click back to return to selection page

CuSO 4 NaSO 4 Yield: blue solution; no precipitate Click back to return to selection page

CuSO 4 AlCl 3 Yield: blue solution; no precipitate Click back to return to selection page

CuSO 4 Fe(NO 3 ) 3 Yield: brown solution; no precipitate Click back to return to selection page

AgNO 3 Pb(NO 3 ) 2 LiOHBaCl 2 CoSO 4 Mg(NO 3 ) 2 CuSO 4 Fe(NO 3 ) 3 NaSO 4 Choose which chemical you want to mix with NaSO 4 and click on it to see the results. Click back to return to main selection page

Na(SO 4 ) AgNO 3 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(SO 4 ) Pb(NO 3 ) 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(SO 4 ) LiOH Yield: clear solution; no precipitate Click back to return to selection page

Na(SO 4 ) BaCl 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(SO 4 ) CoSO 4 Yield: pink solution; no precipitate Click back to return to selection page

Na(SO 4 ) Mg(NO 3 ) 2 Yield: clear solution; no precipitate Click back to return to selection page

Na(SO 4 ) AlCl 3 Yield: clear solution; no precipitate Click back to return to selection page

Na(SO 4 ) CuSO 4 Yield: blue solution; no precipitate Click back to return to selection page

Na(SO 4 ) Fe(NO 3 ) 3 Yield: brownish red solution; no precipitate Click back to return to selection page

AgNO 3 Pb(NO 3 ) 2 LiOHBaCl 2 CoSO 4 NaSO 4 CuSO 4 Fe(NO 3 ) 3 Mg(NO 3 ) 2 Choose which chemical you want to mix with Mg(NO 3 ) 2 and click on it to see the results. Click back to return to main selection page

Mg(NO 3 ) 2 AgNO 3 Yield: clear solution; no precipitate Click back to return to selection page

Mg(NO 3 ) 2 Pb(NO 3 ) 2 Yield: clear solution; no precipitate Click back to return to selection page

Mg(NO 3 ) 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(NO 3 ) 2 BaCl 2 Yield: clear solution; no precipitate Click back to return to selection page

CoSO 4 Yield: pink solution; no precipitate Click back to return to selection page Mg(NO 3 ) 2

NaSO 4 Yield: clear solution; no precipitate Click back to return to selection page

Mg(NO 3 ) 2 AlCl 3 Yield: clear solution; no precipitate Click back to return to selection page

CuSO 4 Yield: blue solution; no precipitate Click back to return to selection page Mg(NO 3 ) 2

Fe(NO 3 ) 3 Yield: brownish/red solution; no precipitate Click back to return to selection page Mg(NO 3 ) 2

AgNO 3 Pb(NO 3 ) 2 LiOHBaCl 2 Mg(NO 3 ) 2 NaSO 4 CuSO 4 Fe(NO 3 ) 3 CoSO 4 Choose which chemical you want to mix with CoSO 4 and click on it to see the results. Click back to return to main selection page

CoSO 4 AgNO 3 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

CoSO 4 Pb(NO 3 ) 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

CoSO 4 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

CoSO 4 BaCl 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

CoSO 4 Mg(NO 3 ) 2 Yield: light pink solution; no precipitate Click back to return to selection page

CoSO 4 NaSO 4 Yield: light pink solution; no precipitate Click back to return to selection page

CoSO 4 AlCl 3 Yield: light pink solution; no precipitate Click back to return to selection page

CoSO 4 CuSO 4 Yield: purple solution; no precipitate Click back to return to selection page

CoSO 4 Fe(NO 3 ) 3 Yield: salmon colored solution; no precipitate Click back to return to selection page

AgNO 3 Pb(NO 3 ) 2 LiOHCoSO 4 Mg(NO 3 ) 2 NaSO 4 CuSO 4 Fe(NO 3 ) 3 BaCl 2 Choose which chemical you want to mix with ZnCl 2 and click on it to see the results. Click back to return to main selection page

AgNO 3 Yield: clear solution; white precipitate Click back to return to selection page BaCl 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

Pb(NO 3 ) 2 Yield: clear solution; white precipitate Click back to return to selection page BaCl 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

LiOH Yield: clear solution; white precipitate Click back to return to selection page BaCl 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

CoSO 4 Yield: light pink solution; white precipitate Click back to return to selection page BaCl 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(NO 3 ) 2 Yield: clear solution; no precipitate Click back to return to selection page BaCl 2

NaSO 4 Yield: clear solution; white precipitate Click back to return to selection page BaCl 2 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

AlCl 3 Yield: clear solution; no precipitate Click back to return to selection page BaCl 2

CuSO 4 Yield: blue solution; white precipitate Click back to return to selection page BaCl 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(NO 3 ) 3 Yield: brownish/red solution; no precipitate Click back to return to selection page BaCl 2

AgNO 3 Pb(NO 3 ) 2 BaCl 2 CoSO 4 Mg(NO 3 ) 2 NaSO 4 CuSO 4 Fe(NO 3 ) 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 AgNO 3 Yield: clear solution; black/brown precipitate Click back to return to selection page

LiOH Pb(NO 3 ) 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

BaCl 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

CoSO 4 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(NO 3 ) 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

NaSO 4 Yield: clear solution; no precipitate Click back to return to selection page LiOH

AlCl 3 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

CuSO 4 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(NO 3 ) 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

AgNO 3 LiOHBaCl 2 CoSO 4 Mg(NO 3 ) 2 NaSO 4 CuSO 4 Fe(NO 3 ) 3 Pb(NO 3 ) 2 Choose which chemical you want to mix with Pb(NO 3 ) 2 and click on it to see the results. Click back to return to main selection page

AgNO 3 Yield: clear solution; no precipitate Click back to return to selection page Pb(NO 3 ) 2

LiOH Yield: clear solution; white precipitate Click back to return to selection page Pb(NO 3 ) 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

BaCl 2 Yield: clear solution; white precipitate Click back to return to selection page Pb(NO 3 ) 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

CoSO 4 Yield: light pink solution; white precipitate Click back to return to selection page Pb(NO 3 ) 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(NO 3 ) 2 Yield: clear solution; no precipitate Click back to return to selection page Pb(NO 3 ) 2

NaSO 4 Yield: clear solution; white precipitate Click back to return to selection page Pb(NO 3 ) 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

AlCl 3 Yield: clear solution; white precipitate Click back to return to selection page Pb(NO 3 ) 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

CuSO 4 Yield: blue solution; white precipitate Click back to return to selection page Pb(NO 3 ) 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(NO 3 ) 3 Yield: brownish/red solution; no precipitate Click back to return to selection page Pb(NO 3 ) 2

Pb(NO 3 ) 2 LiOHBaCl 2 CoSO 4 Mg(NO 3 ) 2 NaSO 4 CuSO 4 Fe(NO 3 ) 3 AgNO 3 Choose which chemical you want to mix with AgNO 3 and click on it to see the results. Click back to return to main selection page

Pb(NO 3 ) 2 Yield: clear solution; no precipitate Click back to return to selection page Ag(NO 3 )

LiOH Yield: clear solution; black/brown precipitate Click back to return to selection page Ag(NO 3 )

BaCl 2 Yield: clear solution; white precipitate Click back to return to selection page Ag(NO 3 ) 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

CoCl 2 Yield: light pink solution; white precipitate Click back to return to selection page Ag(NO 3 ) 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(NO 3 ) 2 Yield: clear solution; no precipitate Click back to return to selection page Ag(NO 3 )

NaSO 4 Yield: clear solution; white precipitate Click back to return to selection page Ag(NO 3 ) 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

AlCl 3 Yield: clear solution; white precipitate Click back to return to selection page Ag(NO 3 ) 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

CuSO 4 Yield: blue solution; white precipitate Click back to return to selection page Ag(NO 3 ) 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(NO 3 ) 3 Yield: brownish/red solution; no precipitate Click back to return to selection page Ag(NO 3 )