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Data and Observations
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Data Table 1
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Sample KCl NaCl BaCl2 AlCl3 Unknown Trial 1 drops of AgNO3 Trial 2 drops of AgNO3 Average drops of AgNO3 Cation/anion ratio
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Chemistry: Matter and Change 11
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Laboratory Manual
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Copyright Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc
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dry test tube 2 Add 2 drops of dichlorofluoroscein indicator solution to the test tube 3 Add silver nitrate drop by drop to the solution until the dichlorofluoroscein turns from white to pink Hold the dropper vertically as you add the drops Carefully shake the tube from side to side as the drops are being added Do not spill any solution 4 Count and record in Data Table 1 the number of drops needed to turn the solution from white to pink
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1 Pour any materials containing silver into a
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container provided by your teacher 2 Return all lab equipment to its proper place 3 Report any broken or damaged equipment 4 Wash your hands thoroughly before leaving the lab
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Name
Date
Class
LAB 112
LABORATORY MANUAL
Analyze and Conclude
1 Using Numbers Calculate the average number of drops of AgNO3 used for each
solution Record these numbers in Data Table 1
2 Using Numbers Assume that the cation-anion ratio is 1:1 for KCl All the solutions are
the same concentration, which means that they all contain the same number of moles of ionic compound per liter of solution Using this information and your results, calculate the cation to anion ratio for each of the known solutions Record these ratios in Data Table 1
3 Comparing How do your answers in question 2 compare with the ratios you predicted in
your hypothesis using the formulas for the compounds
4 Inferring Why must all the solutions being tested be the same concentration
5 Making Predictions Assume you did not know the concentration of the silver nitrate
solution How would this unknown concentration compare with the concentration of the KCl solution if half as much AgNO3 solution as KCl solution was used
Copyright Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc
6 Drawing Conclusions Summarize how the results of this laboratory activity relate to the
formulas of the compounds tested
7 Error Analysis What could you have done to improve the precision of the
measurements
Real-World Chemistry
1 Body fluids are often tested in medical facili2 Silver is a valuable metal Explain how you
ties to determine the concentrations of certain substances How could the techniques used in this lab activity be applied to such testing
could separate any dissolved Ag ions from the solutions you disposed of in the discard beaker
Laboratory Manual
Chemistry: Matter and Change 11
Name
Date
Class
LABORATORY MANUAL
Use with Section 123
Observing a Limiting Reactant
hen two substances react, they react in exact amounts You can determine what amounts of the two reactants are needed to react completely with each other by means of mole ratios based on the balanced chemical equation for the reaction In the laboratory, precise amounts of the reactants are rarely used in a reaction Usually, there is an excess of one of the reactants As soon as the other reactant is used up, the reaction stops The reactant that is used up is called the limiting reactant Based on the quantities of each reactant and the balanced chemical equation, you can predict which substance in a reaction is the limiting reactant
Problem
How can the mole concept be used to predict the limiting reactant in a chemical reaction
Objectives
Calculate the number of moles of each reactant Write a balanced chemical equation for the reaction of hydrochloric acid and magnesium Predict, using the balanced chemical equation, which substance will be the limiting reactant Compare the actual results with your predicted results
Materials
dropper bottle containing 6M HCl magnesium ribbon (2 pieces, 3 5 cm each) test-tube rack 20 150-mm test tube test-tube holder
Copyright Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc
Safety Precautions
Always wear safety goggles, a lab apron, and gloves Point open end of test tube away from your face and away from others Do not inhale released vapors Handle acids carefully Do not use open flames in the lab Hydrogen gas is flammable
Pre-Lab
1 Magnesium and hydrochloric acid react to form 3 Based on the chemical equation and your calcula-
magnesium chloride and hydrogen gas Write the balanced chemical reaction for the reaction 2 Calculate a the number of moles of magnesium in 50 g of magnesium b the number of moles of hydrochloric acid in 10 mL of 60M HCl; 60M HCl contains 6 moles of HCl per liter of solution
tions, what would be left over if these amounts of magnesium and hydrochloric acid were combined What would be used up 4 Describe the term limiting reactant in your own words 5 Read the entire laboratory activity Form a hypothesis about which reactant will be the limiting reactant at steps 5, 6, and 7 in the experiment Record your hypothesis on page 90
Chemistry: Matter and Change 12
Laboratory Manual
Name
Date
Class
LAB 121
LABORATORY MANUAL
7 Now begin adding 6M HCl one drop of at a time,
Procedure
1 Obtain two pieces of magnesium ribbon that are 2
4 5
3 5 cm long Determine and record the mass of the first piece of magnesium Set the second piece aside to use in step 8 In the data table, record your observations of the color, length, and texture of your piece of magnesium Bend the piece of magnesium several times and put it into the test tube Place the test tube containing the magnesium in a test-tube rack and add ten drops of 6M HCl Record in Data Table 1 any observations during and immediately following the reaction CAUTION: Do not inhale vapors or look down into test tube Observe the reaction from the side of the test tube After the reaction has stopped, add another ten drops of 6M HCl to the test tube Record any observations during and immediately following the reaction
watching the reaction and recording observations after each drop has stopped reacting Stop adding drops of hydrochloric acid when all of the magnesium ribbon in the test tube has reacted 8 Place the second piece of magnesium ribbon into the test tube and record your observations
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